Fabrication of Novel Nanohybrid Material for the Removal of Azo Dyes from Wastewater

: This study attempted to harness the dual beneﬁt of adsorption and photocatalytic degradation for efﬁciently removing a model anionic azo dye, Orange G, from an aqueous solution. For this purpose, a series of bifunctional nanohybrids containing different proportions of naturally occurring biopolymer chitosan and ternary photocatalyst made of kaolinite, TiO 2 , and ZnO were prepared through the dissolution of chitosan in acid and subsequent deposition on ternary photocatalyst. The characterization through Fourier-transform infrared spectroscopy (FT-IR), X-ray diffraction (XRD), ﬁeld emission scanning electron microscopy (FE-SEM), and energy dispersive X-ray spectrum (EDS) have conﬁrmed the successful fabrication of nanohybrids from TiO 2 and chitosan. The adsorptive separation of Orange G from the aqueous solution and subsequent degradation under solar irradia-tion was thoroughly studied by recording the λ max value of dye in the ultraviolet–visible (UV-Vis) spectrophotometer at various operating conditions of pH, dye concentration, contact time, and compositional variation. The nanohybrid (TP 0.75 CS 0.25 ) fabricated from 75% ternary photocatalyst ( w / w ) and 25% chitosan ( w / w ) removed 97.4% Orange G within 110 min at pH 2.5 and 10 mg/L dye concentration. The relative contribution of chitosan and ternary composite on dye removal was understood by comparing the experimental results in the dark and sunlight. Recyclability experiments showed the suitability of the nanohybrid for long-term repeated applications. Equilibrium experimental data showed a better correlation with the Langmuir isotherm and pseudo-second-order kinetic model. The rapid and nearly complete removal capacity, long-term reusability, and simple fabrication technique make this novel nanohybrid a promising advanced material for removing hazardous azo dyes from industrial efﬂuents.


Introduction
The textile and garments industries are recognized as major contributors to the severe deterioration of surface water quality [1]. Large quantities of dyestuff are used in these industries due to fabric processing and polishing the final products. These organic dyes are non-biodegradable and present in the range of 10 to 200 ppm concentration in wastewater. As a result, uptake of these wastewater causes serious health hazards, such as skin irritation, kidney failure, or even cancer [2]. In addition, this is also a source of threat to the environment. The natural photosynthetic phenomenon is interrupted by the inhabitation of sunlight into the stream due to the colored compounds of the dyes. For example, vinyl sulfone dyes, also known as azo dyes, are a class of reactive dyes effectively used for silk, cotton, and wool. It is reported in literature that more than 30% of the used dyes remain in the spent dye bath after the dyeing process [3,4]. Effluents from textile industries contain Preparation of chitosan from prawn shells involves three main steps: deproteinization, demineralization, and deacetylation. About 10 gm of the prawn shell was first washed in a 2 L beaker with distilled water for about 90 min at 80 °C with occasional stirring to increase the rate of cleaning. After cleaning, the raw prawn shells were placed in an oven at 60 °C for about 10 h. The dried shells then underwent deproteinization and were treated with 3% NaOH (w/w) at a ratio of 1:18 (w/w) for about 3 h at 80 °C. Then, the proteins underwent decantation for removal. To demineralize the shells, 3 M HCl was used at a ratio of 1:18 (w/w) for about 4 h. In this step, the evolution of CO2 occurred, and chitin was obtained. Then, the chitin was neutralized by washing with distilled water and was placed in the oven at 60 °C for 10 h. To obtain chitosan from this dried chitin, it was deacetylated by using 50% NaOH (w/w) for about 4 h at a ratio of 1:18 (v/v). Then, the chitosan was obtained by filtering the solution and was washed with acid to remove the additional alkali. The solubility of chitosan was tested using a 1% (v/v) acetic acid solution [28]. Figure 1 shows the images of prawn shells at different steps of chitosan preparation: Figure 1. Images of (a) raw prawn shells, (b) prawn shells after sorting, (c) prawn shells after washing, (d) prawn shells after deproteinization, (e) prawn shells after demineralization, (i.e., chitin) and (f) chitosan.

Preparation of Ternary Photocatalyst
The ternary photocatalyst was obtained from kaolinite, TiO 2 , and ZnO. These precursors were mixed at an optimized composition of 50% kaolinite, 45% TiO 2 , and 5% ZnO in deionized water. The mixture was then sonicated for about 60 min at 50 • C. The solid mass was then isolated by evaporation in the oven at 100 • C for about 60 min. Then, the dried product was ground to increase the surface area. The obtained powder then underwent calcination in a muffle furnace at different temperatures. The synthesis was facilitated by this high-temperature environment. Then, the calcined product was ground again to increase its reactivity in the dye removal operation [29]. Figure 2 illustrates the schematic diagram of the preparation steps of the ternary photocatalyst. J. Compos. Sci. 2022, 6, x FOR PEER REVIEW deionized water. The mixture was then sonicated for about 60 min at 50 °C. The solid was then isolated by evaporation in the oven at 100 °C for about 60 min. Then, the product was ground to increase the surface area. The obtained powder then unde calcination in a muffle furnace at different temperatures. The synthesis was facilita this high-temperature environment. Then, the calcined product was ground again crease its reactivity in the dye removal operation [29]. Figure 2 illustrates the sche diagram of the preparation steps of the ternary photocatalyst.

Preparation of Nanohybrid Material
Three different nanohybrids with different weight ratios of ternary photocataly chitosan were prepared. The chitosan flakes were dissolved in 100 mL of 1 M acet solution. After that, the prepared ternary photocatalyst was added to the solution, a final mixture was sonicated for 50 min to obtain a homogenous viscous mixture. The mixture was added to a solvent mixture (15% NaOH and methanol in a ratio of 4:1 at a constant rate in a drop-wise manner that led to the formation of the compo beads. The beads were then washed multiple times to remove the additional NaO placed in the oven at 80 °C for about 10 h. The dried product was ground with mort pestle to make it finer and thus increase its surface area and reactivity [30,31]. The cation of the nanohybrid was strongly controlled by the pH of the medium. Three ent nanocomposites were prepared with varying ratios of ternary photocatalyst an tosan, as shown in Table 1.

Preparation of Nanohybrid Material
Three different nanohybrids with different weight ratios of ternary photocatalyst and chitosan were prepared. The chitosan flakes were dissolved in 100 mL of 1 M acetic acid solution. After that, the prepared ternary photocatalyst was added to the solution, and the final mixture was sonicated for 50 min to obtain a homogenous viscous mixture. Then, the mixture was added to a solvent mixture (15% NaOH and methanol in a ratio of 4:1 (v/v)) at a constant rate in a drop-wise manner that led to the formation of the composite as beads. The beads were then washed multiple times to remove the additional NaOH and placed in the oven at 80 • C for about 10 h. The dried product was ground with mortar and pestle to make it finer and thus increase its surface area and reactivity [30,31]. The fabrication of the nanohybrid was strongly controlled by the pH of the medium. Three different nanocomposites were prepared with varying ratios of ternary photocatalyst and chitosan, as shown in Table 1. To identify the functional groups present in the samples and any chemical interactions among the components of the nanohybrids, FT-IR spectra of samples were recorded on an FT-IR 8400S spectrophotometer (Shimadzu Corporation, Japan) in the wavenumber range of 4000 to 400 cm −1 , resolution of 4 cm −1 ; and scans of 30. Approximately 1 mg of the samples were ground with 100 mg KBr by agate mortar, and then, the pellet was made from the mixture by applying pressure.

X-ray Diffraction (XRD) Analysis
To analyze the phase of the samples, XRD patterns of the samples were recorded by an X-ray diffractometer (Ultima IV, Rigaku Corporation, Tokyo, Japan) at room temperature. Prior to XRD analysis, the samples were ground into fine powders using mortar and pestle. Cu K α radiation (λ = 0.154 nm) from a broad focus Cu tube operated at 40 kV and 40 mA was applied to the samples for measurement. The XRD patterns of the samples were measured in the continuous scanning mode with a scan speed of 3 • /min and in the scan range of 5 to 100 • . Bragg's law was used to compute the basal spacing of the crystalline samples.
Scanning Electron Microscopy (SEM) and Energy Dispersive X-ray Spectrophotometry (EDS) An analytical scanning electron microscope (JEOL JSM-6490LA, Tokyo, Japan) was used to analyze the sizes, surface morphologies, and shapes of the particles. The backscattered electron mode was operated at 20 kV accelerating voltage. Magnification of the sample was employed to further investigate the samples in terms of their microstructures and morphologies. The elemental composition of the prepared composite was determined by taking its EDS spectra.

Removal of Orange G Dye Preparation of Standard Solutions of Orange G
A stock solution of 500 ppm of Orange G was prepared by dissolving 0.125 g of Orange G in distilled water in a 250 mL volumetric flask to reach a total volume of 250 mL. A series of dilutions were made from this stock solution with concentrations of 5 ppm, 10 ppm, 20 ppm, 30 ppm, 40 ppm, 50 ppm, 60 ppm, 70 ppm, 80 ppm, 90 ppm, 100 ppm, and 150 ppm. The λ max was determined, and a calibration curve of absorbance versus concentration was drawn for Orange G. The concentration of Orange G in the aqueous solution was then determined at its λ max using a UV-visible spectrophotometer (UV-2100PC, Human Lab Instrument Co., Suwon-city, Korea).

Removal of Orange G Using the Nanohybrid Particles
Batch experiments were performed for the determination of the % removal of dye using the nanohybrid particles. A total of 25 mL of viscous solutions of Orange G solutions were taken in different 100 mL beakers. Then, 5 mg of nanohybrid was added to the beakers. A mechanical shaker was utilized to shake the beakers at 120 rpm at room temperature. Amounts of 0.1 M NaOH and 0.1 M HCl were introduced to optimize the pH of the solutions. The Orange G loaded composites were separated from the suspensions by centrifuging at 3000 rpm for 60 min, and the residual concentration of Orange G in the solutions was determined by taking absorbance at 478 nm (λ max of Orange G).
The percentage removal of dye was calculated using the following formula (Equation (1)): where C e = the equilibrium concentration of Orange G (mg/L), and C o = the initial concentration of Orange G (mg/L). To find the maximum dye removal efficiency for the synthesized nanohybrid material, several parameters were investigated to observe its behavior in different environments. These parameters may have lesser or greater effects on the efficiency, and thus, we will obtain the optimized situation for the nanohybrid to work in industrial applications. Therefore, we focused on pH, initial dye concentration, compositional variation of nanohybrid, contact time, degradation in dark and in sunlight, and desorption study while carrying out the application of the nanohybrid material on the removal of Orange G dye. The equilibrium adsorption data was tested by plotting in Langmuir and Freundlich adsorp-tion isotherm equations. The kinetics of the dye removal process were studied using the pseudo-first-order and pseudo-second-order kinetic models.

Reusability Experiments
The reusability test was carried out for this nanohybrid and showed excellent removal efficiency up to four cycles at the optimized conditions (pH: 2.5, nanohybrid: TP 0.75 CS 0.25 , concentration: 10 mg/L, time: 110 min). After the end of each operation, the nanohybrid was filtered and washed with alkali (with pH ≈12) to remove the adsorbed dye. The treated dye was then washed with plenty of distilled water to remove extra alkali and finally dried in the oven again. Then, this recovered nanohybrid was reused for the next operation.

Fourier-Transform Infrared (FT-IR) Analysis
The FT-IR spectra of chitosan ( Figure S1) and ternary composite ( Figure S2) are presented in the supporting documentation. The characteristic peaks for the corresponding functional groups were observed in both spectrums. The FT-IR of the ternary composite, chitosan, and their composites of different compositions are compared in Figure 3. The surface chemistry of the quaternary nanohybrids represented in Table 1 could be well explained by comparing their FT-IR transmission spectrum with the starting ternary nanocomposite and chitosan. The comparison also provides valuable information on the interaction at the interface of the two components.
ments. These parameters may have lesser or greater effects on the efficiency, and thus, we will obtain the optimized situation for the nanohybrid to work in industrial applications. Therefore, we focused on pH, initial dye concentration, compositional variation of nanohybrid, contact time, degradation in dark and in sunlight, and desorption study while carrying out the application of the nanohybrid material on the removal of Orange G dye.
The equilibrium adsorption data was tested by plotting in Langmuir and Freundlich adsorption isotherm equations. The kinetics of the dye removal process were studied using the pseudo-first-order and pseudo-second-order kinetic models.

Reusability Experiments
The reusability test was carried out for this nanohybrid and showed excellent removal efficiency up to four cycles at the optimized conditions (pH: 2.5, nanohybrid: TP0.75CS0.25, concentration: 10 mg/L, time: 110 min). After the end of each operation, the nanohybrid was filtered and washed with alkali (with pH ≈12) to remove the adsorbed dye. The treated dye was then washed with plenty of distilled water to remove extra alkali and finally dried in the oven again. Then, this recovered nanohybrid was reused for the next operation.

Fourier-Transform Infrared (FT-IR) Analysis
The FT-IR spectra of chitosan ( Figure S1) and ternary composite ( Figure S2) are presented in the supporting documentation. The characteristic peaks for the corresponding functional groups were observed in both spectrums. The FT-IR of the ternary composite, chitosan, and their composites of different compositions are compared in Figure 3. The surface chemistry of the quaternary nanohybrids represented in Table 1 could be well explained by comparing their FT-IR transmission spectrum with the starting ternary nanocomposite and chitosan. The comparison also provides valuable information on the interaction at the interface of the two components.  The characteristic peaks of kaolinite observed at 1115 and 1004 cm −1 were overlapped to give a new peak at 1035 cm −1 in the prepared ternary composite. Another two characteristic peaks of kaolinite at 3640 cm −1 and at 3670 cm −1 , respectively, for the O-H stretching bond and the Al-O-H stretching bond also disappeared. The illustration in geometry and variation in intensity is shown in Figure 3. The peak of kaolinite that is gone completely in the ternary composite is due to the high-temperature calcination. However, the characteristic reflection from the (001) plane is visible in the spectra. All the characteristic peaks of both the chitosan and ternary composite were present in the nanohybrid. This information confirms the successful fabrication of the nanohybrid. Si-O stretching vibration of kaolinite in ternary composite at 1041 cm −1 is also present in the nanohybrid which justifies the presence of ternary composites [32,33]. Moreover, lower absorption intensity was observed for Ti-O-Ti stretching vibration in the ternary composite.

X-ray Diffraction (XRD) Analysis
The XRD pattern of commercial TiO 2 , ZnO, and ternary composite, as shown in Figure (116), respectively. The appearance of sharp diffraction patterns indicates the small size, high purity, and crystallinity of the sample [35][36][37]. The average crystallite size of titania was calculated by the Debye-Scherrer equation (Equation (2)). The full width at half maximum (FWHM) was calculated 2θ = 25.34 • . This is the most intense anatase peak (101) in XRD. The Debye-Scherrer equation is given below: where D is the crystallite size in nanometers, K is a constant known as Scherrer's constant (K = 0.89), λ is the wavelength of X-ray for this analysis (λ = 1.54056 Å), β is full width at half maximum (FWHM) (in radian) of the diffraction peak and can be measured from the XRD pattern, and θ is the corresponding diffraction angle [34,37,38]. The crystallite size of the TiO 2 was found to be 56.68 nm.   In Figure 5, sharp peaks reveal that the photocatalyst had high crystallinity, and the presence of characteristic peaks of starting materials of different intensities justifies their relative contributions accordingly. Characteristic peaks of kaolinite completely disappeared in the ternary composite due to high-temperature calcination. Apart from chemical interactions, it is also evident that the precursors underwent significant structural rearrangement during the formation of the ternary composite.

Energy-Dispersive X-ray Spectroscopy (EDS) Analysis
EDS spectra of nanohybrid were recorded to investigate the elemental composition and presence of impurities. The EDS spectrum of the nanohybrid is displayed in Figure 6, which confirms the presence of six different elements (C, Al, Si, Zn, O, and Ti). Therefore, it could be stated without any doubt that TiO 2 , ZnO, kaolinite, and chitosan were present in the nanohybrid. Recording the EDS spectrum at different particles of the nanohybrid revealed nearly identical elemental composition, which strongly suggests the uniform chemical combination of ternary nanohybrid with chitosan. Additionally, the elemental composition found from the EDS analysis was identical to the theoretical calculation (Table 2). EDS spectrum also indicates that the nanohybrid was free from any impurities. The presence of impurities is undesirable since they often severely compromise the performance of the adsorbent/photocatalyst. in the nanohybrid. Recording the EDS spectrum at different particles of the nanohybrid revealed nearly identical elemental composition, which strongly suggests the uniform chemical combination of ternary nanohybrid with chitosan. Additionally, the elemental composition found from the EDS analysis was identical to the theoretical calculation (Table 2). EDS spectrum also indicates that the nanohybrid was free from any impurities. The presence of impurities is undesirable since they often severely compromise the performance of the adsorbent/photocatalyst.

Field Emission Scanning Electron Microscopy (FE-SEM) Analysis
The FE-SEM analysis was performed to investigate the surface morphology and particle size distribution. As shown in Figure 7, the surface of ternary particles was smooth with good dispersion. The magnification of a random particle, as displayed in Figure 7a, clearly demonstrates the flaky nature of the particles. The estimated particle size of TiO2 ranged from 50 to 250 nm, as shown in Figure 7b. It showed the majority of the particles duel within the 100 to 150 nm range (58.93%).

Field Emission Scanning Electron Microscopy (FE-SEM) Analysis
The FE-SEM analysis was performed to investigate the surface morphology and particle size distribution. As shown in Figure 7, the surface of ternary particles was smooth with good dispersion. The magnification of a random particle, as displayed in Figure 7a, clearly demonstrates the flaky nature of the particles. The estimated particle size of TiO 2 ranged from 50 to 250 nm, as shown in Figure 7b. It showed the majority of the particles duel within the 100 to 150 nm range (58.93%). However, the FE-SEM images of the nanohybrid showed different morphological aspects compared to the ternary photocatalyst (Figure 7c). The hexagonal shape of the particles was achieved through the fabrication of the novel nanohybrid, confirmed by FE-SEM. The surface also showed no propensity to agglomeration with the majority of particles (44.68%) staying within 101-150 nm particle size. In general, the approximate sizes of However, the FE-SEM images of the nanohybrid showed different morphological aspects compared to the ternary photocatalyst ( Figure 7c). The hexagonal shape of the particles was achieved through the fabrication of the novel nanohybrid, confirmed by FE-SEM. The surface also showed no propensity to agglomeration with the majority of particles (44.68%) staying within 101-150 nm particle size. In general, the approximate sizes of the particles were found in a range of 50 to 250 nm. From Figure 7b,c, we can see that about 34% of nanohybrid particle sizes were in the nanoscale range (1-100 nm). However, in the case of the ternary photocatalyst, only 26% of particles were able to duel in this range. Therefore, it can be easily concluded that the obtained nanohybrid particles were at a higher percentage in terms of nanoscale range compared to the ternary photocatalyst. The uniform wrappings of the ternary nanohybrid by long molecular chains of chitosan with greater efficiency were able to prevent agglomeration. This phenomenon explains the lowering of particle size of nanohybrids. The wrapping of the TiO 2 surface with soft and flexible chitosan could also explain the shift in morphology from flaky to hexagonal. This morphological shift also supports the interfacial interaction of ternary with chitosan. In addition, it should be stated that no odd structures were detected on the surface of the nanohybrid, which is highly expected considering the application point of view.  Figure 8a, the λmax of Orange G was found to be 478 nm, and all the absorbances of the Orange G solutions were measured at this wavelength.

Effect of Different Parameters on Removal of Orange G
To find out the maximum dye removal efficiency for the synthesized nanohybrid material, it would be wise to work with several parameters to observe its behavior in different environments. These parameters may have a lesser or greater effect on the efficiency, and thus, we will obtain the optimized situation for the nanohybrid to work in industrial applications. Therefore, we have focused on several parameters (discussed below) while carrying out the application of the nanohybrid material on the removal of Or-

Effect of Different Parameters on Removal of Orange G
To find out the maximum dye removal efficiency for the synthesized nanohybrid material, it would be wise to work with several parameters to observe its behavior in different environments. These parameters may have a lesser or greater effect on the efficiency, and thus, we will obtain the optimized situation for the nanohybrid to work in industrial applications. Therefore, we have focused on several parameters (discussed below) while carrying out the application of the nanohybrid material on the removal of Orange G dye.

Effect of Compositional Variation of Nanohybrids
Nanohybrids with three different compositions have been prepared to see how the efficiency changes with the variation in the composition of the raw material while being fabricated. The photocatalyst used in this study is an optimized ternary photocatalyst with a compositional ratio of 50% kaolinite, 45% TiO 2 , and 5% ZnO and was reported as highly efficient for low concentration of dye in literature by Hasan et al. [29]. The major incorporation of low-cost kaolinite without compromising its efficiency makes this photocatalyst far more viable for industrial application than other photocatalysts available on the scene. Therefore, it was chosen for this study to fabricate a novel nanohybrid with chitosan. Here, this photocatalyst was taken at ratios of 3:1, 1:1, and 1:3 with chitosan to fabricate a series of nanohybrids to demonstrate its relative efficiency, and the results are shown in Figure 9. series of nanohybrids to demonstrate its relative efficiency, and the results are shown in Figure 9. The nanohybrid (Composite 3) which contains 75% ternary photocatalyst and 25% chitosan showed maximum efficiency in dye removal. The efficient coating of all photocatalysts by the long-chained giant chitosan molecule can be attributed to this phenomenon. This causes an optimized synergistic effect of adsorption and photodegradation on dye molecules and a higher percentage of dye are removed. As for the other two nanohybrids composed of the ratios of 1:1 (TP0.5CS0.5) and 1:3 (TP0.25CS0.75), the adsorption property dominates more than the synergistic effect due to the lesser amount of photocatalyst coated by chitosan. Therefore, the dye removal efficiency experiences a regression, as shown in Figure 9.

Effect of pH
In Figure 10, the maximum efficiency has been found at pH = 2.5 for Composite 3 (TP0.75CS0.25). The nanohybrid material which has been used for the removal of anionic Orange G dye contains chitosan and a ternary photocatalyst. Since photocatalysis occurs The nanohybrid (Composite 3) which contains 75% ternary photocatalyst and 25% chitosan showed maximum efficiency in dye removal. The efficient coating of all photocatalysts by the long-chained giant chitosan molecule can be attributed to this phenomenon. This causes an optimized synergistic effect of adsorption and photodegradation on dye molecules and a higher percentage of dye are removed. As for the other two nanohybrids composed of the ratios of 1:1 (TP 0.5 CS 0.5 ) and 1:3 (TP 0.25 CS 0.75 ), the adsorption property dominates more than the synergistic effect due to the lesser amount of photocatalyst coated by chitosan. Therefore, the dye removal efficiency experiences a regression, as shown in Figure 9.

Effect of pH
In Figure 10, the maximum efficiency has been found at pH = 2.5 for Composite 3 (TP 0.75 CS 0.25 ). The nanohybrid material which has been used for the removal of anionic Orange G dye contains chitosan and a ternary photocatalyst. Since photocatalysis occurs on the surface, the performance of the photocatalyst is greatly influenced by the solution pH, the pollutant type, and the surface's ability to adsorb the pollutant [30]. At pH = 2.5, chitosan is protonated at its optimum condition which pulls anionic Orange G dye towards it due to the electrostatic attraction force and results in maximum adsorption on the surface. The ternary photocatalyst, on the other hand, similarly shows maximum photocatalytic efficiency due to the occurrence of a high positive surface charge. As a result of these two optimum conditions for adsorption and photocatalytic degradation, the prime synergistic benefit from the nanohybrid has been obtained at pH = 2.5, justified by the peak at pH = 2.5 in Figure 10. At a pH lower than 2.5, dye removal by nanohybrid decreased. Because at pH below 2.5, the dissolution of chitosan is higher due to increased protonation, and the interaction of protons with azo linkage causes a decrease in electron density at the azo group, resulting in lower photocatalytic degradation. The right-hand side of the peak also showcases a regression in dye removal efficiency for the synthesized nanohybrid. The environment where pH is higher than 2.5 contributes to the reduction of the degree of protonation of amino functional groups in chitosan. As a result, a lesser number of anionic dyes are attracted which eventually contributes to the rise of the abundance of negative charges. Thus, it can be assumed that repulsion forces overweighed the attractive forces as the pH of the environment increases. As a result, adsorption capability and photocatalytic efficiency of the nanohybrid compromises accordingly, and a decline in removal efficiency is observed at pH higher than 2.5.

Effect of Initial Dye Concentration
The initial dye concentration plays a pivotal role to overcome all the mass transfer resistance of dyes between the aqueous and solid phases. Therefore, the influence of different initial dye concentrations on the removal efficiency by Composite 3 (TP0.75CS0.25) has been examined in this study at pH 2.5 and 0.2 gL −1 adsorbent concentrations for 120 min. At a pH lower than 2.5, dye removal by nanohybrid decreased. Because at pH below 2.5, the dissolution of chitosan is higher due to increased protonation, and the interaction of protons with azo linkage causes a decrease in electron density at the azo group, resulting in lower photocatalytic degradation. The right-hand side of the peak also showcases a regression in dye removal efficiency for the synthesized nanohybrid. The environment where pH is higher than 2.5 contributes to the reduction of the degree of protonation of amino functional groups in chitosan. As a result, a lesser number of anionic dyes are attracted which eventually contributes to the rise of the abundance of negative charges. Thus, it can be assumed that repulsion forces overweighed the attractive forces as the pH of the environment increases. As a result, adsorption capability and photocatalytic efficiency of the nanohybrid compromises accordingly, and a decline in removal efficiency is observed at pH higher than 2.5.

Effect of Initial Dye Concentration
The initial dye concentration plays a pivotal role to overcome all the mass transfer resistance of dyes between the aqueous and solid phases. Therefore, the influence of different initial dye concentrations on the removal efficiency by Composite 3 (TP 0.75 CS 0.25 ) has been examined in this study at pH 2.5 and 0.2 gL −1 adsorbent concentrations for 120 min. It is generally observed in the literature that dye removal efficiency is reported to increase initially with the increase of initial dye concentration up to a saturation point and then slowly decreases as a further increase of dye concentration occurred [40,41]. In this study, there is also an upward curve observed up to 10 mg/L followed by a decline in dye removal efficiency (Figure 11). As initial dye concentration increases, the concentration gradient gradually rises between dye molecules and the nanohybrid surface. This gradient of concentration plays a pivotal role to draw dye molecules onto the surface of the material. As long as the saturation of the surface does not occur, the adsorption of the dye molecule continues to escalate. That is why a sharp upward curve has been found initially with the increase of dye concentration. The saturation of the material surface has seemingly occurred at 10 mg/L in this study, which can be attributed to the fact all the free active sites on the surface are covered by dye molecules at this concentration. Therefore, it is obvious that a decline in dye removal efficiency will happen at any concentration above 10 mg/L for a fixed dose of material, and it has been observed accordingly in the figure as well. Moreover, phenomena, such as an increase in intra-particle diffusion as a function of concentration, can also be responsible for this type of regression in dye removal efficiency.
As the material has photocatalyst activity, we should also carefully discuss this to find out how this behavior affects the dye removal efficiency along with adsorption. The photodegradation capability of the synthesized nanohybrid can be attributed to the probability of the formation of OH radicals (primary oxidants) that react with dye molecules. Initially, more dyes are found available for the nanohybrid to react as the concentration increases, as we discussed earlier. Until 10 mg/L, this process continues. However, the surface of the material seems to be fully covered by the presence of dye molecule due to enhanced adsorption brought by chitosan at 10 mg/L, and as a result, the penetration of light to the surface decreases. Thus, the relative number of available free radicals to attack the dye molecules decreases for the fixed amount of material dose, and thus, the rate of As initial dye concentration increases, the concentration gradient gradually rises between dye molecules and the nanohybrid surface. This gradient of concentration plays a pivotal role to draw dye molecules onto the surface of the material. As long as the saturation of the surface does not occur, the adsorption of the dye molecule continues to escalate. That is why a sharp upward curve has been found initially with the increase of dye concentration. The saturation of the material surface has seemingly occurred at 10 mg/L in this study, which can be attributed to the fact all the free active sites on the surface are covered by dye molecules at this concentration. Therefore, it is obvious that a decline in dye removal efficiency will happen at any concentration above 10 mg/L for a fixed dose of material, and it has been observed accordingly in the figure as well. Moreover, phenomena, such as an increase in intra-particle diffusion as a function of concentration, can also be responsible for this type of regression in dye removal efficiency.
As the material has photocatalyst activity, we should also carefully discuss this to find out how this behavior affects the dye removal efficiency along with adsorption. The photodegradation capability of the synthesized nanohybrid can be attributed to the probability of the formation of OH radicals (primary oxidants) that react with dye molecules.
Initially, more dyes are found available for the nanohybrid to react as the concentration increases, as we discussed earlier. Until 10 mg/L, this process continues. However, the surface of the material seems to be fully covered by the presence of dye molecule due to enhanced adsorption brought by chitosan at 10 mg/L, and as a result, the penetration of light to the surface decreases. Thus, the relative number of available free radicals to attack the dye molecules decreases for the fixed amount of material dose, and thus, the rate of dye degradation also decreases. In addition, the adsorbed dye molecules also shield the UV light to penetrate the catalyst surface and absorb it. This phenomenon leads to lesser available UV photons to generate free radicals [42,43]. Therefore, the photocatalytic activity of the nanohybrid drops after 10 mg/L, and a gradual downward curve can be seen in % removal efficiency versus the initial dye concentration graph, as shown in Figure 11.

Effect of Contact Time
For practical application, it is essential to optimize the contact time for a material to harness the best possible outcome within a given time. Hence, the removal efficiency of Orange G dye by the synthesized nanohybrid material (Composite 3 (TP 0.75 CS 0.25 )) at an optimum pH of 2.5, dye concentration of 10 mg/L, and fixed adsorbent dose has been investigated and is shown as a function of time (0-140 min) in Figure 12. UV light to penetrate the catalyst surface and absorb it. This phenomenon leads to lesser available UV photons to generate free radicals [42,43]. Therefore, the photocatalytic activity of the nanohybrid drops after 10 mg/L, and a gradual downward curve can be seen in % removal efficiency versus the initial dye concentration graph, as shown in Figure 11.

Effect of Contact Time
For practical application, it is essential to optimize the contact time for a material to harness the best possible outcome within a given time. Hence, the removal efficiency of Orange G dye by the synthesized nanohybrid material (Composite 3 (TP0.75CS0.25)) at an optimum pH of 2.5, dye concentration of 10 mg/L, and fixed adsorbent dose has been investigated and is shown as a function of time (0-140 min) in Figure 12. The removal efficiency of the nanohybrid increases during its first 110 min of application followed by a steady equilibrium state until the end of the application. For materials with the dual properties of being an adsorbent as well as a photocatalyst, this initial rise in removal efficiency can be attributed to the ability of the vacant site of the adsorbent to draw more dye molecules onto it and the increased number of photogenerated free radicals with time [42,43]. The equilibrium state, however, can be caused by several reasons, such as the nearly complete coverage of the vacant site of the adsorbent by dye molecules, inhibition of the active site of the catalyst by the by-product deposits, and competition between dye molecules and the intermediate degraded product to reach the catalyst surface [43].

Control Experiments
For a better understanding of the dual effect of the nanohybrid (Composite The removal efficiency of the nanohybrid increases during its first 110 min of application followed by a steady equilibrium state until the end of the application. For materials with the dual properties of being an adsorbent as well as a photocatalyst, this initial rise in removal efficiency can be attributed to the ability of the vacant site of the adsorbent to draw more dye molecules onto it and the increased number of photogenerated free radicals with time [42,43]. The equilibrium state, however, can be caused by several reasons, such as the nearly complete coverage of the vacant site of the adsorbent by dye molecules, inhibition of the active site of the catalyst by the by-product deposits, and competition between dye molecules and the intermediate degraded product to reach the catalyst surface [43].

Control Experiments
For a better understanding of the dual effect of the nanohybrid (Composite 3,TP 0.75 CS 0.25 ), it is important to carry out operations both in daylight and darkness. This will reveal to what extent the photocatalytic activity can affect the dye removal process along with the adsorption. The dual benefits were obtained when the process was optimized under solar irradiation. The blank experiments reveal the total percentage removal, whereas the experiment in the dark shows how much degradation occurred due to the photocatalytic activity of the catalyst. The results of the control experiment are displayed in Figure 13.
J. Compos. Sci. 2022, 6, x FOR PEER REVIEW 16 of along with the adsorption. The dual benefits were obtained when the process was op mized under solar irradiation. The blank experiments reveal the total percentage remov whereas the experiment in the dark shows how much degradation occurred due to photocatalytic activity of the catalyst. The results of the control experiment are display in Figure 13. In the case of the experiment under direct sunlight with Composite 3 (TP0.75CS0.25) is found that the concentration of the dye solution in optimum pH and concentration mained unchanged when it was irradiated without the catalyst. However, in the presen of the catalyst, 90% removal of dye was found in the first 15 min. These observations dicate that without the photocatalyst, the dye solution did not undergo any photodeg dation. When the experiment was carried out in dark conditions, about 15% removal w obtained in the presence of the catalyst. As the dark environment excludes the possibil of any photodegradation occurrences, this phenomenon can be solely attributed to ability of adsorption of the catalyst of the dye molecules. Hence, the rest of the percenta removal can be concluded due to photocatalytic degradation in the presence of solar diation. From the control experiments, it is very clear that neither adsorption nor the ph todegradation alone could lead to the highest achievable limit of dye molecules remo from the aqueous solution under the optimized conditions. The synergistic effects of bo the adsorption and photocatalytic activities contribute to the almost complete removals the dye molecules that strongly justify the fabrication of the quaternary nanohybrid. In the case of the experiment under direct sunlight with Composite 3 (TP 0.75 CS 0.25 ), it is found that the concentration of the dye solution in optimum pH and concentration remained unchanged when it was irradiated without the catalyst. However, in the presence of the catalyst, 90% removal of dye was found in the first 15 min. These observations indicate that without the photocatalyst, the dye solution did not undergo any photodegradation. When the experiment was carried out in dark conditions, about 15% removal was obtained in the presence of the catalyst. As the dark environment excludes the possibility of any photodegradation occurrences, this phenomenon can be solely attributed to the ability of adsorption of the catalyst of the dye molecules. Hence, the rest of the percentage removal can be concluded due to photocatalytic degradation in the presence of solar radiation. From the control experiments, it is very clear that neither adsorption nor the photodegradation alone could lead to the highest achievable limit of dye molecules removal from the aqueous solution under the optimized conditions. The synergistic effects of both the adsorption and photocatalytic activities contribute to the almost complete removals of the dye molecules that strongly justify the fabrication of the quaternary nanohybrid.

Reusability/Recyclability Experiments
To be a suitable material in industrial application, repeated long-term use with easy regeneration and without compromising efficiency is essential. This will benefit the process by making it a cost-effective and more feasible one. In this study, the fabricated nanohybrid material was investigated for up to four cycles and showed almost the same efficiency in optimum conditions. The regeneration was done by treating with alkali (with pH ≈12) followed by the subsequent thorough washing with distilled water and drying after the end of each cycle. The results of this recyclability experiment are displayed as a bar chart in Figure 14.

Reusability/Recyclability Experiments
To be a suitable material in industrial application, repeated long-term use with easy regeneration and without compromising efficiency is essential. This will benefit the process by making it a cost-effective and more feasible one. In this study, the fabricated nanohybrid material was investigated for up to four cycles and showed almost the same efficiency in optimum conditions. The regeneration was done by treating with alkali (with pH ≈12) followed by the subsequent thorough washing with distilled water and drying after the end of each cycle. The results of this recyclability experiment are displayed as a bar chart in Figure 14. The bar chart showed that the nanohybrid displayed a very satisfactory removal performance up to four cycles with a gradual decrease. This fall in performance can be attributed to the poisoning effect of degraded products on the active sites of the catalyst. This effect causes a blockage of solar radiation on the surface of the catalyst. The loss of material during the successive washing can also contribute to this deficiency in performance [44,45]. Nevertheless, the nanohybrid material showed satisfactory potential for long-term repeated use for the removal of dyes from wastewater. With the incorporation of very cheap kaolinite in large amounts and the ability of nearly complete and fast removal of azo dye with long-term reusability, it is very evident that this nanohybrid is a strong candidate for industrial scale uses.

Adsorption Isotherm
Adsorption isotherm provides valuable insights into the nature and mechanism of adsorption. The equilibrium adsorption data in dark was tested by plotting in Langmuir and Freundlich adsorption isotherm equations ( Figure 15). The bar chart showed that the nanohybrid displayed a very satisfactory removal performance up to four cycles with a gradual decrease. This fall in performance can be attributed to the poisoning effect of degraded products on the active sites of the catalyst. This effect causes a blockage of solar radiation on the surface of the catalyst. The loss of material during the successive washing can also contribute to this deficiency in performance [44,45]. Nevertheless, the nanohybrid material showed satisfactory potential for long-term repeated use for the removal of dyes from wastewater. With the incorporation of very cheap kaolinite in large amounts and the ability of nearly complete and fast removal of azo dye with long-term reusability, it is very evident that this nanohybrid is a strong candidate for industrial scale uses.

Adsorption Isotherm
Adsorption isotherm provides valuable insights into the nature and mechanism of adsorption. The equilibrium adsorption data in dark was tested by plotting in Langmuir and Freundlich adsorption isotherm equations (Figure 15). The value of the linear regression correlation coefficient (R 2 ) was higher in the Langmuir isotherm plot (R 2 = 0.98862) than the Freundlich isotherm plot (R 2 = 0.95414), i.e., the experimental adsorption values were better fitted in the Langmuir isotherm model. The strong correlation of equilibrium adsorption data with Langmuir isotherm is indicative of homogeneous and monolayer adsorption of anionic Orange G molecules on the protonated chitosan part of the quaternary nanohybrid. The isotherms data were analyzed, and the list of the obtained parameters is provided in Table 3. The value of the linear regression correlation coefficient (R 2 ) was higher in the Langmuir isotherm plot (R 2 = 0.98862) than the Freundlich isotherm plot (R 2 = 0.95414), i.e., the experimental adsorption values were better fitted in the Langmuir isotherm model. The strong correlation of equilibrium adsorption data with Langmuir isotherm is indicative of homogeneous and monolayer adsorption of anionic Orange G molecules on the protonated chitosan part of the quaternary nanohybrid. The isotherms data were analyzed, and the list of the obtained parameters is provided in Table 3. The kinetics of the dye removal process were studied using the pseudo-first-order and pseudo-second-order kinetic models. Figures 16 and 17 shows the pseudo-first-order and pseudosecond-order kinetic plots for the adsorption of Orange G on the nanohybrid, respectively.  The kinetics of the dye removal process were studied using the pseudo-first-order and pseudo-second-order kinetic models. Figures 16 and 17 shows the pseudo-first-order and pseudo-second-order kinetic plots for the adsorption of Orange G on the nanohybrid, respectively.   The value of R 2 was higher in the pseudo-second-order kinetic plot (R 2 = 0.99129) than the pseudo-first-order kinetic plot (R 2 = 0.97576). From the regression analysis, it suggests that to reach the equilibrium, the removal of Orange G dye followed the pseudo-secondorder kinetics. The higher correlation of experimental data with pseudo-second-order kinetics indicates the chemisorption of anionic Orange G on the positively charged chitosan surface through the electrostatic forces of attraction. The adsorption of Orange G on chitosan is immediately followed by a very fast catalytic degradation by the ternary component in the nanohybrid under solar radiation [23,46]. The kinetics data were analyzed, and the list of the obtained parameters is provided in Table 4. Table 4. Comparison of pseudo-first-order and pseudo-second-order parameters.

Conclusions
This study demonstrates significant insights into the suitability the prepared novel nanohybrid for removing hazardous dyes from industrial effluents. A very simple and cost-effective method has been reported in this study for the fabrication of the nanohybrid at room temperature (25 • C). The surface chemistry, crystallinity, morphology, elemental distribution, and thermal stability of the nanohybrid were thoroughly illustrated using FTIR, XRD, FE-SEM, EDS, and TGA techniques, respectively. The successful binding of chitosan with the ternary photocatalyst at the interface was understood from different physico-chemical characteristics of the nanohybrid from the starting TiO 2 , ZnO, kaolinite, and chitosan, which have been elaborately described with the help of the aforementioned analytical techniques. Very fast and nearly complete removal of Orange G from the aqueous solution by the reusable nanohybrid was the fascinating feature of this study. The quaternary nanohybrid containing 75% ternary photocatalyst (w/w) and 25% chitosan (w/w) showed better performance in dye removal efficiency of 97.4% compare to either the ternary photocatalyst [29] or the chitosan [23] alone. The contribution of both ternary photocatalyst and chitosan in dye removal was understood by carrying out experiments with the nanohybrid in dark. The degradation process followed the Langmuir isotherm and pseudo-second-order kinetics. Finally, it can be concluded that this study has shown tremendous promise for the widespread applications of this novel nanohybrid in removing hazardous pollutants from industrial effluents.