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Green Synthesis of Trimetallic Nanoparticles using Flacourtia Indica (Burm.f.) Merr. Characterization and Applications

Summary Excerpt Details

Anthropogenic activities have led to environmental pollution by toxic heavy metals and dyes such as Congo red. Trimetallic nanoparticles can be used for enrichment heavy metals and photocatalytic degradation of Congo red from the environment. However, the processes used to synthesize nanoparticles can be hazardous to the environment. In the study, green synthesis of Phosphorous doped ZrO2CeO2ZnO nanoparticles were carried out using Flacourtia indica leaf aqueous extracts with phytochemicals as reducing agents. The nanoparticles were used as photocatalysts for degradation of Congo red dye and as sorbents for enrichment of selected toxic metals: lead, cadmium, arsenic and chromium. The influence of various parameters during the synthesis and solid phase extraction stages were investigated using Half, Full and Taguchi experimental designs. Interactions between factors were determined using ANOVA and response surface methodologies. The enrichment methods were validated by using spiked borehole, well, tap and effluent water samples. The P−ZrO2CeO2ZnO nanoparticles and P−ZrO2CeO2ZnO nanoparticles/alginate beads were characterized using Ultra Violet Visible spectrometry, Scanning Electron Microscope(SEM), Fourier Transform-Infra Red Spectroscopy, Transmitting Electron Microscopy (TEM), Brunauer Emmet Teller (BET) analysis, X-ray Photoelectron Spectroscopy (XPS) and X ray Diffraction (XRD). The most significant factors for P−ZrO2CeO2ZnO nanoparticle synthesis were pH, metal ion concentration and leaf extract concentration. The surface areas obtained under optimum synthesis conditions were 0.459 m2g−1 and 7.33 m2g−1for P−ZrO2CeO2ZnO nanoparticles and P−ZrO2CeO2ZnO nanoparticles/alginate beads respectively. The synthesized nanoparticles were crystalline and irregularly shaped The nanoparticles average size was 0.255 nm and the range of the size was from 0.1-4.51nm. Zn−O, Zr−O, C−O, O−H, functional groups were present in the nanoparticles from FTIR data. The optimum conditions for photocatalytic degradation of Congo red using P−ZrO2CeO2ZnO nanoparticles were 0.05 g/L catalyst dosage concentration, 10 mg/L Congo red concentration, 250 min irradiation time. The reaction followed pseudo first order kinetics with a rate constant of 0.069 min-1 and degradation efficiency of 85.85%.The reaction mechanism was explained by light, superoxide radicals and h+ holes. [...]

Excerpt


Table of contents

Abstract

Declarations

Approval Form

Dedications

Acknowdgements

List of Abbreviations and Symbols

Table of Contents

List of Figures

List of Tables

CHAPTER 1: : INTRODUCTION
1.1 Background to the study
1.2 Problem Statement
1.3 Aim
1.4 Objectives
1.5 Hypothesis
1.6 Structure of thesis

CHAPTER 2: : LITERATURE REVIEW
2.1 Background to Nanotechnology
2.1.1 Methods used to synthesize nanoparticles
2.1.2 Factors affecting nanoparticle synthesis
2.1.3 Mechanisms of Green Synthesis
2.1.4 Support material for nanoparticles
2.2 Photocatalysis
2.2.1 Introduction to photocatalysis
2.2.2 Photocatalysis of Congo Red
2.2.3 Factors affecting photocatalysis
2.2.4 Mechanism of Photocatalysis
2.2.5 Trimetallic nanoparticles as photocatalysts
2.2.6 Kinetic Models
2.3 Solid Phase Extraction
2.3.1 Background to Solid Phase Extraction
2.3.2 Methods used to enrich analytes
2.3.3 Factors affecting solid phase extraction of samples
2.3.4 Studies on enrichment of heavy metals using Solid Phase Extraction
2.3.5 Adsorption isotherms

CHAPTER 3: : PRELIMINARY STUDIES
3.1 Preparation of the aqueous leaf extract
3.2 Synthesis of P — ZrO2CeO2ZnO nanoparticles
3.3 Optimization of Synthetic Conditions

CHAPTER 4: METHODOLOGY
4.1 Chemicals and Materials
4.2 Equipment
4.3 Preparation of stock solutions
4.4 Synthesis of the P — ZrO2CeO2ZnO nanoparticles
4.5 Preparation of P — ZrO2CeO2ZnO nanoparticles/alginate beads
4.6 Characterization of the P — ZrO2CeO2ZnO nanoparticles
4.7 Determination of the metal’s concentration in P - ZrO2CeO2ZnO nanoparticles
4.8 Studies of kinetics and reaction mechanisms for photocatalytic degradation of Congo red using P — ZrO2CeO2ZnO nanoparticles photocatalyst
4.9 Enrichment of cadmium and lead
4.9.1 Adsorption Studies
4.10 Enrichment of Arsenic and Chromium by pipette tip solid phase extraction

CHAPTER 5: RESULTS AND DISCUSSION
5.1 Optimization of the method for the green synthesis of P-ZrO2CeO2ZnO nanoparticles using aqueous extracts from Flacourtia indica leaves
5.1.1 Optimization of Synthetic Conditions
5.1.2 Evaluation of interactions and significant factors for the synthesis of P - ZrO2CeO2ZnO using ANOVA
5.1.3 Main effects of variables on nanoparticle synthesis
5.1.4 Evaluation of interactions between influencing factors by response surface methodology for P — ZrO2CeO2ZnO nanoparticle synthesis
5.1.5 Possible reaction mechanism for P — ZrO2CeO2ZnO nanoparticles synthesis
5.1.6 Comparison with other studies
5.2 Characterization of surface composition
5.2.1 UV- Vis Spectroscopy Characterisation
5.2.2 Fourier Transform Infrared Spectroscopy (FT-IR)
5.2.3 Brunauer-Emmet-Teller (BET) analysis
5.2.4 Scanning Electron Microscopy and Energy Dispersive X-ray Spectroscopy Characterisation
5.2.5 X-ray Diffraction Characterisation
5.2.6 X-ray photoelectron spectroscopy characterisation
5.2.7 Determination of Metal Composition by Inductively Coupled Plasma-Mass Spectrometry
5.3 Kinetics and reaction mechanisms for photocatalytic degradation of Congo red using P — ZrO2CeO2ZnO nanoparticles
5.3.1 Catalytic activity of the P — ZrO2CeO2ZnO
5.3.2 The effect of catalyst amount on the degradation of Congo Red... 103
5.3.3 The effect of changing Congo red concentration on its degradation
5.3.4 The effect of reaction time on the degradation of Congo Red 106
5.3.5 Reaction kinetics for the degradation of Congo red 107
5.3.6 Regeneration of the P — ZrO2CeO2ZnO nanoparticle catalyst ... 110
5.3.7 The reaction mechanism for the catalytic degradation of Congo red.
5.4 Enrichment of lead and cadmium from water using P — ZrO2CeO2ZnO Nanoparticles/Alginate Beads: Optimization and determination of significant factors and interactions using response surface methodologies
5.4.1 Adsorption Equilibrium Studies
5.4.2 Screening of significant factors for Cd and Pb extraction
5.4.3 Optimization of the significant extraction conditions for Cd and Pb using the Taguchi experimental design
5.4.4 Evaluation of significant factors and interactions using Analysis of Variance (ANOVA)
5.4.5 Main effects of sample volume, dosage and pH on the enrichment of Cd and Pb using P — ZrO2CeO2ZnO nanoparticles/alginate
5.4.6 Evaluation of the most significant factors and interactions using response surface methodology and interaction plots
5.4.7 Interference Studies
5.4.8 Desorption cycles for Cd and Pb recoveries
5.4.9 Acceptance Criteria
5.4.10 Analytical Applications
5.4.11 Comparison with other methods
5.5 Enrichment of Arsenic and Chromium by pipette tips loaded with P — ZrO2CeO2ZnO nanoparticles /alginate beads
5.5.1 Adsorption Experiments
5.5.2 Optimization of SPE Experiments
5.5.3 Full factorial designs and response surface methodology for optimization of the significant conditions for Cr and As enrichment
5.5.4 Effects of sample volume, pH and dosage on enrichment factors of As and Cr and the interactions between factors
5.5.5 The effect of main factors on As and Cr enrichment
5.5.6 Effect of organic interferences on As and Cr enrichment
5.5.7 Regeneration studies for As and Cr enrichment
5.5.8 Evaluation of the enrichment of As and Cr method performance
5.5.9 Application in real samples
5.5.10 Comparison with other methods

CHAPTER 6: CONCLUSIONS AND RECOMMENDATIONS
6.1 Conclusions
6.2 Recommendations for future work

CHAPTER 7: LIST OF PUBLICATIONS

CHAPTER 8: REFERENCES

CHAPTER 9: APPENDIX
9.1.1.1 Tauc plots data
9.1.1.2 Linear Model Analysis: Means versus pH, Dosage (g), metal concentration (M), volume ratio
9.1.1.3 Determination of hydrogen bonding active sites of the P — ZrO2CeO2ZnO nanoparticle using alcohols
9.1.1.4 Antiplagiarism Report

Abstract

Anthropogenic activities have led to environmental pollution by toxic heavy metals and dyes such as Congo red. Trimetallic nanoparticles can be used for enrichment heavy metals and photocatalytic degradation of Congo red from the environment. However, the processes used to synthesize nanoparticles can be hazardous to the environment. In the study, green synthesis of Phosphorous doped ZrO2CeO2ZnO nanoparticles were carried out using Flacourtia indica leaf aqueous extracts with phytochemicals as reducing agents. The nanoparticles were used as photocatalysts for degradation of Congo red dye and as sorbents for enrichment of selected toxic metals: lead, cadmium, arsenic and chromium. The influence of various parameters during the synthesis and solid phase extraction stages were investigated using Half, Full and Taguchi experimental designs. Interactions between factors were determined using ANOVA and response surface methodologies. The enrichment methods were validated by using spiked borehole, well, tap and effluent water samples. The P-ZrO2CeO2ZnO nanoparticles and P-ZrO2CeO2ZnO nanoparticles/alginate beads were characterized using Ultra Violet Visible spectrometry, Scanning Electron Microscope(SEM), Fourier Transform- Infra Red Spectroscopy, Transmitting Electron Microscopy (TEM), Brunauer Emmet Teller (BET) analysis, X- ray Photoelectron Spectroscopy (XPS) and X ray Diffraction (XRD). The most significant factors for P-ZrO2CeO2ZnO nanoparticle synthesis were pH, metal ion concentration and leaf extract concentration. The surface areas obtained under optimum synthesis conditions were 0.459 m[2]g-[1] and 7.33 m[2]g-[1]for P-ZrO2CeO2ZnO nanoparticles and P-ZrO2CeO2ZnO nanoparticles/alginate beads respectively. The synthesized nanoparticles were crystalline and irregularly shaped The nanoparticles average size was 0.255 nm and the range of the size was from 0.1-4.51nm. Zn-O, Zr-O, C-O, O-H, functional groups were present in the nanoparticles from FTIR data. The optimum conditions for photocatalytic degradation of Congo red using P-ZrO2CeO2ZnO nanoparticles were 0.05 g/L catalyst dosage concentration, 10 mg/L Congo red concentration, 250 min irradiation time. The reaction followed pseudo first order kinetics with a rate constant of 0.069 min-1 and degradation efficiency of 85.85%.The reaction mechanism was explained by light, superoxide radicals and h+ holes. The most significant variable for cadmium recovery using P-ZrO2CeO2ZnO nanoparticles / alginate beads was the sample volume and for chromium recoveries these were sample volume, eluent flow rate and sorbent dosage. Interactions between factors during enrichment occurred between sorbent dosage and pH, sample volume and sorbent dosage, sample volume and pH. The method recoveries were 33.12-116.5, 57.0 -147.70, 46.56-130.65 and 20.96-82.51% and, limits of detection were 0.1022, 0.0297 g/L 0.084 and 0.439 ng/L for lead, cadmium, chromium and arsenic respectively. The SEM, TEM and XRD results showed that P-ZrO2CeO2ZnO nanoparticles can be synthesized using F. indica leaves extracts and they can efficiently degrade Congo red dye. It was also demonstrated that P-ZrO2CeO2ZnO nanoparticles encapsulated in alginate beads enhanced the detection limit of selected heavy metals, which may find applications in toxic metal analysis.

Declaration

I, Nichodimus Hokonya declare that: Green Synthesis of Trimetallic Nanoparticles using Flacourtia Indica (Burm.F.) Merr: Characterization and Applications, is my work and that the sources used have been indicated by means of complete references .

Illustrations are not included in the reading sample

Approval form

The undersigned do hereby certify that they supervised, read and recommend to the Bindura University of Science Education for acceptance the dissertation entitled, “Green Synthesis of Trimetallic Nanoparticles Using Flacourtia Indica (Burm.F.) Merr.: Characterization and Applications”, submitted by Nichodimus Hokonya in partial fulfilment of the requirements for the Doctor of Philosophy in Chemistry

NHokonya 14./...09.../...2024

(Signature of student)

16./.. .09/.. .2024

(Signature of Main Supervisor)

(Signature of Co-supervisor)

17./ 09../.2024

(Signature of Co-Supervisor)

Dedications

The thesis is dedicated to the Almighty, my late father the “General” Moses Mutambiranwa Hokonya who will always be my source of inspiration and motivation, my mum Conelia Marovanidze, my wife Felisters, my son Kudzaishe Moses, my daughter Kunaishe, my brothers Washington, Maxwell Chiromo, Moses Thabani Mpofu, Simukai, my sisters Charity, Jubilant, Hazvineyi, Nothando my cousins Tinomuda Mkweva, Samantha Nokutenda Masvosva and Anotidaishe for their constant prayers and encouragement. It is by God’s grace that I managed to successfully pursue this DPhil degree.

Acknowledgements

I would like to pass my heartfelt gratitude to my main supervisor Prof C. Mahamadi, co-supervisors Dr N. Muchanyereyi and Prof T. Gutu for their patience and timely guidance. I would also like to thank Prof C. Zvinowanda for helping me with characterization and comments as well as suggestions on the photocatalysis paper. Special mention goes to the late Prof M. Mupa for his suggestions during presentations and making sure l had access to all the chemicals and equipment l needed during his tenure as Chairman; Dr C. Machingauta for his meaningful discussions on characterisation of nanoparticles, Prof P. Dzomba for his suggestions on solid phase extraction and Prof N, Chaukura for his suggestions on photocatalysis methodology. Mr T. Chayamiti and Mr V. Chibuku for their technical assistance with FT-IR and UV- Vis spectrometry as well as reagents.

List of Abbreviations and Symbols

ANOVA Analysis of Variance

BET Brunauer-Emmet-Teller analysis

FT-IR Fourier transform infrared spectrometry

GC-MS Gas Chromatography Mass Spectrometry

ICP-MS Inductively Coupled Plasma Mass Spectrometry

SEM Scanning Electron Microscopy

SPE Solid Phase Extraction

TEM Transmission Electron Microscopy

UV DRS Ultra Violet Diffractance spectrometry

WHO World Health Organization

P-XRD Powder X-ray Diffraction

List of Figures

Figure 2:1 A mechanism of biosynthesis of nanovalent ZnO

Figure 2:2: Structure of Sodium alginate

Figure 3:1 A: Flacourtia indica plant

Figure 3:2: F indica plant aqueous leaf extracts (A) and P — ZrO2CeO2ZnO nanoparticle solutions (B) at different pH

Figure 4:1: a) P — ZrO2CeO2ZnO nanoparticles/alginate beads being extruded from syringes and b) wet alginate beads in a petri dish

Figure 4:2. A) The LED warm white light coiled around the beaker photoreactor B) The complete photoreactor used during decolourization experiments consisting of LED light and the beaker wrapped with aluminium foil on a magnetic stirrer 60

Figure 4:3: (A) P — ZrO2CeO2ZnO nanoparticles/alginate beads loaded onto syringe tips and covered by glass wool (B) Sample reservoir, peristaltic pump and syringe setup used during solid phase experiments 62

Figure 4:4: Pipette tips loaded with P — ZrO2CeO2ZnO nanoparticles/alginate beads and glass wool 65

Figure 5:1 The main effects of change in (a) pH, (b) leaf extract concentration or dosage (c) metal ion precursor concentration and (d) metal ion to leaf extracts volume ratio on P — ZrO2CeO2ZnO nanoparticles synthesis 72

Figure 5:2: Response surface plot for the interaction of (a) volume ratio and metal concentration, (b) volume ratio and dosage, (c) metal concentration and dosage, (d) volume ratio and pH, (e) metal concentration and pH, (f) dosage and pH 76

Figure 5:3: UV-Vis spectrum of the P — ZrO2CeO2ZnO nanoparticles at a. 0.05M nanoparticles at pH 3, 5, 9 and 12, b. 0.1M nanoparticles at pH 3, 5, 9, and 12, c. 0.2M nanoparticles at pH 3, 5, 9 and 12 82

Figure 5:4 UV Vis spectrum of a) P — ZrO2CeO2ZnO nanoparticles and b) ZrO2CeO2ZnO nanoparticles and determination of band gap c)and e) for P — ZrO2CeO2ZnO nanoparticles at n=2 and n=1/2 respectively and d) and f) for ZrO2CeO2ZnO nanoparticles at n = 2 and n=1/2 respectively 85

Figure 5:5: FT-IR Spectrum of (a) raw plant (b) P — ZrO2CeO2ZnO nanoparticles

Figure 5:6: FT IR spectrum of a 1% P — ZrO2CeO2ZnO nanoparticles/alginate composite a) before and b) after adsorption

Figure 5:7: N2 adsorption-desorption curves of (a) raw plant and (b) P — ZrO2CeO2ZnO nanoparticles

Figure 5:8: Surface plots for alginate and 1% P — ZrO2CeO2ZnO nanoparticle/ alginate composite

Figure 5:9: Statistical thickness of a) alginate and b) 1% P — ZrO2CeO2ZnO NP alginate

Figure 5:10: (a) SEM image, (b) EDS spectrum, (c & d) TEM image, (e) Particle distribution (f) and (g) SAED images of P — ZrO2CeO2ZnO

Figure 5:11: EDX mapping images for a) oxygen, b) phosphorous, c) zinc, d) cerium, e) zirconium within the P — ZrO2CeO2ZnO nanoparticles

Figure 5:12: a), b), c) SEM image of P — ZrO2CeO2ZnO nanoparticles/alginate beads

Figure 5:13: XRD pattern of the P — ZrO2CeO2ZnO nanoparticles

Figure 5:14: XRD pattern of P — ZrO2CeO2ZnO nanoparticles/alginate beads

Figure 5:15 XPS showing the elements present in the P — ZrO2CeO2ZnO nanoparticles a) sodium, b) zinc, c) cerium, d) carbon, e) chlorine, f) zirconium, g) sulphur, h) phosphorous

Figure 5:16 The effect of 0.05, 1 and 2 g/L catalyst dosage on decolouration of 10 mg/L Congo red and insert colour changes with time after degradation. 105

Figure 5:17. The effect of changing congo red concentrations (10, 15 and 25 mg/L) on photodegradation by 1 g/L of P — ZrO2CeO2ZnO nanoparticles catalyst and insert colour changes as the reaction progressed 106

Figure 5:18. The effect of varying reaction time on the photocatalysis of 15 mg/L congo red by 1 g/L P — ZrO2CeO2ZnO nanoparticles

Figure 5:19. Kinetic modelling for the degradation of 10, 15 and 25 mg/L congo red using 1 g/L P — ZrO2CeO2ZnO nanoparticles a) Pseudo zero order, b) Pseudo first order, c) pseudo-second order

Figure 5:20. The recycling experiments for degradation of 20 mg/L congo red using 1 g/L P — ZrO2CeO2ZnO nanoparticles

Figure 5:21. Effect of different scavengers on degradation of 15 mg/L Congo red

Figure 5:22. a) Pseudo zero order, b) pseudo first order, c) pseudo second order kinetic modelling for the inhibition reactions of 15 mg/L congo red

Figure 5:23. The proposed mechanism of photocatalysis of Congo red using P — ZrO2CeO2ZnO nanoparticles

Figure 5:24: (a) Langmuir, (b) Temkin, (c) Freundlich and (d) Dubinin- Radushkevich plots for Cd adsorption

Figure 5:25: (a) Langmuir, (b) Freundlich, (c)Temkin and (d) Dubinin- Radushkevich plots for Pb adsorption

Figure 5:26: Normal plots for effects of flow, dosage, pH., sample volume, eluent flow rate and eluent concentration on extraction recovery

Figure 5:27: Pareto chart for the effects on flow, dosage, pH., sample volume, eluent flow rate and eluent concentration on extraction recovery of lead and cadmium

Figure 5:28: Residual plots for the enrichment of Cd and Pb

Figure 5:29: Main effect of sample volume, dosage and pH on enrichment factor of (A) Cd and (B) Pb

Figure 5:30 Distribution of lead hydroxide and cadmium hydroxide at various pH

Figure 5:31: Surface plots for sample volume, dosage and pH vs enrichment factor of Pb (A) and Cd (B)

Figure 5:32: Interaction plots for sample volume, dosage and pH vs enrichment factor for Pb and Cd

Figure 5:33: The effect of increasing the concentration of phenol and propanol on recoveries of Cd and Pb from water samples

Figure 5:34: Cd and Pbadsorption-desorption cycles

Figure 5:35: Pareto chart for optimization of the significant effect for solid phase extraction of a) As and b) Cr

Figure 5:36: Residual plots for the enrichment of a) Cr and b) As

Figure 5:37:Interaction plots for the effect of sample volume, dosage and pH on enrichment factors

Figure 5:38: Main effects plots for sample volume, dosage and pH on As and Crenrichment factor

Figure 5:39: Effect of a, b) methanol and c, d) ethanol on recovery of As and Cr

Figure 5:40 Extraction recovery cycles for As and Cr

Figure 9:1: Calibration curve for Cr and As SPE

Figure 9:2Calibration curve for Cr and As SPE

List of tables

Table 2:1: Studies on the synthesis of trimetallic nanoparticles

Table 2:2 Green synthesis of trimetallic nanoparticles

Table 2:3 Removal of pollutants using trimetallic photocatalysts

Table 2:4 Solid phase extraction of heavy metals using various sorbents

Table 3:1: The Taguchi design for the optimization of P — ZrO2CeO2ZnO nanoparticles synthesis

Table 5:1 Optimization of synthetic conditions of P — ZrO2CeO2ZnO nanoparticles

Table 5:2: ANOVA results for the determination of the most significant factors for synthesis of P — ZrO2CeO2ZnO nanoparticles

Table 5:3: A comparison of the current study for the synthesis of P — ZrO2CeO2ZnO nanoparticles with other studies

Table 5:4: BET Surface area analysis of alginate and P — ZrO2CeO2ZnO nanoparticle loaded beads

Table 5:5 XPS Chemical ID and Quantification

Table 5:6: Quantification of metal concentration in P — ZrO2CeO2ZnO nanoparticles and 1% P — ZrO2CeO2ZnO NP/alginate

Table 5:7. Parameters of kinetic study of the photocatalytic degradation of 10, and 25 mg/L congo red using 1 g/L P — ZrO2CeO2ZnO nanoparticles

Table 5:8. Kinetic parameters for the EDTA, t-butanol, and potassium dichromate inhibition reactions

Table 5:9. A comparison of photodegradation efficiency of catalysts using congo red as substrate

Table 5:10: Langmuir, Freundlich, D-R and Temkin isotherm parameters

Table 5:11: Multiple Response Prediction Parameters

Table 5:12: Results of the optimization of the most significant extraction conditions for Cd and Pb

Table 5:13: Taguchi model for optimization of enrichment of Pb

Table 5:14: Taguchi model for optimization of enrichment of cadmium from water samples

Table 5:15: Results of acceptance criteria for the analysis

Table 5:16 Recoveries for well water and borehole water

Table 5:17. Comparison of this study with some enrichment studies in the literature

Table 5:18: Langmuir, Freundlich, D-R and Temkin isotherm parameters

Table 5:19: Multiple Response Prediction Parameters

Table 5:20: Results for optimization of significant extraction conditions for As and Cr

Table 5:21: Results of the validation data for the analysis

Table 5:22: Recovery tests from well and effluent water samples

Table 5:23: Comparison of As and Cr enrichment and determination using other methods

Table 9:1 Tauc plots for undoped nanoparticles

Table 9:2 Tauc plots for dried doped P — ZrO2CeO2ZnO nanoparticles

Table 9:3 Estimated Model Coefficients for Means

Table 9:4: Fits and Diagnostics for Unusual Observations for P — ZrO2CeO2ZnO nanoparticle synthesis

Table 9:5: Adsorption equilibrium studies parameters

Table 9:6: Adsorption equilibrium studies parameters

Table 9:7Adsorption equilibrium parameters for Cd

Table 9:8: Adsorption equilibrium parameters for Pb

Table 9:9: Adsorption desorption cycles for Pb and Cd Solid phase extraction

Table 9:10: Effect of ethanol, methanol, propanol, phenol and mixture on bonds

CHAPTER 1 : INTRODUCTION

1.1 Background to the study

Dyes in wastewater.

Approximately 1-20 % of organic dyes are discharged into the environment after their use in dye-including industries and they pollute huge quantities of water (Nassar et al., 2016). Dyes find various applications in rubber, textile, plastic, cosmetic, leather, paper making and pharmaceutical industry (Ngulube et al., 2016). A large amount of dye material does not bind during the colouration process and is lost to wastewater and this may lead to serious contamination issues (Lima et al., 2018). Dye wastewater has the potential to be carcinogenic and mutagenic since it resists biodegradation and poses a threat to the adjacent environment when waste is disposed of without proper treatment. Hence there is a need to find treatment technologies that can reduce the toxic effects of dyes to within recommended water quality guidelines (Ngulube et al., 2016).

Various methods are used to remove organic pollutants such as dyes from aquatic systems such as biological treatment, advanced oxidation process, photocatalysis, adsorption and membrane bioreactors among others (Ahsan et al., 2018; Bouju et al., 2008; Martínez et al., 2011; Mohammadi & Veisi ., 2018). Metal oxide nanomaterials have attracted much attention as strong candidates for photocatalytic degradation of toxic pollutants (Pascariu et al., 2019). Visible light-induced photocatalysis is highly efficient in degrading dyes without any secondary contamination (Abdelwahab & Helaly, 2017). Photocatalytic degradation can be improved by lessening the band gap and extending the absorption range to the visible region leading to electron-hole separation by coupling semiconductor catalysts (Fazizadeh et al., 2017).

Various studies have shown that bimetallic and trimetallic nanophotocatalysts are more superior to their monometallic counterparts. Monometallic photocatalysts have limitations of fast electron-hole recombination and require a band gap of below 2.0 eV or below them for them to be activated. Bimetallic and trimetallic photocatalysts have a reduced band gap and their adsorption is shifted to the visible region thereby increasing their environmental applications. Both have comparable removal efficiencies. There is a need to combine different metals to study their effect on bandgap energy and hence their photocatalytic activity. The catalyst needs to be tested on various emerging contaminants to check their efficiencies and degradation products need to be identified to determine if they are toxic to the environment. Various ways for synthesizing catalysts have been used, but recently, green synthesis is of major importance since it uses environmentally friendly solvents and renewable materials.

Trace metals in the environment

Rapid growth of global industrialisation and extensive use of metals in manufacturing and mining has caused serious environmental issues in terms of pollution. Water pollution by trace metals has been a challenging problem for human health since some trace metals like arsenic, cadmium, mercury and lead are potentially carcinogenic, difficult to biodegrade and easily accumulate in living organisms even at low concentrations (Huang et al., 2018; Prasse et al., 2015).

Metalloids such as arsenic have maximum adverse effects on human health through drinking contaminated water. Arsenic exists in two oxidation forms namely: (III) and(V). Under anaerobic conditions in groundwater As (III) exists asH3AsO3, H2AsO3 andHAsO3-. As (V) dominates in surface water as H3AsO4, HAsO3-, H2AsO4 . Arsenic finds use in the production of pigments, semiconductors, herbicides, glass, transistors, pesticides, insecticides and paper. Long-term exposure to arsenic may result in the development of conjunctivitis, hyperkeratosis, hyperpigmentation, cardiovascular disease, skin cancer, gangrene of limps, and disorder of the central nervous system and peripheral vascular system (Martinez-Vargas et al., 2018; Masindi & Gitari, 2016; Nidheesh & Singh, 2017).

Chromium is widely used in the manufacture of products for corrosion protection, leather tanning, alloying, metal-ceramic, metal electroplating, manufacture of synthetic rubies, dye, wood preservation and paints. Chromium exists under the II, III and VI oxidation states. The less abundant chromium species is the divalent form because it is unstable. Chromium III has lower solubility, toxicity and mobility than the other forms. It plays an important role in lipid, glucose and protein metabolism making it an essential micronutrient for many living organisms. Chromium VI causes vomiting, liver damage, nausea, vertigo and fever when ingested orally because it is highly soluble, strongly oxidizing and mobile. The maximum permissible limit of chromium in drinking water according to WHO guidelines is 0.005 mg/L (Briffa et al., 2020; Sahayam et al., 2005).

Cadmium is a non-essential metal which is highly toxic at very low exposure levels. It is released into the environment through forest fires, volcanic eruptions and sea sprays. Human activities such as welding, mining, cigarette smoking, and refineries are also the greatest contributors to cadmium pollution (Kasa et al., 2019). The other contributors to cadmium contamination in drinking water are impurities in solders, galvanised pipes and metal fittings. It has a wide range of toxicities on respiratory, renal and nervous systems. Cadmium is also said to be carcinogenic in large doses (Hokonya & Mahamadi, 2017; Nunez et al., 2018). The maximum permissible limit for Cd in drinking water according to WHO guidelines is 0.003 mg/L.

Lead is highly toxic at low concentrations and long-term exposure to lead at low concentrations results in it being accumulated by the body due to its low rate of excretion. Lead accumulation in the body can cause blood and brain disorders as well as serious nervous system disorders (Fayazi et al., 2016).

Trace metal analysis is important for monitoring and identification of health problems. Various techniques have been used to determine the levels of trace metals including Flow Injection Analysis Atomic Adsorption Spectrometry (FIA-AAS), Electrothermal Atomic Absorption Spectrometry (ETAAS), Inductively Coupled Plasma Mass Spectrometry (ICP-MS), Atomic Fluorescence Spectroscopy (AFS), Inductively Coupled Plasma Optical Emission Spectrometry (ICP-OES) (Akhtar et al., 2020;

Amran et al., 2020; Henríquez-Hernández et al., 2017; Magoda et al., 2016b). ICP- MS is the most powerful tool used to determine trace elements due to its wide dynamic linear range, rapid detection, low detection limit, multi-element/isotope analysis and very little interference. The application of ICP-MS for direct trace analysis of elements in complex systems sometimes suffers from problems of the concentration of the target elements being lower than the instrument limit of detection and matrix effects; hence there is a need for some form of appropriate sample pre-treatment for enrichment or removal of matrixes.

Trace metals have been enriched using solid phase extraction (Yavuz et al., 2016), liquid-liquid microextraction (Mandlate et al., 2017; Ozzeybek et al., 2020a), cloud point extraction (Blanchet-Chouinard & Lariviere, 2018; Smithies et al., 2008), coprecipitation (Arslan et al., 2018), reductive extraction (Jung & Baek, 2015) and electrodeposition (Najafi et al., 2009).

Solid phase extraction is used for the preconcentration of samples because the technique; has low cost, has low consumption of solvents, is simple, has high preconcentration factors and is rapid. The performance of solid phase extraction depends on the properties of the sorbent (Ahmad & Solimano, 2016; Calderilla et al., 2018; Molaei et al., 2017; Plotka-Wasylka et al., 2017). The challenge nowadays is on development of a sorbent with excellent enrichment properties. A wide variety of materials such as activated carbon (Dimpe et al., 2018) l-cysteine modified zeolites (S. Ahmad & Soleymanpour, 2016), carbon nanotubes (Li et al., 2009), nanoTiO2 (Yang et al., 2020) and ionic imprinted polymers (Barciela-Alonso et al., 2014) have been used as sorbents for solid phase extraction. Nanomaterials have gained popularity as solid-phase sorbents for trace elements due to their large surface area and chemical stability (He et al., 2017).

Sample preconcentration is influenced by the eluent volume, sorbent mass, time, eluent volume, pH, and sample volume. Screening of these factors one at a time is tedious, and expensive and fails to give information on synergism or antagonism simultaneous contribution to response (Alipanahpour Dil et al., 2018).

Response surface methodologies

Multivariate analysis or response surface methodologies allow optimization of procedures through fast, economic pathways as well as allow more than one variable to be optimized simultaneously. The analysis can also provide high-quality predictions in studying linear , quadratic and interaction effects, which influence a system whereas interactions are not observed in single-factor analysis (Asfaram et al., 2016).

Many studies have employed the one-factor at a time (OFAT) method to determine the sample sizes and testing procedures, regardless of the economic issues and the weakness of this method in examining the interaction effect of variables. The shortcomings of OFAT can be overcome by using Response surface methodology (RSM) which is comprised of statistical procedures applied to determine the optimum conditions for experimental conditions by considering the lowest numbers of experiments. The advantages of RSM are; a minimal number of experiments, fewer chemicals consumed and low cost. The RSM also generate mathematical models that permit the assessment of the relevant interaction effects and statistical significance of factors (Dimpe et al., 2018). The Taguchi experimental design is based on the application of orthogonal arrays which are employed to minimize the number of experiments to be performed and they are useful for identifying the effect and the importance of the factors on the response variable of the experimental design (Tovar- Gomez et al., 2015).

Green synthesis of nanoparticles

The study of nanocomposites is of great interest because they have a high surface area to mass ratio which enhances their absorbing and catalytic activity. This property enhances their effectiveness in pollutant removal from the environment. The properties of nanocomposites are enriched by alloying because it provides structural diversity and optimum composition synergic effect between the constituent metals. These enhanced properties have allowed trimetallic nanoalloys to be applied in various applications (Sharma et al., 2018; Wang et al., 2012). Physical techniques also require high vacuums, high temperatures and relatively expensive equipment. The drawback of chemical synthesis is some pollutants and toxic materials are created as products of chemical reactions (Gharagozlou et al., 2015), hence it is necessary to use environmentally friendly techniques like green synthesis. Based on the aforementioned, the following aims and objectives are highlighted.

1.2 Problem statement

1. Conventional methods used to treat wastewater contaminated with dyes can cause secondary contamination and are inefficient and expensive. Photocatalysis has attracted many researchers’ attention due to its high efficiency in degrading organic dyes and production of non-toxic products. Hence many efforts have been directed towards the synthesis of new catalysts (Li et al., 2019).
2. Direct determination of trace metals is a very difficult task since their concentration is close to or below most analytical instruments detection limit. Sample matrix can cause serious interference during the analysis of real samples. Hence there is a need for sample cleanup and preconcentration.
3. Nanoparticles are used as photocatalysts and adsorbents for the enrichment of toxic trace metals. Most physical and chemical methods used to synthesise nanoparticles suffer from several drawbacks such as the use of high pressure and temperature, long reaction time, toxic reagents, and requirements of external additives such as specific base, stabilizer and promoter during the reaction which limits the purity of the final product (Darroudi et al., 2014). There is a need to search for green and environmentally friendly methods.

1.3 Aim

To synthesize a trimetallic ( P — ZrO2CeO2ZnO) nanoparticles composite using Flacourtia indica (Governor’s plum) aqueous leaf extracts as the reducing agent and use the synthesized nanoparticles at the catalyst for photo-oxidation of toxic Congo red and also immobilize the P — ZrO2CeO2ZnO nanoparticles on alginate for the enrichment of selected toxic trace metals from environmental water solutions.

1.4 Objectives

1) To prepare phytochemical-rich aqueous extracts from F. indica leaves;
2) To study the effect of factors: pH, leaf extract dosage, metal ion concentration, metal ion concentration to leaf extract volume ratio and interactions between the factors on P — ZrO2CeO2ZnO nanoparticle synthesis;
3) To characterize the synthesised nanoparticles by Scanning Electron Microscopy, Transmission Electron Microscopy, X-Ray Diffraction, X-Ray Photoelectron Spectroscopy, Uv- Vis Spectroscopy, Brunauer Emmet-Teller Analysis, Fourier Infrared Spectroscopy, Inductively Coupled Plasma Mass Spectrometry;
4) To determine the catalytic activity, kinetic models and mechanism for the photodegradation of Congo red using P — ZrO2CeO2ZnO nanoparticles;
5) To immobilize the P — ZrO2CeO2ZnO nanoparticles on alginate and characterize them using Scanning Electron Microscopy, Transmission Electron Microscopy, X-ray diffraction and Inductively Coupled Plasma Mass Spectrometry; and,
6) To determine the significant factors and interactions which affect the enrichment of cadmium, lead, arsenic and chromium using P —ZrO2CeO2ZnO nanoparticles/alginate beads to detection using Inductively Coupled Plasma Mass Spectrometry and model the data using Half factorial, Full factorial and Taguchi designs.

1.5 Hypothesis

• P — ZrO2CeO2ZnO nanoparticles can be synthesised using F. indica as a reducing and stabilizing agent.
• P — ZrO2CeO2ZnO nanoparticles/alginate composite beads can be used for solid phase extraction for preconcentration of arsenic, cadmium, lead, and chromium and before ICP-MS analysis.
• P — ZrO2CeO2ZnO nanoparticles can act as an efficient catalyst for photodegradation of Congo red.

1.6 Structure of the thesis

Chapter 1 highlights the background of the study. Chapter 2 reviews the literature for green synthesis of trimetallic nanoparticles, solid phase extraction of cadmium, lead, chromium and arsenic and photocatalysis of Congo red. Chapter 3 highlights the preliminary studies carried out to optimize nanoparticle synthesis. Chapter 4 describes the methodologies applied during the thesis. Chapter 5 describes the (a) optimization of green synthesis of the —ZrO2eO2ZnO nanoparticles and effect of various factors on synthesis (b) reports on optimization of photodegradation of Congo red using P — ZrO2CeO2ZnO nanoparticles, (c) the use of P —ZrO2CeO2ZnO nanoparticles/alginate beads on recovery of lead and cadmium followed by ICP-MS analysis, (d) use of P — ZrO2CeO2ZnO nanoparticles immobilized on alginate loaded in pipette tips for the preconcentration of arsenic and chromium followed by detection using ICP-MS and effects of interactions on recovery. Chapter 6 summarises the research findings and highlights future work.

CHAPTER 2 : LITERATURE REVIEW

2.1 Background to Nanotechnology

Nanotechnology is the understanding and control of matter and processes typically at the nanoscale but not exclusively below 100 nm in one or more dimensions where the onset of size-dependent phenomenon usually enables novel applications. A Nano­object has at least one spatial (Euclidean) dimension less than 100 nm. Nanofibers have two dimensions less than 100 nm and nanoparticles have all three dimensions less than 100 nm (Ramsden, 2018).

Nanotechnology has emerged as the most interesting area of research due to the unique properties of nanoparticles which are decided by crucial parameters such as shape, size and morphology (Sithara et al., 2017). Nanocomposites are enriched by alloying which provides structural diversity and optimum composition synergic effect between the constituent metals. (Sharma et al., 2018; Wang et al., 2012).

Nanoparticles have smart mechanical and physicochemical properties which are completely different from their bulk counterparts (Gnanamoorthi et al., 2015). The properties of nanoparticles are due to reduced dimension about the excitonic radius of the bulk material and high surface-to-volume ratio (Mohan et al., 2015). The physical and chemical properties of nanoparticles also depend on their morphological factors such as shape and size (Sathish & Balakumar, 2017). Metallic nanoparticles have higher surface Plasmon resonance whilst nanoparticles with different shapes and sizes have different scattering and adsorption properties (Martinez-Hurtado, 2011).

2.1.1 Methods used to synthesize nanoparticles

Nanoparticles are synthesised by chemical methods such as solvothermal (Arumugam et al., 2018), sonochemical (Muradov et al., 2018), chemical successive reduction (Suwannarat et al., 2018), biological chemical synthesis (Vaseghi et al., 2018a), microwave-mediated synthesis (Kuzmanoski et al., 2016), precipitation-precipitation and impregnation (Allaedini et al., 2015), wet chemical method (Singh & Khandpekar, 2016), catalytic chemical vapour deposition (CCVD) (Lobiak et al., 2015) and molten salt method (Wu et al., 2009). Physical methods used for nanoparticle synthesis include reverse microemulsion (Xu et al., 2018), co-impregnation (Bkour et al., 2017), water in oil (Fedorenko et al., 2017), solvent-induced (Pandey et al., 2017), practical hot injection method (Tang et al., 2016), sol-gel (Dubey et al., 2015), supercritical route (Zhao et al., 2015), ball milling and reduction (Sun et al., 2013), hydrothermal (Zahedifar et al., 2013), mechano-chemical processing (Sabri et al., 2012), solid-state reaction (Choudhary et al., 2010) and plasma arch discharge (Lee et al., 2010).

Physical and chemical methods are summarized in Table 2.1. Most physical and chemical methods used to synthesize nanoparticles suffer from several drawbacks such as the use of high pressure and temperature, long reaction time, toxic reagents, and requirements of external additives such as specific base, stabilizer and promoter during the reaction which limits the purity of the final product (Darroudi et al., 2014). Physical techniques also require high vacuums, high temperatures and relatively expensive equipment. Chemical synthesis has a drawback since some pollutants and toxic

materials are created as by-products of chemical reactions (Gharagozlou et al., 2015).

Thus, it is necessary to use environmentally friendly techniques called green synthesis.

Table 2:1: Studies on the synthesis of trimetallic nanoparticles

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Green synthesis of nanoparticles

The important issues in green synthesis methods of nanoparticles are utilization of non-toxic chemicals, environmental friendly solvents and renewable materials (Bozkurt, 2017). Biological synthesized nanoparticles exhibit greater specific surface area and catalytic activity compared to nanoparticles synthesized through chemical means (Nordmeier et al., 2017). Nanoparticles have been synthesized using coffee extract (Poggialini et al., 2018), leaf and bark extracts of Syzygiumjambos(L), Myrtaceae (Dutta et al., 2017), Rosa damascene, Thymus vulgaris, Urtiadioica (Fazlzadeh et al., 2017), leaf extracts of Azadirachta indica (Sharma et al., 2017b), Cucumis anguria leaf extracts (Muchanyereyi-Mukaratirwa et al., 2017), Solanum tuberosum (Ramezanpour et al., 2019), Aloe Vera (Ali et al., 2016b), Mangifera indica, Murraya Koenigii, Azadiracta indica, Magnolia champaca (Devatha et al., 2016), Moring orifera plant extracts (Ezhilarasi et al., 2016), Sapindus mukorosi (Jassal et al., 2016) Anthemis xylopoda flowers (Nasrollahzadeh et al., 2015), turmeric leaves (Mihir & Siddhivinayak, 2015), green tea extracts (Mystrioti et al., 2014) Sargassum muticum (brown seaweed) (Mahdavi et al., 2013), Magnolia Kobus and Diopyros kaki leaf extracts (Song et al., 2009). Green synthesis of trimetallic nanoparticles have been a subject to research on and some of the studies are summarised in Table 2.2

Table 2:2 Green synthesis of trimetallic nanoparticles

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Plant mediated synthesis of metal nanoparticles using whole or parts of plants is gaining extensive research focus due to its ease in scaling up for larger production, cost effectiveness and environmental friendliness (Devatha et al., 2016). The biomolecules in plants extracts act as electron shuttles in metal reduction whilst others act as capping agents, thereby controlling the aggregation of nanoparticles as well as post surface modification (Ali et al., 2016).

2.1.2 Factors affecting nanoparticle synthesis

The rate of production of nanoparticles, their quality and other characteristics are affected by the nature of plant extracts, concentration of metal salt, concentration of plant extract, the pH, contact time and temperature of the solution (Mittal et al., 2013).

Furthermore, concentration of the capping and reducing agent plays a vital role in green synthesis of nanoparticles since at very low concentration of capping agent, unstable nanoparticles can be formed and at high concentrations nanoparticles segregation can occur (Kumar & Upadhyay, 2016). Hence concentration is a major determinant for reduction and stabilization exerted by the biomolecules which may determine the shape and size of nanoparticles.

The synthesis of nanoparticles is only possible when the metal salt precursor’s concentration is within the appropriate range for nucleation. Nanoparticle synthesis by reduction of metals precursors is determined by the availability of capping and reducing agent. In a study by Kumar and Upadhyay, (2016) involving synthesis of copper nanoparticles using glucose and L-cysteine, they found out that at 0.1 M glucose/L-cysteine concentration no reduction occurred whereas reduction increased from 0.2 M to 1.0 M glucose/L-cysteine concentration and beyond 1.0 M no increase was observed. Zuo et al., (2014) synthesized ZnO using microcrystalline cellulose and they found out that the added amount of microcrystalline cellulose can tune the morphology of ZnO crystallites. When 0.5 g microcrystalline cellulose was added, ZnO nanoparticles slices existed as a cluster and when the amount of microcrystalline cellulose was increased from 1.0 to 3.0g the morphology of ZnO transformed into flower cluster.

The pH of the plant extract solution can influence the electrical charge of the phytochemicals thereby affecting growth of nanoparticles, the extract capping and stabilizing abilities. A particular pH range can be favourable for the formation of nanoparticles of certain shapes, hence achieving greater stability. Ali and other researchers synthesized ZnO nanoparticles and they found out that less adsorption by nanoparticles occurred at lower pH of 5.0-7.0. They suggested that it was probably due to aggregation rather than nucleation of ZnO nanoparticles to form larger particles. The maximum reduction of ZnSO4 occurred around pH 8.0 (Ali et al., 2016a).

Temperature control is critical during plant mediated nanoparticles synthesis since it may enhance the reaction rate and rapid formation of nuclei from metal ions. The metal ion concentration can also affect the size of the nanoparticles formed. In a study by Matinise et al., (2017), the equivalent diameter varied in a quadratic way with initial concentration i.e. it increases with increase in concentration.

2.1.3 Mechanisms of green synthesis

Three mandatory components are essential for plant mediated nanoparticles synthesis and they are the stabilizing agent, reducing agent and a solvent medium that can solubilise the metal of interest. The reactions which occur during the green synthesis are as follows (i) short induction period, (ii) growth phase (iii) termination period. The nanoparticles growth phase occurs at a slower rate than the reduction and nucleation phases of the metallic ions which leads to higher concentration of nanoparticles. Metallic ions interact with biomass through ionic binding with bioinorganic reducing agents such as terpenoids and flavonoids in the absence of another stronger ligand. The adsorption of bio-reducing agents on the surface of metallic nanoparticles is believed to be attributed to the presence of electrons and carbonyl groups in their molecular structure (Gan & Li, 2012).

Matinise and co-workers proposed a mechanism of biosynthesis of nanovalent ZnO nanoparticles (Figure 2.1). They suggested that three elemental reactions of the solvated zinc ions with phenolic acids, flavonoids and vitamin-based compounds. They suggested that L-ascorbic acid is oxidized to L-dehydro-ascorbic acid via a free radical reaction followed by electrostatic attraction between free radical and cation of the precursors (Matinise et al., 2017).

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Figure 2:1 A mechanism of biosynthesis of nanovalent ZnO

Source: Matinise et al. (2017)

In this study trimetallic nanoparticles were synthesised by combining three different metals and when used as catalysts their properties can be modified better than monometallic catalyst. The trimetallic catalysts’ surfaces are unstable and can be precipitated during the catalysis reactions. However they can be stabilized by block copolymers, organic ligands, surfactants and dendrimers (Sharma et al., 2017c). Doping is used to modify nanoparticles’ luminescence, optical and electrical properties of semiconductor nanoparticles by introducing traps and discrete energy states in the band gap of excited electrons (Muruganandam et al., 2017). Doping transition metals with phosphorous atom into the crystal structure has been widely studied recently. Trimetallic nanoparticles have been used as catalysts (Allaedini et al., 2015; Liang et al., 2018; Zhang et al., 2017), antimicrobials (Vaseghi et al., 2018a), adsorbents (Sharma et al., 2017a), immunosensors (Tian et al., 2016), sensors (Cheng et al., 2014) and charge storage elements for memory devices (Haik et al., 2014).

2.1.4 Support material for nanoparticles

Encapsulation of nanoparticles is necessary because it increases the adsorption properties of the material (Phiri, 2016) and agglomeration of nanoparticles is inevitable hence there is need for an ideal support to decrease nanomaterials agglomeration (Nasrollahzadeh et al., 2016). Support material for nanoparticles includes zeolites (Ghavaminejad et al., 2016) and cellulose nanofibers (Fu et al., 2015), polyvinyl alcohol/ sodium alginate beads (Lv et al., 2013). Alginate is a polymeric acid (Figure 2.2) which occurs naturally, and it is extracted from brown seaweeds namely Macrocystis, Laminaria, Fucus, Ascophyllum, Eklonia and Pelvetia. Microorganisms such as Pseudomonas and Azobacter vinelandi can also synthesize alginate. Alginate is composed of 1,4 linked fl -D- mannuronic acid (M) and a -L-glucuronic acid (G) of varying composition and sequence (Grassi et al., 2009; Qin et al., 2006). Alginates possess a high degree of physiochemical heterogeneity which influences their quality and determines their application potential. The physiochemical properties such as sol/gel transition, viscosity and water retention ability are influenced by its molecular weight, composition and distribution of M and G blocks (Szekalska et al., 2016). Alginate has been used for encapsulation of drugs (Joshy et al., 2018), encapsulation of vitamins (Ota et al., 2018), wound dressing (Taskin et al., 2013; Tong et al., 2017), preparation of hydrogels for sorption of organic compounds (Castilhos et al., 2017), nanoparticles synthesis (Oualid et al., 2017), adsorption of drugs (Fei et al., 2016), immobilization of enzymes (Anwar et al., 2009; Raghu & Rajeshwara, 2015), adsorption of ions (Zahid et al., 2015), adsorption of metals (Lv et al., 2013), drug release Abbaspour et al., 2013; Rajendran & Basu, 2009), thickening, gel forming and colloid stabilizing agent in food and beverages industries and binder in tablet formation (Mandal et al., 2010).

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Figure 2:2: Structure of Sodium alginate.

Source: Grassi et al., (2009)

2.2 Photocatalysis

2.2.1 Introduction to photocatalysis

Photocatalytic transformation of organic pollutants into non-toxic molecules is now widely used for their elimination from the environment due to its high mineralization efficiency, efficient degradation rate and low toxicity of some catalyst (Trandafilovic et al., 2017; Yu et al., 2017). Ideally chemical reactions are supposed to move to equilibrium quickly however some reactions are quite slow. Reactions, which do not reach equilibrium quickly often require harsh conditions like high pressure and temperature to reach equilibrium.

A catalyst is often used to enable reactions to reach equilibrium at acceptable costs, within a reasonable time frame and with economic yield. The catalyst is not consumed by the reactions but it lowers the activation energy required for the reaction to take place and also accelerates the rate at which equilibrium is reached. Catalysts are divided into two classes according to the relationship between the phases of the catalyst, reactants and products. Homogeneous catalysts are in the same phase as reactants and products and they have high activity and selectivity. The shortcomings for the aforementioned catalysis phase include; difficult to separate from raw materials and products.

Heterogeneous catalysis involves reactions in which catalysts are in different phases with reactants and products. The heterogeneous catalysts are stable and easy to separate from the reaction system after the reaction (Chen et al., 2018). Photocatalysts are metal oxide semiconductors which oxidises chemical processes by the aid of near Ultraviolet (UV) light (>385 nm) irradiation and results in the formation of hydroxyl radicals.

2.2.2 Photocatalysis of Congo red

Congo red dye is a non-biodegradable diazo compound which is fairly stable due to its complex aromatic structure. The dye can be difficult to remove from water due to its high solubility. It has carcinogenic properties, hence it has fatal consequences with effects on skin, eyes, reproductive and respiratory systems (Madan et al., 2019). Congo red is used in wool, silk, textile and food industries. It is also used in medicine as a biological stain for diagnosis of amyloidosis and an indicator in acidic medium (Sasmal et al., 2017).

Congo red has been removed from water using photocatalysts such as PANI nanoarrays anchored on 2D-BiOCl nanoplates (Namdarian et al., 2020), Ru nanoparticles supported on unfunctionalized single walled carbon nanotubes (Hemraj­Benny et al., 2018), copper(1) oxide (Zhang & Yan, 2018), MgZnCr-TiO2 (Ma et al., 2017), LaO8AO.TiO356(A=Ba, Sr, Ca) nanoperovskites (Bradha et al., 2015), TiO?/K (Nan et al., 2009).

ZnO is considered to be a promising photocatalyst however its optical absorption is limited in the UV region. However, it has been shown that doping with transition metals alters its photophysical properties and reduce the band gap energy as well as the rate of electron hole pair recombination, resulting in improved catalytic performance (Huerta-Aguilar et al., 2018).

2.2.3 Factors affecting photocatalysis

Photocatalysis is mainly affected by operational parameters such as initial substrate concentration, initial catalyst dosage, the pH of the aqueous solution.

The rate of a catalysed reaction increases with increasing catalyst loading up to a certain value and beyond that the rate reduces. The reduction is due to an increase in catalyst active sites that will be available for photocatalytic reactions and this occurs up to a point where all the particles of the catalyst are fully illuminated. A screening effect of excess particles occurs at higher concentration of catalyst and this musk the photosensitive surface partially. This masking hinders or reflects the penetrating light and a decrease or conversion to the plateau occurs due to loss of photons (Hapeshi et al., 2010). High concentration of catalyst provides more chance to produce hydroxyl radicals and improves the photocatalytic process whereas excess dosage may hinder the penetration of light (Zhang et al., 2017).

The pH of the solution affects the photocatalytic process by affecting the sorption­desorption process on the surface of the catalyst electrostatic interactions between the surface of the catalyst, substrate molecules and charged radicals formed during the reaction process (Shet & Vidya, 2016).The conversion of substrate by a catalyst decrease with increasing initial substrate concentration because the increased substrate occupies most active sites of the catalyst, which inhibits generation of oxidants (Hapeshi et al., 2010).

2.2.4 Mechanism of photocatalysis

Photocatalysis involves ejecting electrons from valence band (VB) to conduction band (CB) of semiconducting materials creating an h+ holes in valence band. The process is facilitated by UV irradiation of the semiconductor with energy superior or equal to the band gap. An extremely reactive radical (e.g. OH) is formed at the semiconductor surface and direct oxidation of the pollutant adsorbed on the semiconductor occurs e.g. (TiO[2]). The equations for the whole photocatalysis process are shown from equations 2.1 to 2.6 (Zhang et al., 2007),

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The ejected electrons then react with electron acceptors like oxygen dissolved or adsorbed in water, (as shown in Equation 2.5);

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The electrons can also recombine without electron acceptor or donor (Equation 2.6);

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For the doped metallic nanoparticles, the mechanism of excitation is based on Localised Surface Plasmon Resonance (LSPR) in the visible light region. The localised surface plasmon resonance can exhibit a wide spectral range from near ultraviolet to visible to mid infra-red region depending on separation distance, dielectric environment, shape and size of the metal nanoparticles on the semiconductor. Collective oscillation of free electrons to form electron hole areas by surface plasmon of the dopant metal nanoparticles generates transient local electromagnetic fields. When the visible light irradiation is imposed as electromagnetic field the frequencies match and the surface plasmon is excited. An electron from dopant is directly transferred to the conduction band of the semiconductor due to the interband transitions between the semiconductor and plasmonic metal nanoparticles. The surface of the dopant on the semiconductor can act as electron trap and active reaction site (Krukowska et al., 2018).The efficiency of a catalyst is affected by its optical adsorption and charge separation efficiency properties as well as the number of catalytic sites (Shen et al., 2015). Doping of nanoparticles enhances photodegradation by trapping electron and holes, thus reducing electron -hole recombination (Mittal et al., 2014) . Addition of H2O2 and the pH value of the reaction solution plays an important role in the photocatalytic process (Liang et al., 2015).

The efficiency of single metal oxide photocatalysts have limitations of fast electron hole recombination and in order to activate the molecules in sunlight the band gap should be 2.0 eV or below. This presents a challenge when trying to activate the catalyst under visible light or natural sunlight. Doping or mixing reduces the band gap and shifts the adsorption to the visible region thereby increasing environmental application (Rani & Shanker, 2018).

Doping is used to modify nanoparticles’ luminescence, optical and electrical properties of semiconductor nanoparticles by introducing traps and discrete energy states in the band gap of excited electrons (Muruganandam et al., 2017). Doping of nanoparticles enhances photo degradation by trapping electron and holes, thus reducing electron­hole recombination (Mittal et al., 2014). Addition of H2O2 and the pH value of the reaction solution plays an important role in the photocatalytic process (Liang et al., 2015).

The combination of two metals is a strategy used to prepare new materials with improved selectivity or new properties than monometallic ones. This is attributed to synergic effects. The band structure is modified due to decreased orbital overlap as the interatomic distance changes resulting in the density states of the d-band and its position in the Fermi level being affected. Hence the reactivity and adsorption properties of bimetallic nanoparticles are different from either metal considered separately (Rosseler et al., 2015).

2.2.5 Trimetallic nanoparticles as photocatalysts

Trimetallic nanoparticles have higher outstanding catalytic performance when compared with single or bimetallic nanoparticles. However, they can be stabilized by block copolymers, organic ligands, surfactants and dendrimers (Sharma et al., 2017c).

Trimetallic photocatalysts have been widely used to degrade organic pollutants (Table 2:3).

LaCuZr trimetallic nanoparticles have good charge recombination separation therefore making the catalyst a good candidate for photodegradation of organic pollutants (Sharma, et al., 2018). In the Co doped RGO-Bi-TiO2 nanotubes composite, Co doping helped to accomplish 1.5 and 3.8 times higher photocatalytic activity than single doping and undoped TiO2 nanotubes under the same conditions. Bi and RGO were favourable for separation of h+ and electron holes which reduces the recombination of charges and hence promotes the formation of OH radicals (Kim et al., 2017).

Deposition of AuPd nanoparticles on the surface of MoM3 nanowire enhanced the activity of the photocatalyst due to the synergic effect of Au and Pd which results in effective separation of electron and h+ holes as well as charge separation efficiency. The excellent photocatalytic activity can be attributed to the enlarged specific surface area and enhanced stability of the catalyst (Zhang & Park, 2018). CoFe2O4/BiO1 fibre exhibit strong magnetic response to external magnetic fields as well as excellent visible light photocatalytic performance towards the degradation of Rhodamine B regardless of preparatory method, in which h+ and O2- play the major roles (Chang et al., 2019). Ni/Pt doped TiO2 nanophotocatalysts were fabricated and exhibited large surface area as well as reduced band gap. The presence of dopants Ni and Pt did not compromise its porosity. Photocatalytic activity of the doped TiO2 outperformed the non-doped TiO2 (Pol et al., 2016).

Table 2:3 Removal of pollutants using trimetallic photocatalysts

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ZnO and TiO2 have been used as effective non-toxic and inexpensive photocatalyst for the effective degradation of a wide range of organic pollutants in recent years. ZnO has an advantage over TiO2 because it absorbs a larger fraction of the UV spectrum (Sacco et al., 2018). The optical absorption of zinc oxide which is a promising photocatalyst is limited to the UV region. However, it has been shown that doping with transition metals alters its photophysical properties and reduce the band gap energy as well as the rate of electron-hole pair recombination, resulting in improved catalytic performance (Huerta-Aguilar et al., 2018).

Cerium oxide (CeO2) has a band gap of 3.19 eV and it is a semiconducting material with a large exciton binding energy. CeO2 is used in pharmaceutical industry, catalysis, biosensors, electronics and drug delivery. It is an ideal for photocatalyst because of its strong light absorption. CeO2 materials have fast electron-hole pair regeneration under light illumination and a longer lifetime (Sharma et al., 2017b).

Zirconium dioxide ( ZrO2) absorbs a small fraction of light hitting its surface because it has a large band gap of 5.0 eV. ZrO2 has biological and environmental compatibility, high redox potentials of photogenerated e-and h+ pairs, good chemical and optical stability, which renders its suitability for photocatalytic reactions. ZrO2 has been modified with rare earth metals, transition metals and non-metals in order to achieve charge separation and photocatalytic reactions using lower electronic photons belonging to the visible light spectra (Dodson et al., 2011; Gionco et al., 2019). Inserting Zirconia into the ceria lattice can improve the lattice oxygen mobility resulting in a better redox quality (Pradeep et al., 2015).

The doping of transition metals with phosphorous atom into the crystal structure has been widely studied recently and studies show that phosphorous enhances the catalytic activity of the catalyst by drawing electrons from metal centres. The d-states at Fermi lever of the electronic structure of metal centre can be modified by the phosphorous atom with abundant valence electrons (Du et al., 2016)

2.2.6 Kinetic models

A catalyst increases the rate of a chemical reaction but does not appear in its stoichiometric equation. There are three classes of catalysis namely heterogeneous, homogeneous and enzyme catalysis. Enzyme catalysis is a special case of homogeneous catalysis and occurs in biological system. In heterogeneous catalysis the reaction occurs on the boundaries between two phases usually on the surface of the catalyst. Kinetic study is crucial because it describes the uptake of Congo red oxidation and controls the residual time of the process. Kinetic studies are represented by mathematical equations which describe how the concentration of reagents affect the rate of reaction. These equations include the pseudo zero order, pseudo second order and the Langmuir-Hinshelwood (L-H) kinetic model. The change in concentration is linear for reaction which follows pseudo zero order kinetics. The model is represented by equations 2.7 (Nan et al., 2009) .

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The Langmuir-Hinshelwood model describes catalysed reaction following pseudo first order kinetics at trivial initial concentration. The rate of change in concentration of reactants against reaction time is directly proportional to the remaining concentration of reactants in the system for pseudo first order kinetics because of the existence of a relatively small catalyst population relative to the number of degrading molecules. Equation 2.8 shows pseudo first order kinetics rate equation (Shoueir et al., 2018) and it was used to analyse the removal rate,

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and the integral form is shown in Equation 2.9 (Sravanthi et al., 2019).

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where C0 is the initial concentration, C is the concentration at time t, kapp is the apparent first order rate constant which is determined from the slope of the plot of ln Illustrations are not included in the reading sample vs t and it also gives the rate of photocatalytic degradation (min-[1]) and the higher the rate the faster the reaction (Mohanan et al., 2019). The half-life for the pseudo first order reaction is calculated using Equation 2.10.

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For a pseudo second order kinetic model the rate of concentration change is proportional to the square of the concentration at that particular instant, the differential equation for a second order photokinetic degradation is shown in Equation 2.11 (Wang, 2018).

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The pseudo second order model is represented by Equation 2.12 (Maldonado-Larios et al., 2020),

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where qt is the amount of dye adsorbed at time t per unit of catalyst (mg/g), k2is the pseudo-second order rate constant (g/mg/min), qe is the amount of dye adsorbed at equilibrium per unit of catalyst (mg/g). A plot of t/Qt vs t produces a straight line and the rate constant is calculated using the gradient of the slope.

Langmuir-Rideal kinetic mechanism (Equations 2.13-2.15) (Turolla et al., 2012) occurs when two substrates react with each other and only one reactant is adsorbed. This mechanism means that the other substrate in the fluid phase must collide with the adsorbed molecules without first being adsorbed

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The first order kinetics equation specifies that the rate of concentration decline is proportional to the concentration in the system. The time taken for a decrease in concentration by a certain percentage is constant and independent of the initial concentration of the one reactant or there is no significant reverse reaction. [C]o is the initial substrate concentration (mg/L), k lh (mg/L) is the Langmuir-Hinshelwood kinetic constant, k0 (mg/L/min) is the zero-order kinetic constant, Ka (L/mg) is the adsorption constant at equilibrium, K, (min) is the first order kinetic constant

2.3 Solid Phase Extraction

2.3.1 Background to solid phase extraction

Analytical laboratories are under pressure to carry out analysis at lower cost and short turnaround time. The rate determining step is sample preparation which is required to accommodate lower technical skills, provide cleaner extracts for the instrument measurement, provide more accurate and reproducible results, decrease the use of solvents and has a short turnaround time at less cost.

Sample preconcentration is the process of increasing an analyte concentration before analysis to enhance detection and quantification and it is used when complete recovery of analyte is desired and the analyte is transferred in such a manner that its concentration is increased. Separation techniques are used to preconcentrate analytes present in different sample matrix. Analytes and interferents can only be separated if there are significant differences in their chemical and physical properties.

2.3.2 Methods used to enrich analytes

Solid phase extraction (El-Sheikh et al., 2019; Yang et al., 2020), reverse phase dispersive liquid- liquid microextraction (Ozzeybek et al., 2020a), ultrasound-assisted surfactant enhanced emulsification microextraction (Yao et al., 2018), liquid phase microextraction (Karimi et al., 2015), mixed cloud point/solid phase extraction (Nekouei et al., 2016) have been used to enrich analytes.

Separation based on size includes filtration, dialysis, size exclusion chromatography and in these techniques, separation is achieved using a porous medium through which only the analyte or interferents passes through. Separation based on mass or density makes use of centrifugation to separate analytes.

Liquid-liquid extraction used to play a major role in sample clean-up and concentration in the past, however it has its shortcomings like being labour intensive and slow, recovery of sample components being incomplete and discharge of a large amount of solvent to the environment.

Solid phase extraction has shown to be a good replacement since it can be easily automated, is more efficient than liquid-liquid extraction, it is faster and less solvents are used. In solid phase extraction, the absorbing material is a suspension of solid particles in an aqueous sample. In order to have a rapid transfer of extracted solutes from one phase to another a large interfacial area is needed between the particles and sample solution. Column solid phase extraction where the liquid sample comes into intimate contact with the solid particles is more common than the batch mode. Solid phase extraction is the ideal method for sample preparation since it involves preconcentration, extraction and clean up procedures being performed in a single step. The advantages of micro solid phase extraction include low sample consumption, high concentration factors, excellent reproducibility, simplicity of operation and short extraction time (Ghorbani et al., 2020).

One of the most challenging parts of solid phase extraction is development of innovative micro-extraction materials which meets many requirements such as selectivity, stability, low costs, repeated use and versatility (Hakova et al., 2019).

2.3.3 Factors affecting solid phase extraction of samples

Solid phase extraction efficiency is affected by sample load volume, conditioning solvent, pH of solution, extraction time and elution solvent. The pH of solution influence the extraction forms of targets as well as surface binding sites of the adsorbent (Jia et al., 2017). Nano-adsorbents have a very high surface area to volume ratio and their short diffusion routes lead to a highly rapid adsorption process. Furthermore, equilibrium between sample solution and adsorbent surface is reached in a short contact time in comparison with other SPE sorbents (Parham & Saeed, 2014). Elution solvent volume determines the maximum achievable enrichment factor for the tested compounds and the volume should ideally be as low as possible while offering a reproducible and quantitative elution of the analytes. The choice of solvent depends on polarity of the substances to be eluted and the principle of solubility which states that like dissolves like (Cao et al., 2015). The enrichment factor is directly affected by the sample volume and an increase in sample volume results in increase in enrichment factor until equilibrium between solute and adsorbate is attained (Rashidi Nodeh et al., 2017).

2.3.4 Studies on enrichment of heavy metals using Solid Phase Extraction

Solid phase extraction can be carried out in batch equilibrium or in mini-column packed with solid particles (Han et al., 2014; Martínez et al., 2013). Alumina supported on graphene oxide nanocomposite was used as a nanosorbent for Dispersive Micro­Solid Phase Extraction (DMSPE) of As (V) and Cr (III) preconcentration. It proved to be a good sorbent with a good recovery of between 92-108 % and precision of 2.7 to 4.0 %. A combination of DMSPE and Energy Dispersive X-Ray Fluorescence (EDXRF) analysis was used for direct measurement of samples without the elution step (Baranik et al., 2018). A polystyrene polydimethyl siloxane polymer was loaded into a micropipette tip of a syringe as a sorbent for miniaturised solid phase microextraction. Less amount of sample and elution reagents were required. The adsorbent is free of chemical interference and has high adsorption capacity (Ali et al., 2016). Magnetic iron cobalt/silica nanocomposite was used as a sorbent for the enrichment of arsenic using micro solid phase extraction. The combination of Inductively Coupled Optical Emission Spectroscopy (ICP-OES) and preconcentration proved to be a sensitive and an effective method for determination of arsenic in river as well as tap water. The method is only suitable for total arsenic not speciation (Magoda et al., 2016). Magnesium oxide-based adsorbent was used for preconcentration and determination of As by graphite furnace atomic adsorption spectrometry (GFAAS). The sorbent proved to be effective for As preconcentration in real water samples when HNO3 was used as an eluent. The preconcentrated As was successfully transferred into the GFAAS without other matrix modifiers needed (Qiang et al., 2017). Solid phase extraction is summarized in detail in Table 2:4.

The concentration of Cd and Pb in the majority of samples is usually around the detection limit of the most sensitive analytical techniques. Accurate determination of these metals is a very important goal for analytical chemists, hence the aim of most researchers is to improve the analytical potential of the different analytical techniques (Krawczyk & Jeszkaskowron, 2016).

Table 2:4 Solid phase extraction of heavy metals using various sorbents

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Adsorption is usually employed as a polishing step to remove inorganic and organic contaminants in wastewater and water treatment. However, the adsorption efficiency of conventional sorbents is usually limited by the active sites, surface area, lack of selectivity and the adsorption kinetics. Nanomaterials are better sorbents with their short intraparticle diffusion distance, tuneable pore size and surface chemistry, extremely higher specific surface area and associated sorption sites (Qu et al., 2013; Zhao et al., 2018 ).

2.3.5 Adsorption isotherms

Adsorption isotherms are generally used to describe adsorption processes and they include Langmuir, Freundlich and Dubinin-Radushkevich isotherm models. The Langmuir isotherm model describes the equilibrium between the amount of solute absorbed per unit mass of adsorbent and the remaining solute in the solution at low surface coverage. It assumes a monolayer homogenous adsorption, identical energy of sorption for all sites, independent of coverage binding energy and absence of interaction between adjacent adsorbate molecules. The non-linear form of the Langmuir isothermal model can be expressed as equation 2.16 (Nanta et al., 2018),

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Where qmis maximum monolayer adsorption (mg/g adsorbent), b is the Langmuir equilibrium constant (L/g adsorbent). The linearized form of the Langmuir isotherm can be expressed by equation 2.17 (Yoosefian et al., 2017),

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A plot of — versus Ce whose slope and intercept are used to determine values of Langmuir constant qm and b.

A dimensionless constant separation factor RL is used to express the essential characteristics of the Langmuir isotherm as shown by equation 2.18 (Pathania et al., 2016),

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where Co is the initial adsorbate concentration (mg/L), the RL value represents the nature of adsorption process which is favourable (0<RL< 1), unfavourable (RL>1), linear ( RL=1) and irreversible ( RL = 0)

The Freundlich isotherm model describes a multilayer heterogeneous adsorbent surface with different adsorption sites and the non-linear form of the model is given by equation 2.19 (Nodehi et al., 2020),

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where KF is the Freundlich adsorption capacity (mg/g adsorbent) and 1/n is the surface heterogeneity parameter. The linear form of the Freundlich equation is represented by equation 2.20 (Pathania et al., 2016),

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the intercept value of KF and the slope of 1/n are estimated from the plot of lnqe versus lnCe.

The Dubinin-Radushkevich -model accounts for the effect of the porous structure of the adsorbent on adsorption and it’s represented by equation 2.21

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The linear equation of the Dubinin-Radushkevich model is represented by equation 2.22-2.23 (Nishikawa et al., 2018)

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overall, the equation can be rewritten as equation 2.24

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the parameters can be obtained by plotting lnqe against In2 Illustrations are not included in the reading sample , the slope of the curve = -KdrR2 T2 and lnqDR gives the intercept, the mean adsorption energy E is obtained by equation 2.25

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where the adsorption energy is related to the constant KDR (mol[2]/kj[2]),qDR(mg/g) is the adsorption capacity. e is the Polanyi potential, R is the gas constant, T is the temperature in Kelvins.

CHAPTER 3 : PRELIMINARY STUDIES

3.1 Preparation of the aqueous leaf extract

Flacourtia indica leaves (Figure 3.1) were collected during the summer of 2021 from Mutoko in Zimbabwe (32.22, 32° 13” 30.17 E -17.41, 17° 24’ 34.26” S). The leaves were washed with deionised water three times to remove dirt and dried in a shade for a week. The leaves were ground into a fine powder using a blender and sieved using a 200 gm sieve. 20 g of the plant leaf powder were dissolved in 0.5 L deionised water and heated for 0.5 hours at a temperature of 100 C using a heating mantle. The resulting water/ F. indica powder mixture was vacuum filtered with the aid of a 0.45 gm filter paper and the brown extract stored at 4 C in fridge before use. The obtained extract was used without further dilution (Soto-Robles et al., 2019).

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Figure 3:1 A: Flacourtia indica plant .

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Figure 3:2: F indica plant aqueous leaf extracts (A) and P —ZrO2CeO2ZnO nanoparticle solutions (B) at different pH.

3.2 Synthesis of P — ZrO2CeO2ZnO nanoparticles

300 mL of Zn (NO3)2.6H2O was added to 1200 mL of F. indica plant extract and heated for 0.5 h. ZrOCl2.8H2O and Ce (SO4)2.4H20 salts were subjected to the same conditions as Zn (NO3)2.6H2O. 25 mL of Hydrophosphorous acid (concentrated) solution (25 mL) was slowly added to the reacting mixture vigorous stirring. The solution was boiled until minimum liquid remains. The semi liquid containing the nanoparticles (Figure 3:2 B) was dried using an oven and a muffle furnace at 800 °C to get the P — ZrO2CeO2ZnO nanoparticles. The effect of leaf dosage concentration was determined by adding 1-5 g of the leaf powder in 100 mL deionized water to a constant concentration of metal salt solution, constant temperature and pH. The effect of metal salt concentration was determined by varying the metal concentration from 0.05 to 0.5 M and keeping temperature, leaf concentration and pH constant.

3.3 Optimization of synthetic conditions

The optimization of the synthetic conditions for green synthesis of P — ZrO2CeO2ZnO nanoparticles were carried out using the Taguchi experimental design. The independent variables which were optimized were pH., dosage, metal concentration and volume ratio. The experimentally recorded response (absorbance and signal/noise ratio) from 16 runs of the optimization are shown in Table 3:1. The optimum conditions which were obtained using the Taguchi design were volume ratio 1:4, pH. 9, dosage 4 g/ 100 mL, and metal ion concentration 0.05 M.

Table 3:1: The Taguchi design for the optimization of P —ZrO2CeO2ZnO nanoparticles synthesis.

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CHAPTER 4 : METHODOLOGY

4.1 Chemicals and materials

All the chemicals used during the study quality was analytical grade unless otherwise stated and used as provided. Flacourtia indica leaves, zirconyl chloride octahydrate ZrOCl2.8H2O 99.5% (Riedel-De Haen Ag Sleeze Hanover), zinc nitrate hexahydrate Zn (NO3)2.6H2O 99.5%, (Merck, RSA), cerium (IV) sulphate hydrate Ce (SO4)2.4H20 98%, (Merck, RSA), phosphoric acid (Merck, RSA), phenol (Riedel-de-Haen. AG), methanol (Avonchem, UK), propanol (ACE, RSA), sodium hydroxide NaOH (Glassworld, SA), hydrochloric acid), HCL, (Merck, RSA) (Reagent grade), disodium Ethylenediaminetetraacetic acid (Merck, SA), potassium dichromate (Merck RSA), phenol liquid (91%) (Riedel-de-Haen.AG), Sodium alginate (Sigma Aldrich USA), cadmium chloride hydrate (Sarchem, RSA), lead nitrate (Skylab’s, SA), phenol (91%) (Riedel-de-Haen, AG), methanol (Avonchem, UK), propan-2-ol (ACE, RSA), phosphoric acid (Merck, RSA), calcium chloride (Merck, RSA), arsenic oxide ( As2O3), phosphoric acid, Merck (RSA), calcium chloride (Saarchem, RSA) (reagent grade). Na2EDTA (Merck, SA), C32H22N6O6S2Na2C32H22N6O6S2Na2- Congo Red (Merck, RSA), As2O3, (Sarchem SA) and deionised water.

4.2 Equipment

The morphology of the P — ZrO2CeO2ZnO nanoparticles and P — ZrO2CeO2ZnO nanoparticles/alginate beads was determined by Scanning Electron Microscope (SEM) (Auriga Zeiss, Germany). SEM determines size, shape and surface morphology with direct visualization of nanoparticles. The nanoparticles powder was mounted onto a sample holder followed by coating with a conductive material using a sputter coater. Analysis is carried out by scanning the whole sample with a focused fine beam of electrons. The surface characteristics of the sample are determined by secondary electrons which are emitted from the sample surface. SEM provides limited information about the true population average and size distribution (Mourdikoudis & Pallares, 2018)

The size of the nanoparticles was determined using Transmission Electron Microscope (TEM) (Tecnai F20, FEI company, USA). TEM is used to determine size, shape and surface morphology of particles. Nanoparticles were deposited onto films or support grids and after dispersion they were fixed by plastic embedding. Fixing was done to make nanoparticles withstand against the instrument facilitate handling or vacuum. When the beam of electrons is transmitted through the ultra-thin sample it interacts with the sample as it passes through it. A diffraction pattern is formed when the transmitted and diffracted beams combine on a fluorescent screen. The information regarding lattice spacing and symmetry of the structure is given by the diffraction pattern (Mourdikoudis & Pallares, 2018).

The leaves were ground the leaves to fine powder using a Blender (HE-House). The synthesized nanoparticles were dried using a Muffle furnace (Carbolite, England). The crystallinity of the nanoparticles and beads was determined using X - ray Diffraction (XRD), D2- Phase Diffractometer, (Bruker, Germany).

XRD is an analytical technique for examining crystalline solids and it operates based on the Bragg equation (equation 4.1)

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where n is the order of reflection (n G (1,2,3...), d is the interplanar spacing, A is the wavelength, 0 is the Bragg angle which is the angle between the incident beam and lattice plane. A collimated beam of X-rays is directed at the sample and the angle at which the beam is diffracted is measured. The information regarding the crystal nature of the substance is given by the angle of diffraction which differs from that of the incident beam (Dahman, 2017).

The nitrogen adsorption and desorption properties as well as BET surface area were determined using Tristar II Plus surface and porosity analyser from Micrometrics (USA). BET technique was developed by S. Brunauer, P.H Emmet and E. Teller in 1938 and they named it Brunauer-Emmet-Teller analysis. It is used to determine surface areas of the solids by measuring nitrogen adsorption at -I96X (Mallard et al., 2015). The Brunauer-Emmett-Teller equation (Equation 4.2) is utilized to estimate the surface area from nitrogen adsorption isotherms (Song & Jhung, 20I7)

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Where P is the equilibrium pressure of adsorbate, P0 is the saturation pressure of adsorbate at temperature of adsorption. Va is the volume of gas reduced (at standard temperature and pressure), Vm is the gas uptake corrected to standard temperature and pressure, C is a constant related to energy of adsorption, A plot of Illustrations are not included in the reading sample gives a straight line with an intercept Illustrations are not included in the reading sample , C and VmC can be obtained from the plot and Vm can be calculated and used to determine specific surface area using equation 4.3,

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Where Vm is the gas uptake corrected to standard temperature and pressure, o is the average area occupied by the adsorbed molecule in Angstrong’ squared, N is the Avogadro’s number, Vois the ideal gas volume, W is the weight of the sample (g), Vm is found by determining the volume of the adsorbed gas (reduced to standard temperature and pressure) at a number of equilibrium relative pressure by use of BET equation.

The functional groups of the nanoparticles and beads were determined using Fourier Transform -Infra Red Spectrometer with Attenuated Total Reflectance (ATR-FTIR, Thermo-fisher scientific). FT-IR is an absorbance analysing technique which measures the amount of light at different wavelength that is absorbed by a sample and express the measurement in a spectrum. Different materials absorb and transmit different range and levels of light and each has its unique spectrum. FT-IR utilizes the Michelson interferometer which separate radiant beams and direct them through different optical paths and then recombines them in order to produce repetitive interference signals which are measured as a function of optical path difference by the detector. Infrared spectral information is generated by the interferometer after radiant beams pass through the sample. The technique can be used to analyse characteristics such as film thickness, optical properties of nanoparticles (Shea, 1998).

The acidity of the reactions was monitored using a pH meter (Adwa AD 1020- Romania). The source of light for photodegradation of Congo red was a Light Emitting Diode (LED) (Panasonic). The nanoparticles were recovered using a Centrifuge 5702 R, (Eppendorf) during synthesis. The liquid solution was driven through the column using a peristaltic pump (Eyela, Model: Microtube MP-3, Japan). The metal content was used to determine using an Agilent ICP-MS 7800 (Agilent Technologies-Australia). The band gap was determined using Genesis 10s UV-Visible spectrometer (Thermo-Fisher Scientific Co.). Ultraviolet-visible (UV-Vis) spectra are produced when incident radiation and the electrons in a chromophore interacts and results in an electronic transition involving the promotion of one or more of the outer shells from a ground state into a higher energy state. UV-Vis spectroscopy is used to measure the number of discrete wavelengths of ultra violet or visible light that are absorbed by or transmitted through a sample in comparison to a blank sample. Information on what is in the sample and at what concentration is obtained based on the absorption or transmittance property. The amount of light absorbed by the sample is quantitatively related to the concentration of the sample. The Beer-Lambert's law is used to obtain the concentration of the substance. It can be defined as the absorption of light is directly proportional to the path length and concentration of the substance. The Beer-Lambert's law is often applied when the path length of the light is known and the molar absorptivity and can be represented by equation 4.4

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Where c is concentration of the sample in mol/L, A is the absorbance and has no units and £ is the molar absorptivity in L/mol/cm and b is the path length in cm (Settle, 1998).

The solutions for absorption studies were stirred using an Orbital shaker (Griffin, Model: CTR, German). The Congo red dye was stirred using Magnetic stirrer (Stuart Scientific, Model: SM3) during photocatalysis. Nanoparticles and beads were dried using drying Oven (Biobase, Model: BOV-V4SF, China).

4.3 Preparation of stock solutions

Preparation of metal salts was carried out as follows; 0.05 M Cerium was prepared by dissolving 20.23 g of Ce (SO4)2.4H20 in 1 L of deionized water, 0.05M. Zirconium was prepared by dissolving 16.11 g of ZrOCl2.8H2O in deionized water and 0.05M Zinc was prepared by dissolving 14.87 g of Zn (NO3)2.6H2O salt in 1 L deionized water.

Arsenic (III) stock solution was prepared by dissolving 1.32 g As2O3 in 20 mL 1.0 M NaOH in a 1000 mL volumetric flask. The resulting solution was topped to the mark using deionised water. As (III) was converted to As (V) by adding 1 mL of 0.01 M KMnO4 for every 2.5 mL of As (III). The solution was stirred for a minute and left to undisturbed for 24 hr and filtered afterwards.

The amount of metal salts needed to prepare 1000 ppm metal solution was determined by the molecular weight of the salt by the molar mass of the metal. The stock solution was prepared by dissolving 0.509 g CdCL2, 0.3995 g PbNO3 in 250 mL deionised water. This solution was further diluted to prepare the other required concentrations.

4.4 Synthesis of the P — ZrO2CeO2ZnO nanoparticles

Flacourtia indica leaves were collected during the summer of 2021 from Mutoko in Zimbabwe (32.22, 32° 13” 30.17 E -17.41, 17° 24’ 34.26” S). The leaves were washed with deionised water three times to remove dirt and dried in a shade for a week. The leaves were ground into a fine powder (200^m) using a blender. 20 g of the plant leaf powder were dissolved in 0.5 L deionised water and heated for 0.5 hr at a temperature of 100C using a heating mantle. The resulting water/ F. indica powder mixture was vacuum filtered with the aid of a 0.45 gm filter paper and the brown extract stored at 4°C in fridge before use. The obtained extract was used without further dilution (Soto- Robles et al., 20I9).

The independent variables that affect the synthesis of the nanoparticles such as pH, plant extract dosage, initial metal concentration and plant extract to metal salt volume ratio (Mittal et al., 20I4) were optimized using the Taguchi experimental design. The variables used during optimizations were pH (3, 6, 9, I2), plant dosage (2, 3, 4, 5 g), initial metal concentration (0.05, 0.I, 0.2, 0.5 M), plant extract to volume ratio (I:2, 1:4, 2:1, 4:1. 300 mL of each metal salt solution (ZrOCl28H2O, Zn(N03)26H20 and Ce(S04)24H20) were added to 1200 mL of F. indica leaf extract sequentially and heated for 0.5 hr at 100°C. All salts were subjected to the same conditions. Concentrated Hydrophosphorous acid solution (25 mL) was added drop wise to metal salts under vigorous stirring in order to further dope the composite using phosphorous (Du et al., 2016). The solution was boiled until minimum liquid remains. The semi liquid containing the nanoparticles was oven dried and then the solid was then calcined at 900OC to get the oxide nanoparticles (Vidya, et al., 2017). The optimized conditions were then used to synthesize the nanoparticles before characterization.

4.5 Preparation of P — ZrO2CeO2ZnO nanoparticles/alginate

beads

P — ZrO2CeO2ZnO nanoparticles were synthesized by the method described in section 4.4. The alginate beads were formed by mixing 4 g P — ZrO2CeO2ZnO nanoparticles with 100 mL of 2 % w/v sodium alginate at room temperature for 4 hours using a magnetic stirrer (Figure 4:1). CaCl2 (20 mL of 0.1M) was slowly added to the solution with stirring using with a magnetic stirrer. The beads were placed in 2 M CaCl2 solution for 12 hours at room temperature to allow for curing. Shrinking of the microcapsules was induced by oven drying at 60 °C for 24 hours.

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Figure 4:1: (a) P — ZrO2CeO2ZnO nanoparticles/alginate beads being extruded from syringes and (b) wet alginate beads in a petri dish

4.6 Characterization of the P — ZrO2CeO2ZnO nanoparticles

The surface plasmon resonance of the nanoparticles composite was characterized using a UV-Vis Spectrophotometer at a wavelength of 180-800 nm. Distilled water was used as a blank. The functional groups responsible for bio-reduction of the metal ions were characterised by Fourier Transform-Infra-red spectrometer operated at a resolution of 2cm-[1], and scanning from 4000- 400 cm-[1] and an average of16 scans. FTIR was carried out on P — ZrO2CeO2ZnO nanoparticles and the F. indica plant extract. The chemical composition of the nanoparticles was determined using Energy Dispersive Spectrometer (EDX) on Scanning Electron Microscopy (SEM). The crystallinity of the nanoparticles was determined using a D2-Phaser X-Ray diffractometer using Cu K (a=1.5406) radiation. The samples were scanned continuously at 29 from 10 - 90°. The samples placed on the sample holder were fine powder only.

Brunauer-Emmet-Teller (BET) surface area analysis was used to determine the surface area of both nanoparticles and beads. A 300 mg quantity of the nanoparticles and bead was used for surface area analysis. The pore size distribution was obtained from a plot of pore size versus incremental pore volume. The total pore volume was determined from a plot of pore size versus pore volume.

The surface morphology analysis was carried out on a Scanning Electron Microscopy instrument at an acceleration of 200 V and a working distance of 6.3 mm. The P — ZrO2CeO2ZnO nanoparticles were scanned and observed after being deposited on SEM specimen stabs. The size of the nanoparticles was determined using Transmission Electron Microscopy at 20-200 kV. The nanoparticles suspension was placed on a carbon coated TEM grid and the equipment was operated at 200 kV.

X-Ray Photoelectron Spectroscopy (XPS) was used to study the surface composition and the oxidation states of the elements of the P — ZrO2CeO2ZnO nanoparticles. The analysis was performed using Kratos axis ultra with DLD equipped with monochromatic X-ray source (E=1486.6 eV) running at 225 V. The photoelectron take-off angle to the sample surface was at 46°. The electron detector was set perpendicular to the sample to avoid the shadowing effect of the ion gun at one side of the particles.

4.7 Determination of the metal’s concentration in P ZrO2CeO2ZnO nanoparticles

A weighed amount of material containing the suspected nanoparticle sample was dissolved in 20 mL of 1 M HNO3/HC1 and boiled until minimum volume was left. The sample was toped up to 25 mL using deionized water and filtered. The concentration of metal elements was determined using an Agilent ICP-MS 7900 (Agilent Technologies-Australia). The operating conditions were: with incident RF power- 1550 W, carrier gas flow rate- 1 L/min, plasma gas flow rate -15 L/min, machine warmup- 1500s, replicate analysis - 3, plasma mode-low matrix, tune mode -He.

4.8 Studies of kinetics and reaction mechanisms for photocatalytic degradation of Congo red using P — ZrO2CeO2ZnO nanoparticles photocatalyst

Congo red was used as a test dye to study the photocatalytic activity of P — ZrO2CeO2ZnO catalysts. Adsorption-desorption equilibria were achieved by dispersing the 1 g/L of the P — ZrO2CeO2ZnO catalyst in 10 mg/L of Congo red dye solution and stirring in the dark for 0.5 hours before being subjected to UV led warm white light (Figure 4.2). At 0.5 hour intervals, 4 mL aliquots were taken and the suspended catalyst was removed by centrifugation at 2500 rpm for 5 minutes. Quantification of the degraded dye was carried out using a UV-Vis spectrophotometer at 562.9 nm. The amount of Congo red degraded was calculated using Equation 4.5 (Yoosefian et al., 2017),

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where Co is the initial Congo red dye concentration prior to illumination with LED white light, Ct is the Congo red dye concentration after illumination with LED white light at time t.

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Figure 4:2. A) The LED warm white light coiled around the beaker photoreactor B) the complete photoreactor used during decolourization experiments consisting of LED light and the beaker wrapped with aluminium foil on a magnetic stirrer.

4.9 Enrichment of cadmium and lead

About 100 mg of P — ZrO2CeO2ZnO nanoparticle/alginate beads were loaded into a 5 mL syringe that was covered with glass wool at the bottom (Figure 4:3). The sorbent was prewashed using 0.1 M HNO3 and deionised water before loading the sample. The model solution consisting of 10 gg/L Pb and Cd was prepared using deionised water and pH was adjusted using 0.1 M HNO3 and 0.1 M NaOH. In this study a screening step to determine the significant variables was carried out using a Half Factorial Design (HFD) experimental design followed by optimization of the significant variables using the Taguchi design. The conditions used during the optimization experiments were amount of adsorbent (50, 100, 150 mg), sample volume (10, 50, 100 mL), sample pH (3, 6, 9), eluent volume (10 mL), eluent concentration (0.5, 1.0 and 2.0 M), eluent flow rate 3 rpm and sample flow rate 2 rpm were used during the optimization experiments. Recovery studies using real samples were used to assess the extraction efficiency from the syringe column. The retained metals were eluted using HNO3 from the syringe column and diluted prior to ICP-MS analysis. HNO3 was chosen as the sole eluent since it does not cause much interference in ICP-MS. ANOVA was used to determine the effect of parameters on sorption. The optimum eluent concentration was investigated by passing 10 mL of 0.5, 1.0, 2.0 M HNO3 through the loaded column and the one with highest desorption was used as the eluting acid. After desorption, the adsorbent was washed with the eluting acid before each new extraction cycle.

The effect of desorption conditions on the release of the metals from the surface of the beads was investigated using extraction recovery (ER %). The optimized procedure was applied on recovery of spiked cadmium and lead for well and borehole water samples. The enrichment factor (EF) was determined by calculating the ratio of concentration of the lead and cadmium in the final extract to the initial concentration in the aqueous phase with and without the P — ZrO2CeO2ZnO nanoparticle/alginate as shown in Equation 4.6 (Li et al., 2017),

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Extraction recovery (ER) was determined using the ratio of eluted to initial concentration by the Equation 4.7 (Ali et al., 2020a),

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Where Cdes, Co, Cdes, Vdes and Vo are the analyte concentration in the extraction solvent, analyte concentration in the sample, extraction solvent volume and sample volume.

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Figure 4:3: (A) P — ZrO2CeO2ZnO nanoparticles/alginate beads loaded onto syringe tips and covered by glass wool (B) Sample reservoir, peristaltic pump and syringe setup used during solid phase experiments.

The developed solid phase extraction method was applied on borehole and well water samples. The water samples were collected in clean empty plastic containers with filtration using a 0.45 gm filter paper. The collected water was acidified using 1 M HNO3 in order to preserve it. The samples were stored at 4 °C.

4.9.1 Adsorption studies

The adsorption capacity of P — ZrO2CeO2ZnO /alginate nanocomposite was determined using batch studies on an orbital shaker. Equilibrium adsorption experiments were carried out with initial concentration ranging from 10-100 mg/L, dosage 150 mg, volume 100 mL and pH 7.0. The solutions were filtered using a 0.45 gm filter paper after reaching equilibrium and quantified using an ICP-MS spectrometer. The adsorption capacity at different concentrations was determined using the Equation 4.8 (Huang et al., 2018),

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where qe is the adsorption equilibrium capacity (mg/g), v = solution volume (L), m = the amount of P — ZrO2CeO2ZnO /alginate nanocomposite in grams, Co and Ce are initial and equilibrium concentration of Cd and Pb in mg/L.

4.10 Enrichment of Arsenic and Chromium by pipette tip solid phase extraction

A known amount of P — ZrO2CeO2ZnO nanoparticle/alginate composite beads were loaded on top of a small layer of glass wool in the pipette tip and covered by glass wool on top (Figure 4.4). 1.0 M HNO3 followed by deionized water at a flow rate of 1 mL/min were used to condition the sorbent bed before use in solid phase experiments. 5 iig/L As and Cr solution was prepared from ultrapure water. The variables which are significant for the enrichment of As and Cr were screened for using Pareto analysis and a Half Factorial Design (HFD). A L27 (3[4]) Full Factorial Design (FFD) matrix was used to carry out the optimization step. 1.0 M HN03 or NaOH solutions were used to adjust the pH of the solution to the desired levels. The spiked water samples were passed through the column at a flow rate of 1 mL/min. Nitric acid was used to elute the retained compounds prior to ICP-MS analysis. The desorption step was investigated by vortexing the beads with 10 mL of 0.01, 0.10, 0.50, 1.00 M HN03 and the one with highest desorption was used as the eluting acid. The highest enrichment factor was obtained by investigating the effect of sample volume on enrichment. The experiments were repeated three times in order to obtain reproducible results. The washed beads were used again for a new cycle of extraction. The effect of desorption conditions on the release of the metals from the surface of the beads was determined using extraction recovery (ER%).

The ratio of concentration of the metal ions in the final extract to the initial concentration in the aqueous phase with and without the P — ZrO2CeO2ZnO alginate was used to calculate the enrichment factor (EF) using Equation 4.6.

Extraction recovery (ER) was determining the ratio of eluted to initial concentration by the Equation 4.7,

The adsorption capacity which is used to determine the effect of different conditions on adsorption was determined using Equation 4.8.

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Figure 4:4: Pipette tips loaded with P — ZrO2CeO2ZnO nanoparticles/alginate beads and glass wool

The proposed method was validated in terms of linearity, precision, recovery, limit of detection, limit of quantification and correlation. Calibration curves were obtained over a range of six standards prepared in deionised water and the procedure was used to obtain the method linearity. The precision was determined from the relative standard deviation of five extractions. The sensitivity was determined by establishing the limit of quantification (LOQ) which gives a signal to noise ratio of 10:1 which is derived from equation 4.9.

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Limit of detection (LOD) which leads to the solute concentration that led to signal to noise of 3:1 and is derived from equation 4.10

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where m is the slope of calibration curve and 5b is the standard deviation of the blank.

Recovery tests were performed by spiking effluent and well water in triplicate in order to study the extraction recovery at optimum conditions.

The developed solid phase extraction method was applied on effluent collected in Avondale Harare S17°48’57.3478, E31°2’43.7208 and well water samples from Retreat Waterfalls, Harare, Zimbabwe S17°55’21.17388, E31°3’5.814. Effluent water was collected in Avondale because the sampling point lies at laboratory which produces effluent water from its analysis. The well water sample was from an informal settlement without proper sanitary facilities.

CHAPTER 5 : RESULTS AND DISCUSSION

5.1 Optimization of the method for the green synthesis of P- ZrO2CeO2ZnO nanoparticles using aqueous extracts from Flacourtia indica leaves

5.1.1 Optimization of synthetic conditions

The optimization of green synthesis of P — ZrO2CeO2ZnO nanoparticles was carried out using the Taguchi L16 orthogonal design array and the experimentally recorded response (absorbance and signal/noise ratio) from 16 runs of the optimization are shown in Table 5.1. The optimum conditions for P — ZrO2CeO2ZnO synthesis which were determined using the Taguchi experimental design were leaf extract concentration 4 g/100 mL, pH 9, metal ion salt concentration of 0.05 M and metal to leaf extract volume ratio 1:4. The P — ZrO2CeO2ZnO nanoparticles were then synthesized using the optimized conditions and characterized.

Table 5:1 Optimization of synthetic conditions of P — ZrO2CeO2ZnO nanoparticles.

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5.1.2 Evaluation of interactions and significant factors for the synthesis of P — ZrO2CeO2ZnO using ANOVA

ANOVA analysis of the data obtained from the green synthesis of P — ZrO2CeO2ZnO nanoparticles was evaluated using Minitab Version 18 as shown in Table 5.2 in order to obtain the probable interactions and most important effects between variables. The probability values less than 5 % shows the statistical significance of related effects at 95 % confidence level. The most significant variables with p values less than 0.05 were leaf extract dosage, metal salt concentration and pH. The volume ratio was statistically insignificant because the p value was above 0.05. Minitab statistical software was used to generate the relationship between tested variables and response as shown in Equation 5.1.

Absorbance (response) = 12.0 - 1.35 P + 9.28 D - 134 M+ 9.7 V+ 0.155 P[2]- 0.427 D + 79.6 M[2]- 1.05 V[2] - 0.429 P*D+ 3.57 P*M+ 0.222P*V + 14.5D*M - 2.04 D*V + 5. M*V. [5.1]

where P is pH, D is leaf extract dosage or concentration, M is metal salt concentration, V is metal salt to leaf extract volume ratio.

A positive value in the equation means the factor is enhanced and a factor which is not enhanced is represented by a negative value for the green synthesis of the nanoparticles in Equation 5.1. The synthesis of P — ZrO2CeO2ZnO nanoparticles was enhanced by concentration of the leaf extract, positive interactions between metal salt concentration, pH, volume ratio of the metal ion concentration to leaf extract concentration. Equation 5.1 describes the effect of various factors on nanoparticle synthesis. The R-squared value obtained from ANOVA was found to be 0.9831 suggesting that the model is appropriate for describing the green synthesis of P — ZrO2CeO2ZnO nanoparticles. Dosage or leaf extract concentration is significant since at high concentration segregation can occur and at low concentration unstable nanoparticles are formed.

Table 5:2: ANOVA results for the determination of the most significant factors for synthesis of P — ZrO2CeO2ZnO nanoparticles.

Source DF Seq SS Adj SS Adj MS F P

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5.1.3 Main effects of variables on nanoparticle synthesis

Figure 5.1 shows the main effects of variables such as dosage, pH, metal ion concentration and metal salts to leaf extract volume ratio. Figure 5.1 a show that the mean response decreased as the pH raised from 3.0 to 6.0 then it started to rise again from 9.0 and dropped at 12.0 when all the other factors were constant. The change in pH affected electrical charges of the phytochemicals present in the leaf extracts which in turn affects their capping and stabilizing abilities, hence overall affected the growth of the nanoparticles. A particular pH favoured the formation of nanoparticles of certain shapes in order to achieve greater stability. Change in pH can also result in formation of nanoparticles with different size and shape as well as favour aggregation of nanoparticles to form larger ones or nucleation to form new nanoparticles (Machalova et al., 2013). The reduction process is accelerated by alkaline conditions because under alkaline conditions the a glucose (cyclic structure) turns to P glucose (open chain structure) which is more reactive since it has an exposed CHO group which can readily reduce the metal ions (Kumar et al., 2016) .

The mean response of nanoparticle synthesis increased as leaf extract dosage increased assuming all factors are kept constant (Figure 5.1 b). The concentration of the plant biomass extract used during the nanoparticles synthesis determines the extent of reduction and stabilization which could affect the resulting shapes and sizes of the nanoparticles (Ghodake et al., 2010).

Figure 5.1 c shows that the mean response for nanoparticle synthesis decreased as the concentration of metal salts increased from 0.05 to 0.10 M and it increased again from 0.10 to 0.20 M and then it decreased again as concentration increased from 0.20 to 0.50 M metal ion concentration. At low metal concentration the rate of metal reduction reached its maximum. The reducing agent became the limiting factor when the metal concentration was increased and the reaction reached equilibrium. Figure 5.1 d shows that the synthesis of nanoparticles was only possible when the phytochemicals in the leaf extracts and metal ions were within suitable range for nucleation. The rate of nucleation is mainly affected by the availability of the capping and reducing agents as they determine whether metal precursors will be reduced (Prathna et al., 2011).

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Figure 5:1 The main effects of change in (a) pH, (b) leaf extract concentration or dosage (c) metal ion precursor concentration and (d) metal ion to leaf extracts volume ratio on P — ZrO2CeO2ZnO nanoparticles synthesis.

5.1.4 Evaluation of interactions between influencing factors by response surface methodology for P — ZrO2CeO2ZnO nanoparticle synthesis

The three-dimensional plots were used to determine the interaction between dosage, volume ratio, pH, and metal concentration. Figure 5.2 (a) shows that nanoparticle synthesis decreased as metal ion concentration increases and increases with volume ratio of metal to plant extract. At low concentration the metal is less than the plant extract so all the metal ions are reduced and as the metal ions concentration increases the plant functional groups are saturated. Volume ratio affected nanoparticle synthesis as more reducing agent is available and less metal ions are in solution, thus more active sites are available for reduction of the metal ions to form nanoparticles.

Figure 5.2 (b) shows that nanoparticle synthesis decreased with increase in volume ratio and increased with increase in plant extract dosage. At higher plant extract dosage more, functional groups are available for synthesis than at low dosage and at higher volume ratio the functional groups responsible for reduction are saturated with high metal concentration. Figure 5.2 (c) shows that nanoparticle synthesis decreased with increase in dosage and increased as metal ion concentration increased. The response decreased as dosage increased due to early attainment of equilibrium between plant and metal ions and the response increased as the metal ion concentration increased. Figure 5.2 (d) shows that nanoparticle synthesis increases with a pH increase and decrease with an increase in volume ratio. The observation is due to the increase in reactive sites responsible for reduction of the metal ions. At low pH, the plants functional groups are protonated whereas at high pH they are deprotonated or lose a proton easily and hence can reduce the metal ion to form the nanoparticles. Figure 5.2 (e) suggests that nanoparticle synthesis increase as both pH and metal ion concentration increased. The reason is that at high metal ion concentration more metals ions are available for reduction until saturation is reached. Figure 5.2 (f) demonstrates that nanoparticle synthesis increased as both dosage and pH were increased. This shows that there is interaction between pH and dosage as the increase in both factors resulted in increase in response.

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Figure 5:2: Response surface plot for interaction of (a) volume ratio and metal concentration, (b) volume ratio and dosage, (c) metal concentration and dosage, (d) volume ratio and pH, (e) metal concentration and pH, (f) dosage and pH

5.1.5 Possible reaction mechanism for P — ZrO2CeO2ZnO nanoparticles synthesis

F. indica leaf extracts contain phytochemicals such as alkaloids, ketones, flavonoids, aldehydes, phenols and carboxylic acid ester. All the phytochemicals have free n electrons or hydroxyl groups which are all potential reducing and stabilizing agents for nanoparticles synthesis. Metal salts containing zinc, zirconia and cerium are reduced to Zr[0], Ce[0] and Zn[0] nanoparticles by the reducing agents and free electrons from the plant extracts (Kumari & Meena, 2020). The first step involves complexation between the phytochemicals in the F indica leaf extract and the metal salts. The second step involves formation of a transition complex between the hydroxyl groups of the flavonoids and phenolic compounds and zirconia, cerium and zinc ions. Zero valent nanoparticles are formed when electrons are transferred to the metal ion as shown in Equations 5.2 to 5.4.

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The oxide nanoparticles were formed when zero valent phytochemical stabilized nanoparticles were oxidized at 900 °C as shown in Equation 5.5 to 5.7.

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The other possible reaction involves reducing sugars donating electrons to metal ions which results in formation of zero valent Zr, Ce and Zn nanoparticles directly. An alternative mechanism involves hydrolysis of sugars into their component reducing sugars before the nanoparticles are reduced. The aldehyde group is oxidized to the carboxyl group by nucleophilic addition of the hydroxyl group. The carboxyl group then reduces the metal ions to nanoparticles. The reduction of Zr[4]+, Ce[2]+ or Zn[2]+ to Zr[0], Ce[0] and Zn[0] occurs under basic conditions.

5.1.6 Comparison with other studies

A comparison of the optimization of the synthesis of P — ZrO2CeO2ZnO nanoparticles with other studies is shown in Table 5.3. The results of the P — ZrO2CeO2ZnO nanoparticles synthesis agrees with other studies for total nanoparticle synthesis time and the size distribution of the nanoparticles.

Table 5:3: A comparison of the current study for the synthesis of P — ZrO2CeO2ZnO nanoparticles with other studies.

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In summary the synthesis of the P — ZrO2CeO2ZnO nanoparticles were affected by experimental variables such as pH, metal ion concentration and leaf extract dosage. There is interaction between factors during the synthesis stage and these were between pH and dosage, metal concentration and volume ratio, pH and metal concentration, plant dosage to volume ratio, pH and volume ratio and between plant dosage to metal concentration. The results obtained allow for the selection of the optimum conditions without interactions. The synthesized nanoparticles have active sites for hydrogen bonding on the C — O, P = O, C = O, C = ONH and OH bands which enhances the particles application for environmental remediation such as catalysis and adsorption.

5.2 Characterization of surface composition

5.2.1 UV- Vis Spectroscopy Characterisation

The colour of the P — ZrO2CeO2ZnO nanoparticles changed from brown to yellowish after 1.5 hr of reaction time. The UV-Vis spectrum of the P — ZrO2CeO2ZnO at different pH and concentration in the wavelength range 300 to 900 nm is shown in Figure 5.3. The maximum adsorption occurred from 300 to 350 nm for all samples at different pH and concentrations.

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Figure 5:3: UV-Vis spectrum of the P — ZrO2CeO2ZnO nanoparticles at a. 0.05M nanoparticles at pH 3, 5, 9 and 12, b. 0.1M nanoparticles at pH 3, 5, 9, and 12, c. 0.2M nanoparticles at pH 3, 5, 9 and 12.

The UV-Vis spectra of the P — ZrO2CeO2ZnO nanoparticles (Figure 5.4 a) showed a maximum at 349 nm and the ZrO2CeO2ZnO nanoparticles (Figure 5.4 b) showed a maximum at 300 nm. The bandgap of the P — ZrO2CeO2ZnO nanoparticles was determined using Ultraviolet Diffuse Reflectance Spectroscopy (UV-DRS) analysis. The optical band gap was determined using the equation 5.8,

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Where a is the absorption coefficient, E(hv) is the photon energy E (hv), A is a constant, n=1/2 is a directly allowed transition, n=2 is an indirectly allowed transition (Soto-Robles et al., 2019). The optical band gap energy was determined using Tauc plots where (a hv)n vs hv were plotted as shown in Figure 5.4 c-f. The experimental determined bandgap of the P — ZrO2CeO2ZnO nanoparticles was found to be 2.4 eV (Figure 5.4 c). The bandgap for the ZrO2CeO2ZnO nanoparticles determined experimentally was found to be 2.65 eV (Figure 5.4 d). Results of the study suggests that phosphorous doping can reduce the optical band gap and hence improve the catalytic properties of the photocatalyst.

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Figure 5:4 UV Vis spectrum of (a) P —ZrO2CeO2ZnO nanoparticles and (b) ZrO2CeO2ZnO nanoparticles and determination of band gap (c)and e) for P — ZrO2CeO2ZnO nanoparticles at n=2 and n=1/2 respectively and (d) and (f) for ZrO2CeO2ZnO nanoparticles at n = 2 and n=1/2 respectively.

5.2.2 Fourier Transform Infrared Spectroscopy (FT-IR)

The role of phytochemicals in green synthesis of P — ZrO2CeO2ZnO nanoparticles was investigated using FT-IR analysis. The spectrum of the F. indica leaf extract is shown in Figure 5.5 a. The presence of the O — H group in the leaf extract is attributed to phenolic compounds and is confirmed by a band at 3285 cm-[1] (Ramezanpour et al., 2019) and a medium band at 2917 cm-[1] represent the C — H stretch of alkanes (Sharmila et al., 2017). A small band at 1706 cm-[1] is due to the C = O stretch of a and P unsaturated aldehydes and ketones (Repo et al., 2011) and the other small band at 1024 cm-[1] is due to the C — O of carboxylic acid ester (Shahwan et al., 2011).

The P — ZrO2CeO2ZnO nanoparticles (Fig 5.5 b) have extra bonds which appear in the region below 1000 cm-[1] and these can be attributed to formation of metal oxide nanoparticles, Ce — O appears at 712 cm-[1] (Senthilkumar et al., 2017), Zr — O stretching band at 508 cm-[1] (Mersian et al., 2018) and Zn — O at 493 cm-[1] (Jayachandraiah et al., (2014), Kirankumar & Sumathi, (2017 ). The location of bands in P — ZrO2CeO2ZnO nanoparticles is different from those of the plant extracts demonstrating a proper linkage between functional groups present in plant extracts and nanoparticles (Vaseghi et al., 2018a). The phenolic O — H band appears at 3285 cm-[1] in plant and in P — ZrO2CeO2ZnO nanoparticles it appears at 3616 cm'[1]. The C = 0 is due to flavonoids or reducing sugars aldehydes and ketones band shift 1706 cm'[1] in raw plant extract to 1682 cm'[1] in P — ZrO2CeO2ZnO nanoparticles (Wicaksono et al., 2020), C —O band shift 1024 cm'[1] in plant to 1055 cm'[1] in P — ZrO2CeO2ZnO

nanoparticles. The P = 0 phosphoryl bond appears at 1267 cm-[1] (Alexandratos &

Zhu, (2018); Zhi et al., (2018 ).

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Figure 5:5: FT-IR Spectrum of (a) raw plant (b) P — ZrO2CeO2ZnO nanoparticles.

The FT-IR spectrum of 1 % P — Zr02Ce02Zn0 nanoparticles/alginate beads before and after sorption is shown in Figure 5.6. The spectrum of 1 % P — Zr02Ce02Zn0 nanoparticle/ alginate beads (Figure 5.6 a) shows a 0 — H band at 3332 cm-[1] (Monier et al., 2018), C — 0 stretching of amide at 1601 cm-[1], C — N stretching of amines at 1127 cm-[1] (Joshy et al., 2018) and a C — 0 — C saccharide stretching of alginate at 1061 and 1018 cm-[1] (Geetha et al., 2016). After sorption (Figure 5.6 b) the 0 — H band shifts to 3231 cm-[1], C — 0 group shifts to 1601 cm-[1] , and C — 0 — C shifts to 1027 cm-[1] indicating that those groups may have participated in enrichment of Pb and Cd.

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Figure 5:6: FT IR spectrum of a 1% P — ZrO2CeO2ZnO nanoparticles/alginate composite (a) before and (b) after adsorption

5.2.3 Brunauer-Emmet-Teller (BET) analysis

The surface area, pore volume and diameter of the nanoparticles were investigated using BET analysis and the results are shown in Figure 5.7. The physisorption isotherms for both plant leaves (Figure 5.7 a) and P — Zr02Ce02Zn0 phytochemical caped nanoparticles (Figure 5.7 b) are similar suggesting that the surface properties are influenced by the capping material from the plant. Both plant and nanoparticles exhibited Type III physisorption isotherm which is obtained when interactions between the adsorbent and adsorbate are weak, the material has no identifiable monolayer formation and the adsorbed molecules are clustered around the most favourable sites on the surface of the nonporous solid (Thommes et al., 2015). The surface area, pore size and pore volume of the P — ZrO2CeO2ZnO nanoparticles were 0.4593 m[2]g-[1], 6.80 nm, 0.000734 cm[3]g-[1] respectively. The pore size is within the range of 2-50 nm hence the material is classified as mesoporous (Ravi et al., (2019; Zhang et al., 2009) and physisorption takes place in two or less distinct stages which is capillary condensation and monolayer-multilayer adsorption (Sing et al., 1985).

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Figure 5:7: N2 adsorption-desorption curves of (a) raw plant and (b) P — ZrO2CeO2ZnO nanoparticles

The BET surface area of the 1% P — ZrO2CeO2ZnO nanoparticles/alginate beds was determined using BET N2 adsorption-desorption isotherms and the material exhibited type V physisorption isotherm as shown in Figure 5.8. The statistical thickness of the beads is shown in Figure 5.9 and it ranges from 0 - 1 Ä.

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Figure 5:8: Surface plots for alginate and 1% P —ZrO2CeO2ZnO nanoparticle/ alginate composite.

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Figure 5:9: Statistical thickness of (a) alginate and (b) 1% P — ZrO2CeO2ZnO NP alginate.

The effect of inclusion of P — ZrO2CeO2ZnO into the calcium alginate beads is shown in Table 5.4 and the results show that the surface area increased from 4.38 to 7.33 m[2]g -[1], micropore volume from 0.00087 to 0.0016 cm[3]g-[1], and pore size decreased from 423.94 to 386.48 A respectively. The volume, micropore area and surface area of the alginate increased after encapsulation with 1 % P — ZrO2CeO2ZnO nanoparticles. Saturation of the pores occurred when the nanoparticle content was increased to 4 and 6 %. Hence in the study the 1 % P — ZrO2CeO2ZnO nanoparticle/alginate composite beads were selected for the enrichment of Pb, As, Cd and Cr due to their larger pore volume and higher surface area of the composite beads which enhances better uptake and interaction. Both calcium alginate and P — ZrO2CeO2ZnO nanoparticles /alginate beads exhibits type V physisorption isotherm which shows weak adsorbent-adsorbate interactions and is obtained with certain porous materials (Thommes et al., 2015).

Table 5:4: BET Surface area analysis of alginate and P — ZrO2CeO2ZnO nanoparticle loaded beads.

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nanoparticles/alginate beads

5.2.4 Scanning Electron Microscopy and Energy Dispersive X-ray spectroscopy characterisation

The morphology and topography of the P — ZrO2CeO2ZnO nanoparticles were determined by SEM and the SEM images are shown in Figure 5.10 (a). Small irregular shaped particles embedded within flakelike structures are visible in the SEM images. Figure 5.10 (b) shows the results of SEM-EDX elemental mapping of the nanoparticles. The quantities of the elements present were, cerium (5.9%), carbon (7.66%), iron (1.57%), oxygen (41.14%), calcium (0.29%), phosphorous (24.5%), zirconium (10.39%) potassium (0.92%) and zinc (4.34%). The carbon, potassium, oxygen, calcium and iron, which were detected were from impurities present in the plant leaf extracts and metal salts used to synthesize the nanoparticles. The size of the nanoparticles was determined from transmission electron microscopy (TEM) micrographs or images using ImageJ software. The images are shown in Figure 5.10 (c; d). The respective particle size distribution plots in Figure 5.10 (e). The P — ZrO2CeO2ZnO nanoparticles particle size range was 0.10-4.51 nm and they demonstrated some dispersion and a few clusters. The majority of the nanoparticles was within 0.10- 0.59 nm range. The mean nanoparticle size was 0.255 nm. Both TEM and SEM images also confirms that the nanoparticles have an irregular shape.

The selected area electron diffraction (SAED) patterns were also recorded and are shown in Figure 5.10 (f; g). The ring like structure of the SAED pattern confirms the polycrystalline nature of the nanoparticles (Lian et al., 2017). The Odpin online software was used to index the SAED images with a diffraction constant of 440 and the results showed that the diffraction pattern at a,/>’ and y = 90 °, a (Â) = 4.05, b (Â) = 4.05, c (Â)= 4.05. The (hkl)1 circle corresponding to 211 was indexed to ZrO2 26 = 60.1. The SAED indexing results pointed out to the formation of oxides of zirconia and cerium nanoparticles. The other circle with (hkl)1 corresponding to 220 can be indexed to 26 =54.54 of CeO2. Figure 5.11 shows the selected area electron mapping of a) oxygen, 16 b) phosphorous, 16 c) zinc 16 d) Cerium, 16 e) zirconium. The inclusion of the elements during nanoparticle synthesis is shown by EDX elemental mapping images which show that the elements are evenly distributed.

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Figure 5:10: (a) SEM image, (b) EDS spectrum, (c & d) TEM image, (e) Particle distribution (f) and (g) SAED images of P — ZrO2CeO2ZnO.

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Figure 5:11: EDX mapping images for (a) oxygen, (b) phosphorous, (c) zinc, (d) cerium, (e) zirconium within the P — ZrO2CeO2ZnO nanoparticles.

The morphology of the P — ZrO2CeO2ZnO nanoparticles/alginate beads was determined by scanning electron microscopy and the images of the P — ZrO2CeO2ZnO nanoparticles/alginate beads are shown in Figure 5.12 (a), (b) and (c). The beads have a microporous structure with the nanoparticles embedded within the beads.

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Figure 5:12: a), b), c) SEM image of P — ZrO2CeO2ZnO nanoparticles/alginate beads

5.2.5 X-ray Diffraction characterisation

Powder X-ray Diffraction (XRD) and Profex software version 4.2.4 were used to investigate the crystalline nature, phase identification and composition analysis of the P — ZrO2CeO2ZnO nanoparticles. The pure wurtzite structure of bulk ZnO was indexed by the corresponding XRD patterns shown in Figure 5.13 (Ali et al., 2016; Bandeira et al., 2020; Joint Committee on powder Diffraction Standards, JCPDS NO. 36-1451; Khorsand Zak et al., 2017). The diffraction peaks observed at 29=36.33, 37.48 and 48.17 were indexed to the Bragg reflections (020), (101) and (102) planes of the wurtzite structure of ZnO. Similar findings were observed on ZnO synthesis ( Güy and Ozacar, (2016); Choudhary et al., (2010). The monoclinic phase of ZrO2 (JCPDS No. 01-0731523) was attributed by diffraction peaks at 29=30.19, 50.25, 60.10 indexed to the Bragg reflections (101), (112), (211). Various authors assigned the diffraction peaks to ZrO2 nanoparticles ( da Silva et al., 2019; Mangla & Roy, 2018; Sharma et al., 2019). The presence of CeO2 was confirmed by diffraction peaks at 29 = 28.5, 33.08, 54.54 and 59.08 which were indexed to the (111), (200), (220) and (222) face centred cubic structure of CeO2 (JCPDS No. 34-0394). Similar diffraction pattern was observed during CeO2 synthesis (Aboutaleb and El-Salamony, 2019; Akbari et al., 2017; Chen et al., 2012; da Silva et al., 2019; Krishnan et al., 2019; Mishra and Rai, 2019; Ravi and Shashikanth, 2017) The peak at 29 = 21.59 and 26.51 can be indexed to the amorphous carbon in the nanoparticles (Koç et al., 2019;

Mohammadi & Veisi, 2018). The peak at 29 =24.16 can be indexed to the (012) of

Fe3O2 from the leaf extract (Benhammada et al., 2020).

Both XRD and SAED analysis confirmed the crystalline nature of the P — ZrO2CeO2ZnO nanoparticles. The crystalline size was calculated using the Debye - Scherrer’s formula, Equation 5.9 (Birajdar et al., 2016),

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where 1 is the X-ray wavelength (1.5406 A), P is the Full Width Half Maximum (FWHM) of the most intense peak and 9 is the Bragg’s angle position. The crystalline size of ZnO nanoparticles at 29 = 36.2 was 0.247 nm. The size of ZrO2 was 0.296 nm at 29 = 30.198. At 29 = 47.48 the crystalline size of CeO2 was 0.191 nm. The sizes of the nanoparticles were found to be in the same range when size determination was carried out by both XRD and TEM. The results from EDX, ICP-MS and XRD investigations revealed that zinc, phosphorous, zirconia and cerium were successfully incorporated into the P — ZrO2CeO2ZnO nanoparticles. FT-IR, UV Vis, ICP-MS, SEM, TEM, SAED, XRD and elemental imaging maps investigations point out to the formation of P — ZrO2CeO2ZnO nanoparticles.

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Figure 5:13: XRD pattern of the P — ZrO2CeO2ZnO nanoparticles.

The crystallinity of the P — ZrO2CeO2ZnO nanoparticles/alginate beads was determined using a D2-Phaser Powder Diffractometer and the pattern is shown in Figure 5.14. The beads were amorphous as shown by the disordered pattern suggesting that the nanoparticles were incorporated into the structure of the beads. This suggested that the nanoparticles did not retain their original structure but disturbed the structure of the alginate by penetrating into its pores. Larosa et al., (2018) characterized bare and tannese loaded calcium alginate beads and found out that tannese loaded beads were not crystalline.

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Figure 5:14: XRD pattern of P — ZrO2CeO2ZnO nanoparticles/alginate beads

5.2.6 X-ray photoelectron spectroscopy characterisation

The XPS spectra of elements present in P — Zr02Ce02Zn0 nanoparticles are presented in Figure 5:15. The spectra confirm the presence of P 2p, Zr 3d[5], C 1s sp[2] and sp[3], O 1s, Ce d[5] and Zn 2p[3] as summarized in Table 5.5. The Zr 3d[5] at 181.9 and 184.6 eV could be ascribed to Zr[4]+ ions (Nascimento et al., 2022). The peaks at 883.1 and 901.2 eV are ascribed to Ce[3]+ whilst the peak at 917.4 is due to Ce[4]+ ions (Zhang et al., 2015). The peak at 133.5 eV could be ascribed to P[5]+ ions (Omer et al., 2019). The peaks at 1022.4 and 1046.6 eV could be ascribed to Zn 2p[3] of Zn[2]+ ions (Zhou et al., 2018). The peaks at 284.6, 285.8, 293.4 and 298.2 eV are due to the C — C, C — 0, C = 0,0 — C = 0 of Carbon1s respectively (Chen et al., 2022). The peaks at 168.8 and 170 eV are due to S 2sp[3] and 2 p[1] from the sulphate of starting salts (Kafashan, 2019).The peaks at 198.8 and 200.4 eV is due to Cl 2p[3] and 2p[1] respectively from to the metal chloride of the starting salts. From XPS results the suggested structures are P-ZrO2CeO2ZnO and P - ZrO2CeOZnO.

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Figure 5:15 XPS showing the elements present in the P— ZrO2CeO2ZnO nanoparticles (a) sodium, (b) zinc, c) cerium, (d) carbon, (e) chlorine, (f) zirconium, (g) sulphur, (h) phosphorous

Table 5:5 XPS Chemical ID and Quantification

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5.2.7 Determination of metal composition by Inductively Coupled Plasma-Mass Spectrometry

The concentration of zinc, zirconia and ceria metals in P —ZrO2CeO2ZnO nanoparticles and P — ZrO2CeO2ZnO nanoparticles encapsulated into alginate was investigated by ICP-MS. The results of the investigation are shown in Table 5.6 and they prove that the nanoparticles were successfully incorporated in the alginate beads.

Table 5:6: Quantification of metal concentration in P — ZrO2CeO2ZnO nanoparticles and 1% P — ZrO2CeO2ZnO NP/alginate.

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5.3 Kinetics and reaction mechanisms for photocatalytic degradation of Congo red using P — ZrO2CeO2ZnO nanoparticles

5.3.1 Catalytic activity of the P — ZrO2CeO2ZnO

The catalytic activity of P — ZrO2CeO2ZnO nanoparticles was evaluated for the photodegradation of Congo red with the aid of UV LED light. The parameters which were optimized during the study includes amount of catalyst, initial Congo red concentration and degradation time.

5.3.2 The effect of catalyst amount on degradation of Congo red

The evaluation of the effect of catalyst amount was carried out at a fixed concentration of Congo red (10 mg/L) and varied P — ZrO2CeO2ZnO nanoparticles catalyst amount (0.5, 1.0 and 2.0 g/L). The outcome of the evaluation is shown in Figure 5.16. UV- Vis spectrometry was used to quantify the amount of Congo red remaining in solution. Before light illumination the removal efficiencies were 32.6, 20.46 and 7.13% and after light illumination they increased to 77.82, 59.90 and 35.55 % for 0.5, 1.0 and 2.0 g/L catalyst concentrations, respectively. A similar trend was observed by Aboutaleb and El-Salamony, (2019) whereby an increase in the amount of catalyst gave rise to a decrease in removal efficiencies. The observed phenomenon is attributed to the reduction in active sites of the catalyst which occurs when it becomes saturated with substrate.

The higher removal efficiency at low catalyst concentration is due to the increased amount of catalyst surface available for uptake of the Congo red molecules and corresponding increased absorption of photon energy leading to production of more free reactive radicals for dye decomposition. Higher catalyst concentration results in lower rate of decolouration due to the accumulation of particles, which leads to dispersion and reduced penetration of light and subsequently limited decolourization (Arbab et al., 2018; Guo et al., 2012).

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Figure 5:16 The effect of 0.05, 1 and 2 g/L catalyst dosage on decolouration of 10 mg/L Congo red and insert colour changes with time after degradation.

5.3.3 The effect of changing Congo red concentration on its degradation

The determination of effect of changing Congo red dye concentration on its degradation was investigated using 10, 15 and 25 mg/L of Congo red and 1 g/L catalyst concentration. The results of the investigation are as shown in Figure 5.17. Before light illumination the removal efficiencies of Congo red were 27.57, 43.17 and 15.87 % and after light illumination the removal efficiencies were 85.85, 82.07 and 66.19 % at 10, 15 and 25 mg/L Congo red concentrations respectively. A similar trend was observed by Shekardasht et al., (2020) who suggested that more light exposure would be required for higher concentrations of Congo red. The removal efficiencies were very high when the dye concentrations were low due to high absorption-desorption equilibria. When the concentration of the dye increased, more Congo red molecules, intermediates and photoproducts competed for absorption onto the active sites of the catalyst surface leading to an effective reduction in the reaction rate (Martínez et al., 2013).

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Figure 5:17. The effect of changing Congo red concentrations (10, 15 and 25 mg/L) on photodegradation by 1 g/L of P — ZrO2CeO2ZnO nanoparticles catalyst and insert colour changes as the reaction progressed.

5.3.4 The effect of reaction time on degradation of Congo red

The reaction time for the degradation of Congo red was optimized using 100 mL of 15 mg/L of Congo red dye and 1 g/L of P — ZrO2CeO2ZnO nanoparticles catalyst. The reaction was followed by taking samples between 30-300 min for every 30 min. Figure 5.18 shows the experimental results and the optimum reaction time for the catalytic degradation of the dye was 250 min. Arunadevi et al., (2018) reported an optimum time of 180 min using Cd, Ba — CuO nanoparticles. In similar studies, Aboutaleb and

El-Salamony, (2019) also managed to reach optimum degradation time of 180 min using Fe2O3 — CeO2 nanoparticles. Clamping of the P — ZrO2CeO2ZnO nanoparticle photocatalyst and the low strength of the LED light source contributed to the longer degradation time experienced in this study.

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Figure 5:18. The effect of varying reaction time on the photocatalysis of 15 mg/L Congo red by 1 g/L P — ZrO2CeO2ZnO nanoparticles.

5.3.5 Reaction kinetics for the degradation of Congo red

In catalysis studies, kinetic modelling is crucial because it gives the rate of Congo red degradation which indicates the amount of time needed for the reaction go towards completion. The degradation of Congo red was investigated using pseudo zero order, pseudo second order and Langmuir-Hinshelwood (L-H) kinetic models.

The pseudo zero, pseudo first and pseudo second order kinetic models as shown in Figure 5:19 were used to model the results of the kinetic study. The apparent rate constant and reaction rates are shown in Table 5.7. At low concentration (10 mg/L) the reaction best fitted pseudo first order kinetics with rate constant 0.0069 min-[1] and a similar trend was observed (Boudiaf et al., (2020), Zhang and Yan, (2019) and Vattikuti et al., (2016). Pseudo first order reactions are heterogeneous photocatalysis and adsorption-desorption process on the photocatalyst is not disturbed by decomposing reactions (Duta & Visa, 2015). In the study the reaction followed pseudo first order kinetics meaning the reaction rate depended only on Congo red and excess reactant did not affect the reaction. The reaction followed pseudo second order kinetics at 15 mg/L with R2 = 0.9401 with a rate constant of 0.2376 min-[1]. The degradation reactions followed zero order kinetics with a rate constant of 0.0775 min-[1] at 25 mg/L Congo red concentration. The reaction rate is independent of the concentration of all reacting species and constant for zero order kinetics.

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Figure 5:19. Kinetic modelling for the degradation of 10, 15 and 25 mg/L Congo red using 1 g/L P — ZrO2CeO2ZnO nanoparticles (a) Pseudo zero order, (b) Pseudo first order, (c) pseudo second order.

Table 5:7. Parameters of kinetic study of the photocatalytic degradation of 10, 15 and 25 mg/L Congo red using 1 g/L P — ZrO2CeO2ZnO nanoparticles.

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5.3.6 Regeneration of the P —ZrO2CeO2ZnO nanoparticle catalyst

The experiments to determine the regeneration of catalyst were run using 20 mg/L Congo red concentration, 1 g/L catalyst amount, and uncontrolled pH for four cycles. The used catalyst was regenerated by centrifugation followed by washing with distilled water followed by oven drying at 110 °C. Figure 5:20 shows the extraction efficiencies obtained during the experiment and they were 75, 46.6, 47.7 and 51.1 % for the first, second, third and fourth cycle respectively. The general decrease in photocatalytic activity of the P — ZrO2CeO2ZnO catalyst can be ascribed to photo-corrosion under light irradiation and loss of some weakly bound nanoparticles on the catalyst surface (Zhu et al., 2016). The increase between the third and fourth cycles can be attributed to trace amount of Congo red remaining on the catalyst surface during catalyst regeneration. The residual Congo red has a cumulative effect on the total concentration of the dye upon addition of fresh dye after each cycle.

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Figure 5:20. The recycling experiments for degradation of 20 mg/L Congo red using 1 g/L P — ZrO2CeO2ZnO nanoparticles.

5.3.7 The reaction mechanism for the catalytic degradation of Congo red

The reaction mechanism for Congo red photodegradation was investigated using scavenging experiments using 15 mg/L Congo red solution with (a) no scavenger, (b) 1 mM isopropanol (c) 1 mM Ethylenediaminetetraacetic acid (EDTA) and (d) 1 mM potassium dichromate. The progress of the reaction was monitored by withdrawing samples every 30 min and analysing using UV-Vis spectrometry. The results of the investigation are shown in Figure 5:21. Ethylenediaminetetraacetic acid was used to scavenge for holes (Zhu et al., 2016). Isopropanol and Potassium dichromate were used to scavenge for hydroxyl and superoxide radicals, respectively (Zeghioud et al., 2018). Addition of potassium dichromate caused a decrease in the reaction efficiency by 76.01%. The relatively large decrease confirms that the superoxide species played a major role in oxidative degradation of Congo red. Similar observations were noted by Adam et al., (2018) during their studies on degradation of Congo red. The major role played by h + holes in the degradation of Congo red was shown by a decrease in efficiency by 53% upon addition of ethyleaminetetraacetic acid. The hydroxyl radicals had a minor role as indicated by a 49.9% decrease in efficiency upon addition of isopropanol. Photolysis also played a minor role in the reaction as evidenced by a 53.0% decrease in efficiency when light was the limiting factor in the reaction.

Figure 5:21. Effect of different scavengers on degradation of 15 mg/L Congo red

The kinetics of the inhibition reaction were studied and the results are shown in Figure 5:22 and Table 5.8. The inhibition reactions using potassium dichromate, ethyleaminetetraacetic acid, t-butanol and light only without catalyst were best described by second order kinetics with rate constants of 0.0652, 0.0651, 0.0889 and 0.0889 min-[1], respectively. Both Congo red and the inhibitors played a key role during the degradation reaction at different levels. The reaction rate is proportional to the product of the concentration of the two reactants or the square of the molar concentration if the reactant is only one for pseudo second order reactions. Zero order kinetics with a rate constant of 0.0306 min-[1] best described the reaction without inhibitor. The concentration of Congo red and other reactants had a significant effect on the photodegradation reaction.

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Figure 5:22. (a) Pseudo zero order, (b) pseudo first order, (c) pseudo second order kinetic modelling for the inhibition reactions of 15 mg/L Congo red

Table 5:8. Kinetic parameters for the EDTA, t-butanol, potassium dichromate inhibition reactions.

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When irradiated with visible light P —ZrO2CeO2ZnO nanoparticles absorbed the photons possessing energy greater than their bandgap and the electrons got excited. The electrons got excited in the valence band (VB) and moved to the conduction band (CB). Electrons and holes were transferred between ZrO2, CeO2 and ZnO when an equal number of holes (h+) were generated in the VB. Electrons jumped from ZnO to CeO2 to ZrO2 in the conduction band. The holes were transferred from ZrO2 to CeO2 to ZnO in the valence band. The holes and electrons took part in the chemical reaction which resulted in separation of photo induced electron-hole pairs and a decrease of recombination rate in the catalyst (Qin et al., 2018). Positive holes were formed when electrons reside in the conduction band as shown in Equation 5.10

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Excited electrons were transferred from a conduction band of ZnO which has better electrical conductivity and a lower fermi level, Equations 5.11 (Vidya et al., 2017) to 5.13.

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The generated photoelectrons were scavenged by dissolved oxygen in water producing oxygen radicals, Equation 5.14.

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The generated oxygen radicals combined with hydrogen ions to form HOO-, Equation 5.15.

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HOO- combined with trapped electrons to generate hydrogen peroxide, Equation 5.16.

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Hydrogen peroxide combined with trapped electrons to form hydroxyl radicals, Equation 5.17.

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The positive holes on the VB reacted with water or the surface hydroxyl groups to form hydroxyl radicals as shown by Equations 5.18 and 5.19.

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equations 5.14-5.19 were adapted from (Darabdhara & Das, 2018)

The hydroxyl and superoxide radicals reacted with Congo red to form carbon dioxide, water and other non-toxic products as shown by Equation 5.20.

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Figure 5:23 shows the proposed reaction mechanism summarising the above discussed equations. Electrons were transferred within the metal element in the photocatalyst resulting in creation of positive holes. The electrons reacted with oxygen and hydroxides to form radicals which oxidizes Congo red to non-toxic compounds.

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The effectiveness of the P — ZrO2CeO2ZnO nanoparticles catalyst was compared with other catalysts as shown in Table 5.9. The photocatalyst compared well with other catalysts in terms of degradation efficiency and rate.

Table 5:9. A comparison of photodegradation efficiency of catalysts using Congo red as substrate

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The major findings were low catalyst of 10 mg/L concentration promoted increased rate of reaction due to availability of free active sites until equilibrium is reached. High catalyst concentration of 25 mg/ L resulted in lower rate of degradation due to the aggregation of nanoparticles which leads to low dispersion and reduced penetration of photons and subsequently reduced photodegradation. Removal efficiencies were enhanced by low dye concentrations due to high absorption- desorption equilibria. Congo red molecules, intermediates and photoproducts competed for adsorption onto the active sites of the catalyst surface leading to an effective reduction in the reaction rate due to the high concentration of dye. The reaction required more time to enable the catalyst to reach equilibrium and degrade optimum molecules. At lower concentration the reaction follows pseudo first order kinetics, at medium concentration it follows pseudo second order kinetics and at high concentration follows zero order kinetics. The reaction mechanism for the efficient degradation of Congo red was determined by superoxide, h+ holes and light. The high removal efficiency for the P — ZrO2CeO2ZnO catalyst means it can be used to degrade the toxic Congo red dye effectively.

5.4 Enrichment of lead and cadmium from water using P — ZrO2CeO2ZnO Nanoparticles/Alginate Beads: Optimization and determination of significant factors and interactions using response surface methodologies

5.4.1 Adsorption equilibrium studies

The performance of a sorbent is evaluated by determining the adsorption capacity which establishes how much sorbent is required to quantitatively concentrate the analyte from aqueous matrices. The adsorption equilibrium studies were determined by varying the Cd and Pb concentration from 10 - 100 mg/L, the sample volume was kept at 100 mL, the optimum pH was 7, the adsorbent dosage was 150 mg. The maximum adsorption capacity was estimated by fitting adsorption data into Freundlich, Langmuir, Temkin and Dubinin-Radushkevich models. The fitness of the isotherms was judged using the correlation coefficient R[2]. The isotherm plots for Cd and Pb are shown in Figures 5:24 and 5:25 respectively.

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Figure 5:25: (a) Langmuir (b) Freundlich (c) Temkin and (d) Dubinin-Radushkevich plots for Pb adsorption

The maximum adsorption capacity was 62.89 mg/g for Cd and 292.93 mg/g for

Pb according to the Dubinin Radushkevich equation. Cd fitted the Dubinin

Radushkevich equation with R = 0.992 and represented by Equation 5.21,

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and sorption mechanism was mainly physical in nature. Pb fitted into the Freundlich isotherm model with R = 0.975 and represented by Equation 5.22,

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The Langmuir, Freundlich, Temkin and Dubinin-Radushkevich isotherm model parameters are shown in Table 5.10.

Table 5:10: Langmuir, Freundlich, D-R and Temkin isotherm parameters.

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5.4.2 Screening of Significant Factors for Cd and Pb extraction

The significant variables which affect the removal efficiency of Cd and Pb were screened by carrying out a half factorial design with 8 runs using Minitab 18. The optimised variables included sample flow rate, dosage, pH, sample volume, eluent flow rate and eluent concentration.

The significant variables for Cd recovery was selected according to their estimated effects which are represented by normal plots (Figure 5: 26) and Pareto chart (Figure 5: 27). Each variable which exceeded the reference line was considered to be significant at 95% confidence interval. Sample volume was found to be the most significant variable for Cd recovery and the other variables were insignificant. The other factors were kept constant in the subsequent experiments. In the case of Pb,, no variable was found to be significant at 95% confidence interval.

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Figure 5:26: Normal plots for effects of flow, dosage, pH, sample volume, eluent flow rate and eluent concentration on extraction recovery.

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Figure 5:27: Pareto chart for the effects on flow, dosage, pH., sample volume, eluent flow rate and eluent concentration on extraction recovery of lead and cadmium.

5.4.3 Optimization of the significant extraction conditions for Cd and Pb using the Taguchi experimental design

Optimization of the significant variables was carried out by the Taguchi experimental design and included 16 runs in order to determine the varied variables which are sample volume, dosage, and pH and eluent concentration. The model to predict the enrichment factor of Cd and Pb is shown in Equations 5.23 to 5.24 respectively. A positive value indicates enhancement and a negative value vice versa.

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The predicted responses are shown in Table 5.11 and actual optimum conditions were sample volume 100 mL, dosage 50 mg, and pH 7.0 and for recovery, the optimum elution conditions were 0.1 MHNO3 from results in Table 5.12. The predicted responses only agreed on sample volume and the rest were different which is expected since the model fit is not 100 %.

Table 5:11: Multiple Response Prediction Parameters

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Table 5:12: Results of the optimization of the most significant extraction conditions for CD and Pb

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The residual plot is shown in Figure 5:28 and the residuals are randomly scattered in a constant band with about the zero-line indicating the appropriateness of the model.

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Figure 5:28: Residual plots for the enrichment of Cd and Pb.

5.4.4 Evaluation of significant factors and interactions using Analysis of Variance (ANOVA)

To test the probable interaction and important effects between variables, ANOVA was carried out using Minitab 18 and the probability values less than 5% indicated statistical significance at a 95% confidence level. In this case, the linear model and sample volume were statistically significant parameters. The coefficient of determination (R[2]) for the model is 0.9159 implying the model can explain 91.59% of the observed variation in the experimental results by changing variables of the modelled parameters.

ANOVA was used to test the significance of the Taguchi design model for Pb and Cd enrichment. The responses and the results of the ANOVA analysis are presented in Tables 5.13 and 5.14 respectively. In all cases for the enrichment of Pb the values of p were above 5% at a 95% confidence interval meaning that they were not statistically significant at selected variables. Hence enrichment of Pb is independent of any change in variables and can be carried out under any conditions. However, for the enrichment of Cd, the effect of sample volume was statistically significant as well as the model itself.

Table 5:13: Taguchi model for optimization of enrichment of Pb.

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Model Summary

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Table 5:14: Taguchi model for optimization of enrichment of cadmium from water samples.

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Model Summary

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5.4.5 Main effects of sample volume, dosage and pH on the enrichment of Cd and Pb using P — ZrO2CeO2ZnO nanoparticles/alginate

The sample volume is an important parameter in preconcentration studies since high preconcentration factors are desirable when analysing trace metals in real samples. There was an exponential increase in enrichment factor for Cd (Figure 5:29 A) when sample volume changes from its lowest level to its highest level assuming all other factors are kept constant. There is a decrease at first followed by an increase in enrichment factor for Pb (Figure 5:29 B) when sample volume changes from 10 mL to 100 mL assuming all other factors are kept constant. The use of a large sample volume allows the enrichment factor to be improved in this case; hence 100 mL was selected as the optimum sample volume in this study. Further higher volumes above 100 mL were avoided since the recoveries decrease swiftly with increasing sample volume for each analyte (Tokay et al., 2021).

There was a decrease in the enrichment factor for Pb and Cd when sorbent dosage changes from 10 mg to 150 mg when all other factors are kept constant. As the amount of adsorbent increases in solid-phase extraction methods, desorption of the analytes attached to the adsorbent becomes difficult since a higher eluent volume is needed resulting in a decrease in sensitivity and extraction efficiency(Ulusoy et al., 2019). The extraction efficiency does not increase with the increase in dosage because the concentration of the metal ions is kept constant (Yuan et al., 2020).

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Figure 5:29: Main effect of sample volume, dosage and pH on enrichment factor of (A) Cd and (B) Pb

A gradual increase in enrichment factors for Cd under acidic conditions followed by a decrease from pH 6.0 was observed when pH changed from pH 3.0 to 9.0 when all the other factors were kept constant was observed. There was a decrease in the enrichment factor for Pb when pH changes from pH 3.0 to 9.0 when all the other factors are kept constant. At lower pH values there was protonation of the functional groups of P — ZrO2CeO2ZnONanoparticles/alginate beads nanocomposite which caused the reduction of hydrogen bonding between adsorbent and Cd. Sorption of Pb was found to be high at low pH. In basic solution, hydroxide ions may form complexes with metal ions and precipitate them whereas in acidic solutions protonation of binding sites of chelating molecules may also occur thereby affecting the enrichment of the Pb and Cd as shown in Figure 5:30 (Urns et al., 2013).

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Figure 5:30 Distribution of lead hydroxide and cadmium hydroxide at various pH Optimum conditions were obtained using the half-factorial design and the levels which produced the highest enrichment factors with few interactions were selected as the optimum conditions

5.4.6 Evaluation of the most significant factors and interactions using response surface methodology and interaction plots

The enrichment factor increased with enhancing sample volumes from 10 to 100 mL whereas increasing sorbent dosage from 10 to 150 mg resulted in a decline in enrichment factor and this was due to the sample reaching equilibrium earlier as shown in surface plots in Figure 5:31. Interactions occurred between sample volume and dosage as shown in Figure 5:32. Interactions were observed at sample volume below 30 mL for both. Cd (Figure 5:32 a) and Pb (Figure 5:32 g). Dosages also experienced interactions above 80 mg for Cd (Figure 5:32 c) whereas for Pb they were observed below 40 mg and above 100 mg (Figure 5:32 i).

The enrichment factor was enhanced when the sample volume was increased from 5 to 100 mL. When pH was increased from 3 to 9 for the same experiment the enrichment factor decreased due to analytes and surface properties of sorbent being affected such that they favour or hinder sorption as shown in the surface plots in Figure 5:31. Interaction occurred between sample volume and pH as shown in Figure 5:32. Interactions occurred for sample volume less than 30 mL and above 70 mL for Cd (Figure 5:32 b) and only below 50 ml for Pb (Figure 5:32 h). Interactions were observed below pH 5.0 and above 7.0 for Pb (Figure 5:32 k).

Surface plots in Figure 5:31 show that when the adsorbent dosage was increased from 50 to 150 mg, a decrease in enrichment factor due to early attainment of equilibrium was observed. An increase in pH resulted in an increase in the enrichment factor up until neutral pH and the enrichment factor started to decline thereafter because the forms of analytes and sorbent surface chemistry changed as pH was increased and some forms favoured uptake whilst others inhibited it. The interaction plots are shown in Figure 5:32. Interactions were observed for dosages below 50 mg for Cd (Figure 5:32 b) and above pH 7 for Cd (Figure 5:32 f).

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Figure 5:31: Surface plots for sample volume, dosage and pH vs enrichment factor of Pb (A) and Cd (B)

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All displayed terms are in the model,

Figure 5:32: Interaction plots for sample volume, dosage and pH vs enrichment factor for Pb and Cd

5.4.7 Interference studies

Metals and other coexisting ions associated with heavy metals show interference in the presence of some heavy metal ions. The interference occurs through redox reactions, formation of precipitates and participating in complexation reactions (Ahmad et al., 2019). The effect of anions and metals have been investigated by several authors and results show that metal interactions are mainly antagonistic (Mahamadi & Madocha, 2013). The effect of organic contaminants has been rarely investigated hence in this study the effect of alcohol on recoveries of Cd and Pb metals were determined by varying the concentration from 1, 5, and 10 % phenol and propane-2-ol at pH 7, sorbent dosage 50 mg and 10 pg/L Cd and Pb concentration and the results are shown in Figure 5:33. Phenol-enhanced Cd and Pb recovery at low concentrations up to 5 % and depressed recovery at high concentrations. Propanol enhanced recovery at 1 % and depressed recovery at 5 and 10 % concentrations. Both alcohols depressed recovery at 10% concentration due to enhancement of bonding between sorbent and analyte.

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Figure 5:33: The effect of increasing the concentration of phenol and propanol on recoveries of Cd and Pb from water samples.

5.4.8 Desorption cycles for Cd and Pb recoveries

Five adsorption-desorption cycles were carried out to assess the effectiveness of the sorbent to recover Cd and Pb from water samples as shown in Figure 5:34. The extraction recovery of Cd and Pb were almost constant for four cycles however it is depressed at the fifth cycle. The lower recovery values of between 20-30% may be due to strong adsorption which hinders the desorption step leading to a decrease in the recovery values (Maranata et al., 2021).

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Figure 5:34: Cd and Pb adsorption desorption cycles

5.4.9 Acceptance criteria

The linearity was determined over a range of six calibration standards ranging from

31.25-1000 gg/L. The calibration points were fitted to linear regression. Five extractions of 50 pg/L Cd and Pb by P — ZrO2CeO2ZnO nanoparticles/alginate composite and calculating the relative standard deviation were used to determine method precision (repeatability). The limit of quantification (LOQ) was calculated using equation 4.5. The limit of detection (LOD) was calculated using equation 4.6. The acceptance criteria are shown in Table 5.15.

Table 5:15: Results of acceptance criteria for the analysis

Parameter

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Recovery (ER)% 57.0 -147.70 33.12- 116.5

5.4.10 Analytical applications

The validation of the proposed procedure was determined by carrying out addition recovery experiments on real water samples and the results are shown in Table 5.16. It was done by spiking real samples from well and borehole water with analyte ions and recoveries were calculated using Equation 4.3. Spiking was done at three different levels i.e., at 1.0, 5.0 and 10 pg/L for each metal ion. The borehole water sample was collected from Avondale, Harare and the well water sample was collected from Retreat farm in Waterfalls, Harare, Zimbabwe.

Table 5:16 Recoveries for well water and borehole water

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5.4.11 Comparison with other methods

The analytical performance of the method was compared with other reported methods as shown in Table 5.17. The limit of detection, precision, recovery and enrichment factors of the present method compares well with other methods in literature.

Table 5:17. Comparison of this study with some enrichment studies in literature.

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The major findings were the experimental results showed that 0 — H, C — 0, and C — 0 — C bonds played a role on enrichment of Cd and Pb because they did not appear in the FTIR spectrum after uptake. Sorption of Cd was mainly physical in nature and Pb involved multilayer adsorption. Sample volume was selected as the most significant factor for Cd recovery during screening experiments whereas Pb could be analysed under any conditions. High sample volume 100 mL, low sorbent dosage 10 mg and acidic pH below 7 favoured enrichments of both Cd and Pb. The recoveries of the metal ions were enhanced by low concentration at 1% of propanol and phenol and depressed their high concentrations at 10%. The method showed great potential for enrichment of the selected metals because a very low limit of detection was obtained.

5.5 Enrichment of Arsenic and Chromium by pipette tips loaded with P — ZrO2CeO2ZnO nanoparticles /alginate beads

5.5.1 Adsorption experiments

The sorption capacity of the adsorbent is important since it determines how much adsorbent is required to remove a specific amount of the metal ions from solution. Adsorption capacity was calculated using Equation 4.4.

The adsorption capacity was determined by varying initial As and Cr concentration from 5 to 20 mg/mL, 100 mL sample volume, dosage 20 mg, at pH. 7.0, at 1 mL/ min flow rate and the results are shown in Table 5:18. Both Cr and As sorption followed Dubinin Radushkevich isotherm model meaning the main mechanism of sorption was physical. The equilibrium isotherm equation forCr was lnqe = In 2.0 + 0.015e[2] and the equation model of As was In qe = In 1.84 — 0.012 e[2]. The maximum sorption capacity for Cr was 137.12 mg/g and 154.74 mg/g for As according to the Dubinin Radushkevich model.

Table 5:18: Langmuir, Freundlich, D-R and Temkin isotherm parameters

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5.5.2 Optimization of SPE experiments

The screening of the most significant factors on Cr and As enrichment was determined using the half fractional factorial design with eight experimental runs. The screened factors were eluent concentration, pH, sorbent dosage, sample volume, eluent flow rate. The eluent concentration (2.0 M), amount of adsorbent (10;40 mg), eluent flow rate (2 rpm) sample volume (5;100 mL), sample pH (3;9) and eluent volume (10 mL) were used during the optimization experiments. The extraction efficiency was assed using recovery studies.

A Pareto chart in Figure 5:35 was used to select the significant variables from sample volume, pH, eluent concentration, eluent flow rate and sample flow rate based on their absolute values. The values which exceeded the reference determining line were considered significant variables at 95% confidence interval. Data from the Pareto chart shows that dosage, eluent flow rate and sample volume were the most significant factors on removal of Cr. For subsequent experiments significant variables were considered for optimization using the full factorial design and the others were fixed (Abbaspour et al., 2013).

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Figure 5:35: Pareto chart for optimization of the significant effect for solid phase extraction of a) As and b) Cr.

5.5.3 Full factorial designs and response surface methodology for

optimization of the significant conditions for Cr an As enrichment A full factorial design with 21 runs was used to optimize the screened significant variables (dosage, eluent flow rate and sample volume). Figure 5:36 shows the residual plots for the optimization process. The model is appropriate for the study since the points are scattered around the centre.

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Figure 5:36: Residual plots for enrichment of a) Cr and b) As

The optimum conditions which gave favourable results for As and Cr enrichment were eluent flow rate- 1 mL/min, sample volume-5 mL, pH 7 and dosage 40 mg. The obtained values were close to the predicted values in Table 5.19.

Table 5:19: Multiple Response Prediction Parameters

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The responses of the runs and the independent variables runs are shown in Table 5.20.

The data in the table was used to model the interactions between the factors, main factors and to predict the enrichment factors of arsenic and chromium.

Table 5:20: Results for optimization of significant extraction conditions for As and Cr.

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Equations 5.25 and 5.26 shows the model to predict the EF of As and Cr respectively. An enhancement relationship among responses is shown by positive value whilst a negative value indicates decline between responses among terms.

Illustrations are not included in the reading sample

where D is dosage or amount of beads sorbent, P is pH and S is sample volume.

5.5.4 Effects of sample volume, pH and dosage on enrichment factors of As and Cr and the interactions between factors

Interaction plots were used to determine interactions between the variables. The results are displayed in the Figure 5.37. Interactions between sample volume and dosage were observed for Cr and As. The interactions for Cr occurred at 50 mL sample volume (Figure 5:37 a), 12-15 mg sorbent dosage (Figure 5:37 c). The interactions for As were observed between 40 to 50 mL and above 80 mL (Figure 5:37 iii) and at 10, 20 and 40 mg sorbent dosage (Figure 5:37 i). Interactions between sample volume and pH were also observed during the study. Interactions between pH and sample volume were observed at pH 4 and 7 (Figure 5:37 e) and at 40-60 mL sample volume (Figure 5:37 b) for Cr enrichment. Interactions were also observed between sample volume and pH for As enrichment. Other interactions occurred as below pH 4 (Figure 5:37 ii) and between 10- 40 mL and at 100 mL (Figure 5:37 v). Interactions were observed between pH and dosage for Cr enrichment at 15 mg and above 35 mg of sorbent dosage (Figure 5:37 d) and at pH 4 and 5 (Figure 5; 37 f). Similar interactions were noted during As enrichment between pH 4-6 and above pH 8 (Figure 5:37 iv) and at 15, 20-30 mg sorbent dosage (Figure 5:37 vii). The results from interaction studies shows regions to avoid when choosing optimum conditions.

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5.5.5 The effect of main factors on As and Cr enrichment

Figure 5:38 shows main effects of sample volume, dosage and pH on the enrichment of As and Cr enrichment.

The pH of the enrichment solution plays an important role in uptake of ions. An increase in enrichment factor was observed for both Cr and As when the pH was increased from 3.0 to 9.0. However, after pH 7.0 a decline in enrichment was observed for Cr from pH 7 to 9 whereas for As the mean response was almost constant. The optimum pH chosen for the enrichment of As and Cr in this study was pH 7.0. Serkan Yalgin et al., (2020) obtained quantitative recoveries for Cr (III) at similar pH range of 6.0 to 8.0 using Phallus impudicus loaded with YFe2O3. Hydroxyl groups on the sorbent are mainly responsible for sample uptake. The groups retain anions under acidic conditions and under basic conditions they retain cations (Baranik et al., 2018).

A general increase in the enrichment factor was observed when the dosage was increased from10 to 40 mg as shown in Figure 5:38. The enrichment factor was higher for Cr than As suggesting it was preferentially enriched. This is due to the fact that at low dosage more of the metal ions remain in solution since the sorption sites becomes saturated quickly. The enrichment factor increased at higher sorbent dosage because a lot of free active sites were available for the uptake of Cr and As. Ghorbani et al., (2020) also observed a similar trend for recovery of Cr . They suggested the reason for the trend was due to an increase in free active sites for the uptake of the analytes and surface area.

The other parameter which was evaluated in this study which can influence the extraction efficiency was the sample volume. A decrease in enrichment of As and Cr was observed when sample volume was increased from 5 to 100 mL as shown in Figure 5:38. Zhang et al., (2010) also observed a similar trend when they enriched As. Huang et al., (2007) found that quantitative recoveries of Cr were found when sample volumes were less than 30 mL.

5.5.6 Effect of organic interferences on As and Cr enrichment

The effect of ethanol and methanol on solid phase extraction of As and Cr enrichment was determined at pH 7.0 by varying the alcohol concentration from1, 5 and 10 % fo r methanol 1, 2 and 10 % for ethanol. The results of the determination are shown in F igure 5:39. During the experiment the dosage of the adsorbent was 20 mg; the sample and eluent volumes were 10 mL and As and Cr concentration was 10 gg/L.

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Figure 5:39: Effect of (a, b) methanol and (c, d) ethanol on recovery of As and Cr Increase in methanol concentration depresses the recovery of both As by 6 % and Cr by over 100 %. The increase in ethanol concentration from 1 to 10 % results in increase in recovery of As by 3 %, however increase in concentration of ethanol results in Cr enrichment increasing by up to 5 %. At higher ethanol concentrations recovery of As and Cr was depressed.

5.5.7 Regeneration studies for As and Cr enrichment

Adsorption desorption cycles were carried out to assesses the regeneration and reusability of the sorbent for As and Cr enrichment. As recovery was constant during the desorption cycles, however Cr recoveries dropped during the second cycle from 102 to 39% and in the fourth cycle it was 19% as shown in Figure 5:40.

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Figure 5:40 Extraction recovery cycles for As and Cr

5.5.8 Evaluation of the enrichment of As and Cr method performance

Six standards ranging from 31.25, 62.5, 125, 250, 500, 1000 gg/L were used to determine the linearity of the method. Linear regression analysis was used to fit the calibration points. In order to confirm that the selected regression and linearity are appropriate a sample spiked with a standard was analysed. Five extractions of As and Cr 20 gg/L using P — ZrO2CeO2ZnO nanoparticle/alginate composite were used to determine the precision of the method. A single analytical run was carried out in a single day respectively to determine precision as relative standard deviation RSD %. The limit of quantification was calculated using equation 4.5 and the limit of detection was calculated using equation 4.6. The results for the validation data for the analysis is shown in Table 5.21.

Table 5:21: Results of the validation data for the analysis

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5.5.9 Application in real samples

Addition recovery experiments were carried out to determine the accuracy of the method for As and Cr enrichment by spiking real samples from well and effluent water and the results are shown in Table 5.22. Spiking of the water samples was carried out at 2, 5.0 and 10 pg/L for Cr and As. Recovery as % was calculated from mass in the analyte of spiked sample towards added mass after replicate analysis of spiked samples at various concentrations using Equation 4.7.

Table 5:22: Recovery tests from well and effluent water samples.

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5.5.10 Comparison with other methods

The developed method was compared with previous methods reported in literature as shown in Table 5:23. The LOD, recoveries and precision of the current method were comparable or even lower than other methods on As and Cr recovery based on enrichment before spectroscopy analysis.

Table 5:23: Comparison of As and Cr enrichment and determination using other methods.

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During As and Cr enrichment study the most significant factors were screened using a half factorial design. The number of factors were reduced from five to three. The three were dosage, eluent flow rate and sample volume. Interactions were observed for sample volume and dosage at 50 mL between 12-15 mg for Cr, sample volume and pH at pH 4 and 7 between 40-60 mL for Cr and for As above pH 4 between 10-40 mL, dosage and pH at pH 4 and 5 above dosage 35mg for Cr and for As at pH 4-6 at 20-30 mg sorbent dosage. The method shows great potential for enrichment of arsenic and chromium due to its low limit of detection.

CHAPTER 6 : CONCLUSIONS AND RECOMMENDATIONS

6.1 Conclusions

A green method for the synthesis of P — ZrO2CeO2ZnO nanoparticles was established. The synthesis of nanoparticles was shown to be affected by variables such as pH, dosage and metal concentration. There were interactions between factors during the synthesis stage. These interactions were between metal concentration and volume ratio, plant dosage to volume ratio, plant dosage to metal concentration, pH and volume ratio, pH and metal concentration, pH and dosage. The FTIR results suggest that phytochemicals such as flavonoids, aldehydes, ketones, reducing and sugars, participated in the synthesis and stabilization of P — ZrO2CeO2ZnO nanoparticles. Their functional groups shifted or were totally absent in the nanoparticle band. The synthesised nanoparticles have active sites for hydrogen bonding on the C — O, P = O, C = O, C = O and O — H bands which enhances the particles application for environmental remediation such as catalysis and adsorption.

P — ZrO2CeO2ZnO nanoparticles show high activity for Congo red degradation under domestic LED light irradiation in aqueous medium. Low catalyst concentration at 0.5 g/L promotes an increase in rate of reaction due to availability of active sites and high catalyst concentration results in lower rate of decolouration due to the accumulation of particles which leads to dispersion and reduced penetration of light and subsequently limited decolourization. Low dye concentrations at 10 mg/L resulted in large removal efficiencies due to high absorption desorption equilibria. High dye concentrations at 25 mg/L result in more Congo red molecules, intermediates and photoproducts competing for absorption onto the active sites of the catalyst surface leading to an effective reduction in the reaction rate. The reaction requires a longer time to enable the catalyst to degrade optimum molecules and reach equilibrium. The reaction follows pseudo first order kinetics at 10 mg/L dye concentration, pseudo second order kinetics at 15mg/L concentration and zero order kinetics at 25 mg/L concentrations of Congo red. The results of the photocatalytic studies reveal that superoxide, h+ holes and light are the main determinants of the reaction mechanism for the efficient degradation of Congo red.

For Cd and Pb enrichment on P — ZrO2CeO2ZnO nanoparticles/ alginate beads the experimental results showed that O — H, C — O, and C — O — C bonds played a role on enrichment of Cd and Pb. Sorption of Cd was mainly physical in nature and Pb involved multilayer adsorption. Sample volume was selected as the most significant factor for Cd recovery during screening experiments whereas Pb could be analysed under any conditions. The significance of sample volume for the recovery of Cd was reinforced as the statistically significant parameter during evaluation of significant parameters by ANOVA. High sample volume of 100 mL, low sorbent dosage of 10 mg and acidic pH at 4 favoured enrichments of both Cd and Pb. The recoveries of the metal ions were enhanced by low concentration of propanol and phenol and depressed their high concentrations.

Novel P — ZrO2CeO2ZnO nanoparticles/ alginate beads were successfully used for As and Cr enrichment. The most significant factors were screened using a half factorial design and the number was reduced from five to three namely sample volume, dosage and eluent flow rate. Interactions were observed for sample volume and dosage at 50 mL between 12-15 mg for Cr, sample volume and pH at pH 4 and 7 between 40-60 mL for Cr and for As above pH 4 between 10-40 mL, dosage and pH at pH 4 and 5 above dosage 35 mg for Cr and for As at pH 4-6 at 20-30 mg sorbent dosage.

6.2 Recommendations for future work

Specific phytochemical can be extracted from plants using organic solvent and utilized during synthesis of nanoparticles. Samples from each different condition in the experimental design can be analysed using TEM and SEM to determine effect of factors on size and morphology. The effect of temperature on nanoparticle synthesis can also be explored. The optimization of green synthesis can be carried out using other experimental design techniques as well as response surface methodology.

Nanoparticles can also be immobilized in different matrix and form membranes which can be explored for the enrichment of heavy metals. Multielement enrichment can also be explored for solid phase extraction studies.

Further studies need to be carried out to determine the exact causes of the colour changes which occurred to Congo red in the presence of LED light and P —ZrO2CeO2ZnO nanoparticles. The products at each stage of the decolourization reaction can be identified using Gas Chromatography­Mass Spectrometry (GC-MS) or Liquid chromatography Mass spectrometry (LC- MS).

CHAPTER 7 LIST OF PUBLICATIONS

A. Hokonya, N., Mahamadi, C., Mukaratirwa-Muchanyereyi, N., Timothy Gutu, T. and Zvinowanda, C., (2022). Green synthesis of P — ZrO 2CeO 2ZnO nanoparticles using leaves extract of Flacourtia indica and their application for photocatalytic degradation of a model toxic dye, Congo red, Heliyon, 8 (8). https://doi.Org/10.1016/j.heliyon.2022.e10277

B. Hokonya, N., Mahamadi, C., Mukaratirwa-Muchanyereyi, N., Timothy Gutu, T. and Zvinowanda, C., (2022). Enrichment of lead and Cadmium from water using P — ZrO 2CeO 2ZnO Nanoparticles/Alginate Beads: Optimization and determination of significant factors and interactions using response surface methodologies. Scientific African, 17. https://doi.org/10.1016/j.sciaf.2022.e01 340

C. Hokonya, N., Mahamadi, C., Mukaratirwa-Muchanyereyi, N., Timothy Gutu, T. and Zvinowanda, C., (2022). Evaluation of effects of factors and interactions on enrichment of Arsenic and Chromium by pipette tip solid phase extraction using novel P — ZrO 2CeO 2ZnO nanoparticles /alginate beads. European Journal of Chemistry. https://doi10.5155/eurjchem.13.3.327-336.2295

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CHAPTER 9 APPENDIX

9.1.1.1 Tauc plots data

Table A: 1 Tauc plots for undoped nanoparticles

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Table A: 2 Tauc plots for dried doped P — ZrO 2CeO 2ZnO nanoparticles dried nano

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AE1) Power flux calculation

Power of LED light = 20 watt = work/time = 20 Js-[1] Equation A.1

Energy of photon (E) = lic/A =6.626 x10-34 Js-[1] x 3.0 x108 ms-[1]/5.95 x10-[9] m

Equation A.2

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Number of photons emitted per second = 20 Js-[1]/3.3408 x 10 -[39] J Equation A.3

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9.1.1.2 Linear Model Analysis: Means versus pH, Dosage (g), metal concentration

(M), volume ratio

Table A: 3 Estimated Model Coefficients for Means

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Model Summary

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0.3336 98.31% 91.57%

Table A: 4: Fits and Diagnostics for Unusual Observations for P — ZrO 2CeO 2ZnO nanoparticle synthesis

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Figure A: 1: Calibration curve for Cr and As SPE

Table A: 5: Adsorption equilibrium studies parameters

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Table A: 6: Adsorption equilibrium studies parameters

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Table A:7Adsorption equilibrium parameters for Cd

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Table A: 8: Adsorption equilibrium parameters for Pb

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Table A: 9: Adsorption desorption cycles for Pb and Cd Solid phase extraction

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Figure A: 2Calibration curve for Cr and As SPE

9.1.1.3 Determination of hydrogen bonding active sites of the P — ZrO 2 CeO 2 ZnO nanoparticle using alcohols.

The nanoparticles were soaked in 10 cm[3] of neat solution, 1) water, 2) methanol 3) ethanol, 4) propan-2-ol, 5) phenol separately and left overnight in a tightly sealed container. The nanoparticles were air dried for 10 minutes prior to IR measurements.

The IR shifts were then recorded. The effect of adsorption from a mixture of dilute penetrants was investigated by adding about 5 cm[3] of methanol, ethanol, prop-2-ol, phenol, butanol to 15 cm[3] water and then added to the nanoparticles. The nanoparticles were air dried before FT IR analysis.

The interaction of the nanoparticles with ethanol, methanol, propanol, phenol and a mixture of alcohols was used to study hydrogen bonding. The hydrogen bonding was monitored using the IR red shift. The ATR FT-IR yields the information about the identity of active sites on the P — ZrO 2CeO 2ZnO nanoparticles. The interaction was studied using neat solution, dilute solution and mixed solution. A red shifted hydrogen bond leads to a decrease in the hydrogen bond vibrational frequency and usually to bond length elongation whereas the blue shifted hydrogen bond leads to bond length contraction and increase in vibrational frequency (Lu et al., 2005). Blue shifted hydrogen bonds are shifted towards a higher wavelength number A spectral shift towards a higher wavelength number is called a blue shift (Liu et al., 2007) and a shift towards a lower wavelength is a red shift.

Table A: 10: Effect of ethanol, methanol, propanol, phenol and mixture on bonds

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The IR bands for Ce — 0 at 712 cm-[1], Zr — 0 at 508 and 438 cm-[1], Zn — 0 at 493 cm-[1], does not appear in dilute and neat solutions of nanoparticles in the alcohols. Blue shifted hydrogen bonds were experienced by a) P = 0 bonds in neat methanol, b) amidel bonds in dilute mixture of alcohols, c) 0H bonds in neat and dilute methanol, neat and dilute propanol neat phenol and the dilute mixture of alcohols. The red shifted hydrogen bonds were experienced by a) C — 0 bonds in dilute propanol and neat phenol, b) C = 0 bonds in dilute mixture of alcohols, c) P = 0 bonds in dilute ethanol and dilute phenol, d) amide 1 bonds in dilute ethanol, dilute phenol, e) 0H bonds in dilute ethanol and dilute phenol. The hydrogen bonding active sites which were identified by determining the effect of neat and dilute ethanol, methanol, propanol, phenol and dilute alcohols on FT-IR spectrum of the nanoparticles were P = 0, C — 0, C = 0, Amide 1 and 0 — H.

9.1.1.4 Antiplagiarism report

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Title: Green Synthesis of Trimetallic Nanoparticles using Flacourtia Indica (Burm.f.) Merr. Characterization and Applications

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Title
Green Synthesis of Trimetallic Nanoparticles using Flacourtia Indica (Burm.f.) Merr. Characterization and Applications
College
Bindura University of Science Education  (CHEMISTRY)
Course
PHD
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N/A
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Nichodimus Hokonya (Author)
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2024
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254
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Nichodimus Hokonya (Author), 2024, Green Synthesis of Trimetallic Nanoparticles using Flacourtia Indica (Burm.f.) Merr. Characterization and Applications, Munich, GRIN Verlag, https://www.grin.com/document/1590457
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  • Depending on your browser, you might see this message in place of the failed image.
  • Depending on your browser, you might see this message in place of the failed image.
  • Depending on your browser, you might see this message in place of the failed image.
  • Depending on your browser, you might see this message in place of the failed image.
  • Depending on your browser, you might see this message in place of the failed image.
  • Depending on your browser, you might see this message in place of the failed image.
  • Depending on your browser, you might see this message in place of the failed image.
  • Depending on your browser, you might see this message in place of the failed image.
  • Depending on your browser, you might see this message in place of the failed image.
  • Depending on your browser, you might see this message in place of the failed image.
  • Depending on your browser, you might see this message in place of the failed image.
  • Depending on your browser, you might see this message in place of the failed image.
  • Depending on your browser, you might see this message in place of the failed image.
  • Depending on your browser, you might see this message in place of the failed image.
  • Depending on your browser, you might see this message in place of the failed image.
  • Depending on your browser, you might see this message in place of the failed image.
  • Depending on your browser, you might see this message in place of the failed image.
  • Depending on your browser, you might see this message in place of the failed image.
  • Depending on your browser, you might see this message in place of the failed image.
  • Depending on your browser, you might see this message in place of the failed image.
  • Depending on your browser, you might see this message in place of the failed image.
  • Depending on your browser, you might see this message in place of the failed image.
  • Depending on your browser, you might see this message in place of the failed image.
  • Depending on your browser, you might see this message in place of the failed image.
  • Depending on your browser, you might see this message in place of the failed image.
  • Depending on your browser, you might see this message in place of the failed image.
  • Depending on your browser, you might see this message in place of the failed image.
  • Depending on your browser, you might see this message in place of the failed image.
  • Depending on your browser, you might see this message in place of the failed image.
  • Depending on your browser, you might see this message in place of the failed image.
  • Depending on your browser, you might see this message in place of the failed image.
  • Depending on your browser, you might see this message in place of the failed image.
  • Depending on your browser, you might see this message in place of the failed image.
  • Depending on your browser, you might see this message in place of the failed image.
  • Depending on your browser, you might see this message in place of the failed image.
  • Depending on your browser, you might see this message in place of the failed image.
  • Depending on your browser, you might see this message in place of the failed image.
  • Depending on your browser, you might see this message in place of the failed image.
  • Depending on your browser, you might see this message in place of the failed image.
  • Depending on your browser, you might see this message in place of the failed image.
  • Depending on your browser, you might see this message in place of the failed image.
  • Depending on your browser, you might see this message in place of the failed image.
  • Depending on your browser, you might see this message in place of the failed image.
  • Depending on your browser, you might see this message in place of the failed image.
  • Depending on your browser, you might see this message in place of the failed image.
  • Depending on your browser, you might see this message in place of the failed image.
  • Depending on your browser, you might see this message in place of the failed image.
  • Depending on your browser, you might see this message in place of the failed image.
  • Depending on your browser, you might see this message in place of the failed image.
  • Depending on your browser, you might see this message in place of the failed image.
  • Depending on your browser, you might see this message in place of the failed image.
  • Depending on your browser, you might see this message in place of the failed image.
  • Depending on your browser, you might see this message in place of the failed image.
  • Depending on your browser, you might see this message in place of the failed image.
  • Depending on your browser, you might see this message in place of the failed image.
  • Depending on your browser, you might see this message in place of the failed image.
  • Depending on your browser, you might see this message in place of the failed image.
  • Depending on your browser, you might see this message in place of the failed image.
  • Depending on your browser, you might see this message in place of the failed image.
  • Depending on your browser, you might see this message in place of the failed image.
  • Depending on your browser, you might see this message in place of the failed image.
  • Depending on your browser, you might see this message in place of the failed image.
  • Depending on your browser, you might see this message in place of the failed image.
  • Depending on your browser, you might see this message in place of the failed image.
  • Depending on your browser, you might see this message in place of the failed image.
  • Depending on your browser, you might see this message in place of the failed image.
  • Depending on your browser, you might see this message in place of the failed image.
  • Depending on your browser, you might see this message in place of the failed image.
  • Depending on your browser, you might see this message in place of the failed image.
  • Depending on your browser, you might see this message in place of the failed image.
  • Depending on your browser, you might see this message in place of the failed image.
  • Depending on your browser, you might see this message in place of the failed image.
  • Depending on your browser, you might see this message in place of the failed image.
  • Depending on your browser, you might see this message in place of the failed image.
  • Depending on your browser, you might see this message in place of the failed image.
  • Depending on your browser, you might see this message in place of the failed image.
  • Depending on your browser, you might see this message in place of the failed image.
  • Depending on your browser, you might see this message in place of the failed image.
  • Depending on your browser, you might see this message in place of the failed image.
Excerpt from  254  pages
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