Environ Eng Res > Volume 28(1); 2023 > Article
Singh and Mishra: Removal of chlorhexidine digluconate from aqueous solution by heterogenous photocatalysis using sunlight-driven Ni-doped TiO2 material

### Abstract

Photoactive Ni-TiO2 was synthesized through green hydrothermal method with preferential photocatalytic performance in visible and solar light for synthetic and formulated wastewater treatment. Incorporation of this transition metal into TiO2 was examined by XRD, FTIR, UV–visible DRS, XPS, SEM-EDS and HRTEM analysis. According to the Langmuir–Hinshelwood model, the photodegradation of the chlorhexidine digluconate under solar (R2=0.986) and simulated visible light (R2=0.982), follows a pseudo-first-order kinetics. The interaction of operational fractions, such as S/C ratio, irradiation time, and pH of the reaction mixture, were evaluated using the RSM. Although complete mineralization of CHD was not achieved using Ni-TiO2 under visible light, but the parent compound was mineralized to some extent, as demonstrated by TOC reduction (85.71%-synthetic wastewater and 61.17%-formulated wastewater), UV254 (89.91% synthetic wastewater and 55.39%-formulated wastewater) and UV280 (68.23%-synthetic wastewater and 68.23%-formulated wastewater) absorbance variations. Based on the identified transformed products, the possible degradation pathway was proposed and bacterial susceptibility test on Bacillus cereus DPAML065 was performed to evaluate the toxicity of oxidation intermediates. Comparative studies about energy consumption and removal efficiency during simulated visible light/Ni-TiO2 and sunlight/Ni-TiO2 mediated treatment system for formulated wastewater revealed that sunlight/Ni-TiO2 mediated treatment system was high energy efficient (1.67 kWhKg−1) system.

### 1. Introduction

Although personal care products (PCPs) have been used for decades, their fate and discharge into the aquatic environment only has recently been identified as one of the most significant environmental chemistry issues. In accordance with the Water Framework Directive (2000/60/EC of the European Parliament and Council) and other legal statutes (Decision 2455/2001/EC, Directive 2008/105/EC), various organic pollutants including PCPs have been identified as priority pollutants in the environmental strategy of EU against water pollution [1]. These compounds are formulated to be physiologically active and resistant to biodegradation, which significantly increases their presence in aquatic environment and are labelled as “pollutant” [2]. The principal pathway of these compound into the aquatic ecosystem is through excreta from human or animal urine or faces [3]. The model compound chlorhexidine digluconate (CHD) is widely used as a disinfectant in handwash, sanitizer, toothpaste, mouthwash, and cosmetic preservatives. When the COVID-19 pandemic broke out, the use of personal care products such as disinfectants soared dramatically in hospitals, health care facilities, and households all around the world [4]. They are excreted directly into the environment after usage, without being modified or treated in any way. The long-term exposure of CHD is associated with harmful effect on human health. Even though small concentration of CHD has received little attention because it was found that transformed products render the total mineralization of parent compound. Additionally, monitoring programs of the European Union for pharmaceutical and personal care products are not yet defined even though they could be future candidates for causing acute or chronic toxicity in the aquatic ecosystem [5].
Thus, removal of CHD is not adequate effective by conventional treatment process. Therefore, considering the disadvantages of all the conventional treatment, semiconductor nanostructure developed significantly in the field of photocatalytic application for efficient removal of organic pollutant [6]. High quantum efficiency, high chemical stability in aqueous media, inexpensiveness, and nontoxicity of TiO2 were recognized as a significant reason for their widespread acceptance as photocatalyst compared to another semiconductor. Nevertheless, some of their internal limitations including poor visible light consumption, decreased photogenerated electrons and holes pairs separation, and a lack of active species generation hampered their practical uses. Thus, the development of an efficient and new type visible light-driven (VLD) photocatalysts, as well as extensive synthesis and modification methods, are the main challenges in current studies to maximize the exploration of solar light [7, 8].
Very recently, transition metal/nonmetals (V, Cr, Mn, Fe, Ni, Cu) doped TiO2 are widely used photocatalysts for the removal of organic pollutant. In addition to this, wide band gap, high oxidation capacity, low cost, and remarkable potential application under visible and solar radiation of Ni doped TiO2 have been found to be promising photocatalyst [9]. To obtain the sunlight driven photocatalyst, the addition of Ni-content tuned the band gap from 3.03 to 2.54 eV for tetragonal and cubic structure of TiO2 and Ni-TiO2, respectively. Furthermore, similar ionic radius of Ti4+ (0.68 °A) and Ni2+ (0.72 °A), could be beneficial in the substitution of Ni2+ in the place of Ti4+ in the crystalline lattice of TiO2 [10]. Though various studies reported the modification of electrical and optical properties by controlling their microstructure for practical applicability [11]. The development of a simple and cost-effective method for producing high-yield nanostructured Ni-TiO2 toward sunlight driven photocatalytic application remains a major challenge.
Photodegradation involves number of independent and dependent variables because this manual optimization is quite difficult to carry out. Keeping the above facts, Response surface methodology (RSM) has been used to elaborate the interaction among the operating condition (pH, substrate to catalyst ratio and time) and their subsequent effect on photocatalytic activity with respect to mineralization of CHD, phenolic compound, and reduction of aromaticity during photocatalysis process [12]. The optimization of photocatalysis process has been carried out using Face Centered Central Composite Design (FCCD), resulting in a good estimate of the optimum response.
To understand the mineralization process of PCPs such as CHD into their transformed products and conversion of heteroatoms as well as functional group during photocatalysis process are again another challenging task. Monitoring of such intermediate generally carried out with the help of GC-MS, LC-MS and HPLC, which is the time consuming and costly procedural. The present study not only provide ideal scenario for photocatalysis process with different photocatalyst, but also opens a new avenue to understand the mineralisation of emerging pollutant coupled with simultaneous reduction of phenolic as well as aromaticity through Absorbance Slope Index (ASI) and spectral indices [13]. For example, UV absorbance at specific wavelengths (e.g., UVA 203, 204, 220, 230, 253 254, 260, 265, 272, 275 and 280), and ASI correlate well with the degradation CHD, aromaticity, hydrophobicity and transformed products. In previous studies, employment of spectral indices approach for characterization of DOM (aromatic components) has been demonstrated to be feasible, fast and easy tool [14].
In this research, a green hydrothermal synthesis approach was adopted, which is simple to use and can reduce time as compared to other conventional TiO2 modification techniques. The work describes the effect of Ni-doping on the photocatalytic activities of TiO2 under natural sunlight and simulated visible light with respect to degradation of the CHD, the mineralization rate (in terms of TOC) and UV absorbance (UV254 and UV280). Meanwhile, the presence of Ni-particle in TiO2 was validated by XPS, XRD, HRTEM and EDS. Radicals trapping experiment carried out to discuss the prominent radicals in the photodegradation system. A toxicity test of oxidation intermediates, high reusability, and electrical energy consumption, indicating the practical reliability and safe disposal of Ni-TiO2. The research also established the efficiency of photo mineralisation of CHD through HPLC and toxicity test of its oxidative by-products on the water bodies. Thus, current study provides the guidance for large scale applicability of Ni-TiO2 system in the field of pharmaceuticals and personal care products (PPCPs) with special emphasis on personal care products loaded wastewater.

### 2.1. Materials

Chlorhexidine digluconate (CAS # 18472-51-0-C9394) of 20% in H2O was purchased from Sigma-Aldrich. Titanium dioxide and other chemicals were procured from Merck (India) and Sigma-Aldrich. Chlorhexidine digluconate solution and formulated wastewater were prepared using a Milli-Q water system (Millipore). All chemicals are analytical graded.

### 2.2. Synthesis of Photocatalyst

The raw material and precursor used for preparation of Ni-doped TiO2 includes titanium tetra-isopropoxide, Ni(NO3)2·6H2O and HNO3. The clear aqueous solution was prepared by adding 10 mL of titanium tetra-isopropoxide into a beaker containing 60 mL of deionized water and 10 mL of isopropanol for 1 h of stirring. This clear solution was then added to 3 mmol of nickel (II) nitrate hexahydrate and 60 mL of 0.02M nitric acid for 2 h of continuous stirring. After obtaining clear solution, later add ammonium hydroxide drop-wise into the solution followed by vigorous stirring for 2 h to obtain a residue. The stirring was maintained for the next 6 h at a steady temperature of 80°C to ensure proper mixing of the solution. The resulting material was washed several times using distilled water to remove the impurities and dried in the air for 24 h. Thus, dried material was grinded in agate mortar and then calcined in the furnace at 600°C for 2 h [10, 15].

### 2.3. Characterization of Photocatalyst

The crystallinity, morphology, elemental analysis, optical measurement, and bandgap modification of the prepared photocatalyst were analyzed. Scanning electron microscopy (SEM) using Hitachi S-4300 type, High Resolution Transmission electron microscopy (HRTEM), energy dispersive spectroscopy (EDS) and selected area electron diffraction (SAED) patterns were used to examine the morphology, microstructure, distribution, and incorporation of elements on the TiO2. X-ray diffraction (XRD) were recorded using Cu-Kα (λ = 1.5406 Å) radiation on a Bruker D8 ADVANCE diffractometer to analyze the crystalline phase of the prepared material. The optical properties of the sample were recorded from UV–vis spectrophotometer (Perkin Elmer Lambda 900 spectrophotometer) equipped with BaSO4 powder was used as a reference for baseline study. Bandgap calculated from the modified Kubelka-Munk plot against wavelength ranging from 200–900 nm using diffuse reflectance spectra (DRS). The Brunauer Emmett Teller (BET) model was used to calculate specific surface area using the linear portion (P/Po = 0.05 – 0.2). The infrared spectrum of Ni-TiO2 was scanned through Bruker Vertex-70 Fourier transform infrared (FTIR) to identify the presence of functional groups of prepared material. X-ray photoelectron spectroscopy (XPS) were used to examine the oxidation state and charge compensation of the element present in the material using a VG 250 Escalab spectrometer equipped with an Al anode (Al-Kα = 1,486.7 eV) as an X-ray source. The textural and optical properties of the synthesized catalysts are given in Table S1.

### 2.4. Synthetic Wastewater Formulation

The pharmaceutical wastewater was prepared in the laboratory, based on the composition of real wastewater of the pharmaceutical industry with slight modifications [16]. The physiochemical characteristics of formulated wastewater such as pH, TOC, COD, BOD5 and Ultraviolet (UV) absorbance at 254 nm are presented in Table S2.

### 2.5. Experimental Setup and Procedures

The photocatalytic activity of Ni-TiO2 was investigated through CHD degradation using simulated visible light and natural sunlight as a source of irradiation. In a typical photocatalytic degradation experiment using simulated visible light, an aqueous solution of CHD was mixed and stirred well with Ni-TiO2 powder in a photocatalytic system consisting of a 1 L Pyrex reactor (diameter 96 mm and height 140 mm) with Hg lamp (200 W), mounted inside the system and a beaker with the same dimensions used for sunlight mediated experiment. To compare the performance of Ni-TiO2 in different light sources, the photocatalytic degradation of formulated wastewater containing CHD was also carried out using UV, visible, and solar light as irradiation sources [17]. The suspension was sonicated for 5 m and then irradiated with simulated visible light (300–420 nm and 40 m·W/cm2) or sunlight (30–40 m·W/cm2). The light intensity was measured by a radiometer (Delta OHM, LP-NET14). Aliquots (3 mL) were taken from the suspension at equal intervals, and centrifuged (4°C, 11,000 X g, 5 min) before being filtered with 0.22 m syringe filters for UV absorption spectra and TOC analyses.

### 2.6 Experimental Design Using Response Surface Methodology

Response Surface methodology was used to optimize three variables (S/C ratio, pH and time) with 3 different levels (+1, 0 and −1) for maximum CHD removal as response. The experiment design (DoE) was performed on the basis of the FCCD devised by Design Expert v7.0.0 software (SaMeep 104, State Ease, INC. Minneapolia (USA). A total of 20 different combinations were obtained with six center points in random order according to Central Composite Design (CCD) configuration for three factors. In this analysis, FCCD was used to model the percentage removal of CHD as quadratic model. Statistical validation was done by using “Analysis of variance” (ANOVA), correlation coefficient (R2), lack of fit, CV% and R2adj. A general second order polynomial model was selected and expressed by an Eq. (1) to investigate the effects of individual parameters as well as their synergistic interactive effects on the response variable [12].
##### (1)
$y=bo+∑i=13bi Xi+∑i=13bii Xi2+∑j=13∑j=13bij XiXj$
Where y is the response variable, bo is the constant, bi the linear coefficient, bii the quadratic coefficient, bij the interaction coefficient and Xi dimensional coded variables (X1 for the S/C ratio, X2 for the time and X3 for the reaction medium pH).

### 2.7. Analytical Procedure

The quantitative measurements of concentration of CHD and their degradation products were monitored by UV–vis spectrophotometer (Lab-tech, China) at 275 nm wavelength and LC-MS analysis (Thermo Scientific TSQ 8000 liquid chromatograph-mass spectrometer). TOC analyser (Shimandzu 5000) was used to determine the extent of CHD mineralization.
The Langmuir-Hinshelwood model has been carried out to study the modelling CHD degradation Eqs. (2) and (3).
##### (2)
$lnCtCo=-kobst$
##### (3)
$robs=-kobsCCHD$
Where, kobs (Reaction rate constant) was calculated from the slope by plotting a graph between $lnCtCo$ versus t and robs is the observed CHD degradation rate (mg L−1 min) in the photoreactor [18].
UV absorbance at various wavelengths (203, 204, 220, 230, 253 254, 260, 265, 272, 275 and 280) were employed to investigate the reduction in aromaticity of compound, residuals of phenols and ASI, calculation can be represented as [19]:
##### (4)
$ASI=0.56 [A254-A272A220-A230]$
Where A220, A230, A254 and A272 are the representative of UV absorbance at wavelength 220, 230, 254 and 272 nm, respectively.
The quantitative measurements of the conversions of CHD and the degradation products were validated on a High-Performance Liquid chromatograph (Phenomenex UK) equipped with a hyperclone (Eclipse plus C18 column; 3.5 × 4.6 × 100 mm) and connected to a UV-ViS detector. The spectrophotometer was set at 275 nm and 1.5 ml/mi. flow rate for 10 min. of retention time was used for the chromatograph. As a mobile phase solution of acetonitrile (70% v/v) and ultrapure water (30% v/v) was selected. Sample injection volumes were 10 μL and filtered by 0.2 μm syringe filters prior to injection [5]. Liquid Chromatography-Mass Spectrophotometer was used to investigate degradation pathway of CHD and its metabolites formation.

### 2.8. Bacterial Susceptibility Test

Bacillus cereus DPAML065 was used in a susceptibility test to determine the toxicity of partially/fully mineralized CHD using autoclaved Muller Hinton agar medium and petri plates at 121°C for 20 min. Approximately 1 mL of Bacillus cereus culture broth suspension was added to fresh medium and mixed. After incubation, this homogeneously mixed culture solution of bacteria and medium displays a confluent lawn of growth. Prior to the observation of the inhibition zone, the bacterial growth was incubated for 24 h at 37°C.

### 3.1. Characterization of the Photocatalysts

The XRD pattern showed the phase structure of the prepared photocatalyst in (Fig. 1(a)). The observed peaks at ~ 25° and 56° confirm the anatase form of tetragonal structure of pure TiO2 matched with (ICSD reference number 01-086-1155). In addition, the characteristic peaks of NiTiO3 at ~ 27°, 36°, 47° and 54° were ascribed the cubic structure of Ni-TiO2 matched with (ICSD reference number 01-075-0399) [20]. Thus, analysis provides a possible assumption that incorporation of Ni2+ into the TiO2 favouring the formation of NiTiO3 [21]. The intensity of peaks of undoped TiO2 decreased and slightly shifted due to the doping of metal; this revealed that Ni enter the TiO2 crystal lattice successfully. This Ni2+ could replace Ti4+ due to the similar ionic radius i.e. 0.72 Ao (Ni2+) and 0.68 Ao (Ti4+) and cause distortion as well as a defect in their lattice. Cubic crystal structure of Ni-TiO2 demonstrated that doping of nickel modifies the tetragonal crystal structure of TiO2 and Ti4+ lattice sites were occupied by Ni2+ as a substitutional impurity [11]. This phase transformation was observed with incorporation of Ni content can be explained by the fact that when Ni and Ti bond attached to O atom, Ti loses electron more easily than Ni atom due to the difference of electronegativity between Ti (1.54) and Ni (1.91). Thus, the large angle was found between the among Ni–O bonds than the Ti–O bonds this leads to the stronger interaction between the second Ti–O bonds and also due to the stronger polarity of the Ni–O bonds and hence results in deviation of crystal structure from tetragonal to cubic [22]. The Debye–Scherrer formula used FWHM data form the XRD peak to calculate the average crystallite sizes of the photocatalyst (Eq. (5)).
##### (5)
$D=Kλβcosθ$
Moreover, it was found that there is decrease in crystallite size of pure TiO2 (3.91 nm) due to doping of nickel in Ni-TiO2 (2.96 nm). Thus, Ni2+ tries to replace Ti4+ which may be better explained by the broadening of peaks due to defects formed by Ni2+ in TiO2 [23]. Fig. 1(b) depicts clearly the prominent peak and shifting of 2θ in prepared material (Ni-TiO2), which verifies the doping of Ni in TiO2 [24]. Doping of Ni2+ in TiO2 inhibits the size of crystallite and enhance the formation of anatase crystalline phase of TiO2. This smaller crystallite size of Ni-TiO2 particles were further validated by the scanning electron microscopy (SEM) and our findings are consistent with previous studies [10].
The SEM and High-resolution transmission electron microscopy (HRTEM) confirmed the smaller crystallite sizes of Ni-doped TiO2 particles. The SEM micrographs of undoped TiO2 clearly shows the uniform regular spherical particle distribution (Fig. 2(a), (b)). After loading of Ni, the surface of TiO2 sphere exhibits both spherical and slightly elongated rod-like porous structure (Fig. 2(c)~(h)). Furthermore, EDS analysis was also performed to verify and confirm the elemental composition of undoped TiO2 and the loading of Ni content in Ni-TiO2. The EDS spectrum shows the presence of Ti, O along with Ni were found confirming the undoped and Ni doped TiO2 [10]. The content of observed element in sample are mentioned in Table S1. HRTEM images and selected area electron diffraction (SAED) patterns show the presence of the lattice fringes and crystallinity of prepared material. Additionally, mapping shows the successful incorporation and equal distribution of metal ion onto Ni-TiO2 sample [25].
FTIR spectrum was recorded to elucidate the presence of chemical group on the surface of TiO2 and formation Ni-TiO2 (Fig. 1(d)). The broad hump on TiO2 and Ni-TiO2 showed absorption peak around 3,402.71 cm−1, which is characteristic peak of the OH-stretching vibration of surface absorbed water molecules. The peak representing Ti-O stretching bond were identified at 544 cm−1, which is the characteristic band of pure TiO2 sample [26]. Interestingly, characteristic peak of metal-oxygen vibrational bond were observed in the range of 700–400 cm−1, thus sharp absorption peaks around 500–450 cm−1 confirms the characteristic peak of metal titanate bond Ti–O–Ni [9]. Additionally, the characteristic peaks of Ni-OTiO2 and O-O stretching vibration were identified around 609.88 and 854.49 cm−1. The peaks around 1,380 cm−1 caused by substitution of the Ni2+ in place Ti4+ lattice sites [27, 28]. On other hand, the physically adsorbed water from H-O-H bending vibration, which was identified from the sharp peak at 1,630 cm−1. In contrast to pure TiO2, the Ti-O peaks for Ni doped TiO2 occurred at higher wavenumbers. For instance, Ti-O stretching bond of pure TiO2 and Ni-OTiO2 were identified at 544 and 609.88 cm−1, respectively. This could be due to the incorporation of Ni2+ into the TiO2 crystal structure which was further validated by XPS and confirmed by XRD. The high-resolution XPS spectra showed the chemical state of the elements and its effect in pure TiO2 and Ni-doped TiO2 (Fig. 3). The characteristics peak of Ti 2p3/2 and Ti 2p1/2 found at 458.89 and 464.77 eV, respectively indicated the existence of Ti4+ species [29]. On comparison of undoped TiO2, two distinct peaks attributed to Ni 2p3/2 and Ni 2p1/2 at binding energies of 854.3 and 872.1 eV were observed. The presence of a Ni-O band is suggested by the difference between these peaks, which is 17.6 eV [30]. This slightly shifting of the binding energy of Ti 2p corresponding to Ti 2p3/2 and Ti 2p1/2, respectively in Ni-TiO2 (Fig. 3(b)). The photoelectron peaks of the oxygen lattice (O 1s) in Ni-doped TiO2 i.e 529.76 is slightly lower than 530.15 eV of undoped TiO2 (Fig. 3(d)). Thus, change in state of oxygen and intensity of peak slightly toward the higher binding energy due to the difference in electronegativity of both element (Ti = 1.54 and Ni = 1.91) [31]. Consequently, transformation of titanium ions to higher valent state takes place by releasing plethoric electron to achieve charge balance in the TiO2 lattice following the introduction of Ni2+ [32]. Thus, this indicated the incorporation of Ni2+ ions in TiO2 lattice of Ni-doped TiO2 sample [25]. The surface hydroxyl group or chemisorbed water molecules also reflects peak in Ni-doped TiO2 at 532.30 eV [33]. These observation has been ascribed the successful formation of bond among Ni-O-Ti in the Ni-TiO2 material [10].
UV-vis spectrum analysis was used to determine the electronic structure of the samples, which provides the optical properties (such as absorption and band gap) through the irradiating light intensity. Kubelka-Munk and Tauc’s plots were used to convert the reflectance spectra for bandgap estimation (Fig. 1(e) and (f)). Undoped TiO2 and Ni doped TiO2 showed absorption bands ranging from 200 to 300 nm and 400 to 500 nm, respectively. It has also been observed that photocatalytic efficiency of Ni doped TiO2 is significant in the UVA lamp used in the experiment. Undoped TiO2 (3.03 eV) showed significant absorption below 400 nm due to the charge transfer between ligand (O2−) and metal ion (Ti4+) [34]. However, doping of nickel ion causes new electronic states in TiO2, which led to the narrowing of band gap and shifting of absorption into the visible region of Ni-TiO2 (2.54 eV). This electronic transition occurs from the valence band (2p level of oxygen) to conduction band (3d level of titanium) in pure TiO2. As a result of doping Ni2+ ions into the TiO2 lattice, a Schottky barrier forms at the interface, which inhibiting electron-hole recombination. The electron transport from Ni2+ (3d) to TiO2 conduction band is aided by this interfacial barrier [35]. Thus, obtained results demonstrated that Ni2+ doping could alter the crystalline structure, lowers the band energies, and widen the optical properties to the visible light.
The electrochemical impedance spectroscopy (EIS) provides information about the electrical property of material. The charge transfer process and the solid electrolyte interface film are responsible for the two semicircles in the high-to-medium frequency range, respectively. The Nyquist plot is drawn between the real and imaginary parts of the impedance, and a smaller arc radius indicates that photogenerated electron–hole pairs are effectively separated, and that interfacial charge transfer is rapid. The result shows the smallest arc radius of EIS Nyquist plot in Ni-incorporated material, which is indicating the most effective separation of electron–hole pairs and the fastest interfacial charge transfer (Fig. 1(c)) [36].
The surface area of pure TiO2 was 5.71 m2g−1 and increased to 12.19 m2g−1 for Ni-TiO2 materials. The increase in surface area implying the presence of Ni2+ in TiO2 lattice with their small crystallite sizes of Ni-TiO2 materials [37].

### 3.2. Regression Analysis for Photocatalytic Activity of Photocatalyst on CHD Removal

ANOVA is one of the statistical tools which is used to determine the significance and accuracy of quadratic model developed through response surface methodology. The regression analysis was carried out in order to obtain a good fit in the response function and to predict the catalytic behaviour of the photocatalyst using quadratic equation in terms of CHD removal efficiency. The three-dimensional response surface plots of CHD reduction over different catalyst have been shown in Fig. S1. The quadratic model has been developed to predict the catalytic activity and CHD removal as a function of X1(S/C), X2(pH), X3(Time) and calculated as three first order effect (X1, X2 and X3), interaction effect (X1X2, X1X3 and X2X3) and three second order effect (X12, X22 and X32). A polynomial model was used to represent the effects of individual parameters as well as their synergistic interactive effects on the response variable in Eqs. (6) and (7).
##### (6)
$CHD removal % (TiO2) γ=44.97-3.35X1+8.69X2+3.42X3+0.92X1X2-0.044X2X3-12X12-0.84X22-1.79X32$
##### (7)
$CHD removal % (N-TiO2) γ=47.19-2.66X1+9.32X2+4.02X3-2.26X1X2-0.54X1X3+1.17X2X3-14.32X12-2.41 X22-2.62 X32$
The results of the analysis of variance (ANOVA) (Table S3) represent the suitable model for photocatalyst during photocatalysis process. The P-value of the model, for both the photocatalyst, was < 0.0001, and the F-value was 27.84 and 396.87 for TiO2 and Ni-TiO2 respectively. These results confirmed that the model was highly significant, which is supported by the close agreement between the predicted and observed values. The R2 values were obtained 0.9616, and 0.9970 for TiO2 and Ni-TiO2, respectively, which implies good correlation in actual and predicted values for CHD removal and further confirmed the reliability of model [38]. Smaller P > F (< 0.05) values show the significance of the particular model and the higher contribution towards the response variable, while the greater P-value of terms indicates the insignificance of the model.

### 3.3. Photocatalytic Degradation and Mineralization Efficiency

The photocatalytic performance of prepared catalyst compared to TiO2 was investigated under simulated visible light and natural sunlight (winter season) for removal of CHD from synthetic water and formulated wastewater under optimized conditions. The results showed higher removal efficiency of Ni-TiO2 (90.34%-visible and 79.26%-solar light) as compared to TiO2 (23.64%-visible and 15.69%-solar light) under both simulated visible and solar light (Fig. 4(a)).
These photocatalytic results demonstrated that doping of transition metal onto TiO2 could improve the optical properties of Ni-TiO2 to visible range and give rise to new energy level in the bandgap of TiO2, which facilitates the inhibition of electron- hole recombination. SEM, EDX and TEM results demonstrated the modification of TiO2 and revealed the shape of synthesised material as a slightly elongated particle, with presence of characteristic element. XPS and XRD results revealed the amount and state of Ni2+ in TiO2 lattice that could promote the photocatalytic performance of prepared material. These results suggested that photocatalytic performance enhanced by doping of cationic metal in TiO2 with small radii, which could occupy the lattice site of Ti4+ with more oxygen vacancies [39]. Therefore, extended light absorption properties of Ni-TiO2 to visible region leads to the investigation of photocatalytic activity of Ni-TiO2 under natural sunlight. The results depicted slight decrease in the removal efficiency of Ni-TiO2 as compared to the visible region due to the variation in the intensity of sunlight [17]. This decreased solar intensity occurs due to the decrease in solar altitude and less transparency in the path of sunlight in the winter season [40]. Since, intensity of light is an important factor for the performance evaluation of a photocatalyst. Doping of metal on the surface of TiO2 can be accessible by hydroxyl group present on the surface of a material, which can trap both electron and hole generated. Evidently, trapping experiment has been carried out to evaluate the active radicals responsible for the mineralization process [41]. Isopropanol (IPA) (1%), 1.0 mM of potassium persulfate (K2S2O8) and ethylenediaminetetraacetic acid (EDTA) were used as scavengers of hydroxyl radicals (oOH), electron (e−), and holes (h+), respectively (Fig. 4(f)). This result indicates that IPA and EDTA inhibited the CHD degradation and further confirms that oOH and h+ were dominating reactive species. Therefore, the effect of photogenerated reactive species was found as decreased in order of oOH > h+ > e−. Therefore, it can be assumed that the generation of reactive species was influenced by intensity of sunlight which led to lowers the photocatalytic activity of Ni-TiO2 sample.
Apart from light absorption, solution pH, surface charge and surface area of the catalyst are also responsible for high photocatalytic activity of Ni-TiO2 compared to TiO2. The point zero charge (pHPZC) was measured to evaluate the surface charge of TiO2 (6.2) and Ni-TiO2 (6.8), respectively (Fig. 5(b)). The surface of catalysts was positively charged at the pH lower than their pHPZC values and negatively charged at the pH higher than their pHPZC values. Thus, higher degradation and mineralization of CHD takes place in alkaline condition (pH = 9.5), where surface of catalyst is negatively charged i.e. pH > pHPZC and CHD (pKa = 2.2 and 10.8) remain protonated which facilitates the interaction of catalyst and pollutant through electrostatic interaction [42]. Hence, alkaline condition enhances the photocatalysis process because the formation of hydroxyl radicals increased due to sufficient availability of OH in the reaction mixture.
The photocatalytic performance of Ni-TiO2 was investigated by using Langmuir–Hinshelwood (L-H) kinetic model, based on pseudo-first-order kinetics (Eq. (2), (3)) for a solid-liquid interface. Rate of reaction found by plotting the graph among ln(C/C0) versus t (Fig. 4). The rate of reaction decreases under solar light due to the variation of light intensity during the experiment. The results showed that photocatalysis of synthetic wastewater using Ni-TiO2 under simulated visible light and sunlight well fitted with pseudo-first kinetic order (Table 1). Among various photocatalytic conditions, Ni-TiO2 showed highest kCHD of 0.024 min−1 under optimized condition. Considering the fact that increasing the surface area enhanced the photocatalytic reaction rate because photocatalysis mainly occur on the surface of catalyst [43].
For industrial application and better understanding of the photocatalytic efficiency of prepared catalyst, comparative studies have been carried out to treat formulated wastewater. The results demonstrated that removal efficiency of Ni-TiO2 deduced for formulated wastewater treatment due to interference of other ions (Fig. 6(a)~(e)). The use of Ni-TiO2 for the removal of organic pollutant could be scaled-up under sunlight because of cost effective, reusability and easy applicability even though removal efficiency decreased.

### 3.4. Possible Pathway and Toxicity Test

The performance of photocatalyst was also estimated in terms of TOC removal and reduction of UV254. The oxidation process produces more harmful intermediates than the parent compound, which can be assessed using UV absorbance. The reactive organic fraction of wastewater loaded with organic pollutant is measured at a wavelength of UV254 nm.
The overall reaction during photo mineralization of CHD in the excess of oxygen under optimized experimental condition is validated by the equation (Eq. (8)) given below:
##### (8)
$C34H54Cl2N10O7+36O2+hϑ(370-400 nm)→34CO2+10NH3+2HCl+11H2O$
As can be observed, reduction in reactive organic fraction increased rapidly after 20 min during the photocatalytic process using Ni-TiO2 under visible (89.92%) and solar light (57.15%) (Fig. 4(e)). This difference in removal efficiency may be explained by the availability of sufficient solar light to generate a significant number of reactive species for the degradation of parent compound and their intermediate. Moreover, leftover reactive organic species in reaction mixture after photocatalysis process may be due to the formation of intermediate, which need more time to be removed [44]. A similar trend of mineralization was observed, where Ni-TiO2 (85.71%-visible and 71.79%-solar light) showed highest TOC removal as compared to TiO2 (21.70%-visible and 17.06%-solar) under visible and solar light, respectively (Fig. 4(d)). The results were validated using chromatogram of HPLC (Fig. S6). The toxicity test has been carried out for the successful applicability of photocatalyst in solar as well as visible light.
The possible degraded by-product and pathway during Ni-TiO2 mediated photocatalysis of formulated wastewater under simulated visible light and solar light was investigated by LC-MS spectroscopy. The peak at 505 and 507 m/z shows two isotopes of Cl atoms (35 and 37) attached to CHD in aqueous solution. This characteristics peak disappeared upon increasing the time during photocatalysis of formulated wastewater using Ni-TiO2 under visible light process. According to LC/MS results, transformation of the characteristics peak to 453,316,221,127 and 200 m/z belongs to the intimidated products of photooxidation process. According to LC/MS results and literature available, a possible pathway was proposed by substitution and addition [45, 46] (Fig. S2(a) and S3). OHo and h+ were produced as a reactive species in Ni-TiO2 mediated photocatalysis process, where OHo was dominating in the photocatalytic oxidation was investigated by trapping experiment. OHo attacked on benzene ring of CHD and involve breaking of C-Cl bond i.e., dichlorination of aromatic ring takes place by addition of OHo. Finally, resulted to the breakdown of biguanide moiety leads to the formation of smaller molecules of transformed products. In addition, quantification and mass identification of transformed product are beyond the scope of study.
Toxicological studies have been carried out to investigate the toxicity of transformed products. Bacillus cereus was subjected to bacterial susceptibility test, which is commonly found in human oral cavities. Inhibition zone of a standard solution of CHD, 30 mg/L concentration of sample, ciprofloxacin and amoxicillin antibiotics was 30, 15, 50 and 3 mm in diameter (Fig. S4). Negligible inhibition zone was observed for the degraded product after photocatalytic degradation of CHD. From the obtained results, it can be foreseen that the transformed products after photocatalytic degradation of CHD using Ni-TiO2 as a photocatalyst are non-toxic upon release in the environment.
Thus, higher mineralization of CHD was found using Ni-TiO2 as a photocatalyst under simulated visible light because modification of TiO2 enhanced the absorption of light with the wavelength > 400 nm and promotes the formation of sufficient number of reactive species. This reactive species attack phenyl ring of CHD during oxidation process and break up into short-carbon compounds. Atomic adsorption analysis of treated wastewater has been carried out to check the metal leaching during photocatalysis process. The analysis result indicated that the leaching concentration of Ni in treated water was found to be below detection limit depicting the stability of prepared catalyst during photocatalysis process [47].

### 3.5. Correlation between Spectroscopic indices and mineralization of CHD using TiO2 and Ni-TiO2

CHD is composed of phenyl aromatic carbon, presence of reactive and aromatic components in water after treatment referred as left-over organic compound. ASI could be the best way to quantify the left-over reactive organic compound in treated water in Eq. (4). Formation of aliphatic compounds and reduction in ASI, UV280 and TOC values in treated wastewater confirms the mineralization of CHD during photocatalysis reaction. ASI and TOC are considered as reactivity of activated aromatic group and oxidized organic carbon in terms of CO2 release. This spectral approach has been introduced to understand the cleavage of aromatic C=C and decrease in hydrophobic compound in treated water during photocatalysis process, which is measured at 280 nm in UV-spectroscopy. This reduction in the value of aromatic C=C content present in CHD with respect to time validated the reduction of TOC and mineralization of CHD.
Reduction of ASI and UV280 was observed, which validates mineralisation process of organic compound through spectral approach. Due to the solubility of phenol, removal of phenyl containing compound might have one reason for drastic reduction in TOC through photocatalysis. However, dominating reactive species such as OH·• and holes produced using TiO2 and Ni-TiO2 mediated photocatalytic degradation of CHD (Fig. S5), the mineralization of CHD (90.34%) with respect to TOC reduction (85.71%), aromaticity reduction (ASI-59.66%) and hydrophobic compound reduction (UV280-68.23%) was observed.
The comparative studies for photodegradation efficiencies of both the synthesised photocatalysts (TiO2and Ni-TiO2), it was found that doped-TiO2 photocatalyst was efficient for removal of recalcitrant organic pollutant with respect to mineralization of targeted compound and also remove reactive hydrophobic as well as aromatic compound from organic pollutant loaded wastewater.
The mineralisation process of CHD through spectral approach with respect to TOC reduction, aromaticity reduction (ASI) and hydrophobic compound reduction (UV280) was validated with HPLC results. The results showed decrease in characteristic peak of CHD with time after photocatalytic degradation process. Additionally, chromatogram of LC-MS confirms the breakdown of complex structure of CHD into smaller molecules due to presence of new peaks in the treated water. The interference and toxicity of transformed products were investigated with respect of reduction in ASI, TOC and UV280.

### 3.6. Comparison of Degradation Efficiency of Photocatalyst under Simulated and Sunlight with Energy Consumption in Treatment Process

The photocatalytic treatment of CHD using TiO2 and Ni-TiO2 under simulated and solar light were depicted the higher mineralization in visible light. In order to cost-effectiveness and large-scale applicability of treatment process, energy consumption was investigated using Eq. (9) and (10), respectively [17].
##### (9)
$Total power consumed (kWh)=Power used (kW)×Reaction time (h)60×1000$
##### (10)
$Total power consumption per CHD removal (kWhKg-1)=Power Concunption (kWh)[(CO-Cf)×(working volume (L)]$
Where, Co and Cf are the initial and final concentration of CHD in KgL−1. The energy consumption during photocatalytic treatment process for synthetic and formulated wastewater under simulated visible and sunlight was calculated. The experimental results showed higher mineralization for visible light as compared to the solar, which may be due to variation in intensity of solar light during the experiment led to the insufficient production of reactive species. Furthermore, energy was used simply for stirring during solar treatment, whereas visible mediated photocatalytic treatment required a high-powered lamp and stirrer. On comparing the treatment condition, sunlight mediated photocatalysis of synthetic wastewater using Ni-TiO2 showed lower energy consumption (1.87 kWhkg−1) with comparable CHD removal (79.26%) than other treatment condition (Table 2). The reusability of prepared catalyst was also investigated, and results showed good stability even after 3 cycles. Additionally, pH of the treated water was found near 7 to 7.8, which can be reused for a different purpose other than drinking (Fig. 5(a)).
Thus, results demonstrated that photocatalytic treatment of organic pollutant using Ni-TiO2 under sunlight could be used as economical and energy-efficient treatment process for large scale treatment system.

### 4. Conclusions

The synthesized Ni-TiO2 photocatalyst showed improved photocatalytic treatment due to the incorporation of Ni into the TiO2 lattice, exhibiting superior properties such as phase structure, crystallinity, crystallite size, morphology, separation of charge carriers and favourable for the shift of the bandgap into the visible region. SEM and TEM images confirmed the aggregation of particles and enhanced optical property due to the formation of bond between Ni and O atoms. The experimental results indicated removal of CHD using Ni-TiO2 under simulated visible light and natural solar light was ~90.34 and 79.26%, respectively. In addition, toxicity assessment of photooxidation products show the efficiency of treatment system and indicating the safe disposal of treated water into the aquatic environment. Thus, the preferential removal efficiency with lower energy consumption (1.87 kWhKg−1) indicated that Ni-TiO2 mediated heterogeneous photocatalysis under sunlight could be used for a larg-scale treatment system.

### Acknowledgment

The authors are very thankful for the financial support from Indian Institute of Technology (Indian School of Mines), Dhanbad under a Junior Research Fellowship scheme funded by Ministry of Human Resource Development (MHRD), Government of India, New Delhi to carry out this research work. We would also like to acknowledge Nanotechnology Research Centre (NRC), SRMIST for providing the instrumentation facilities.

### Notes

Conflict-of-Interest

The authors declare that they have no conflict of interest.

Author Contributions

A.S. (Ph.D. student) did Conceptualization, Methodology, Investigation, Formal analysis & Writing-Original Draft. B.K.M. (Associate Professor) did Supervision, Conceptualization, Writing - Review & Editing.

### References

1. Santiago-Morales J, Gómez MJ, Herrera-López S, Fernández-Alba AR, García-Calvo E, Rosal R. Energy Efficiency for the Removal of Non-Polar Pollutants during Ultraviolet Irradiation, Visible Light Photocatalysis and Ozonation of a Wastewater Effluent. Water Res. 2013;47(15)5546–5556. https://doi.org/10.1016/j.watres.2013.06.030

2. Das R, Sarkar S, Bhattacharjee C. Photocatalytic Degradation of Chlorhexidine-A Chemical Assessment and Prediction of Optimal Condition by Response Surface Methodology. J Water Process Eng. 2014;2:79–86. https://doi.org/10.1016/j.jwpe.2014.05.005

3. Khetan SK, Collins TJ. Human Pharmaceuticals in the Aquatic Environment : A Challenge to Green Chemistry. Chem Rev. 2007;107:2319–2364. https://doi.org/10.1021/cr020441w

4. Majumder A, Gupta AK, Ghosal PS, Varma M. A Review on Hospital Wastewater Treatment: A Special Emphasis on Occurrence and Removal of Pharmaceutically Active Compounds, Resistant Microorganisms, and SARS-CoV-2. J Environ Chem Eng. 2020;9(2)104812 https://doi.org/10.1016/j.jece.2020.104812

5. Das R, Sarkar S, Chakraborty S, Choi H, Bhattacharjee C. Remediation of Antiseptic Components in Wastewater by Photocatalysis Using TiO2 Nanoparticles. Ind Eng Chem Res. 2014;53(8)3012–3020. https://doi.org/10.1021/ie403817z

6. Aziz KHH, Omer KM, Mahyar A, Miessner H, Mueller S, Moeller D. Application of Photocatalytic Falling Film Reactor to Elucidate the Degradation Pathways of Pharmaceutical Diclofenac and Ibuprofen in Aqueous Solutions. Coatings. 2019;9(8)465 https://doi.org/10.3390/coatings9080465

7. Liu ML, Chen B, Bin Li RS, Li CM, Zou HY, Huang CZ. Dendritic CuSe with Hierarchical Side-Branches: Synthesis, Efficient Adsorption, and Enhanced Photocatalytic Activities under Daylight. ACS Sustain Chem Eng. 2017;5(5)4154–4160. https://doi.org/10.1021/acssuschemeng.7b00126

8. Aziz KHH, Miessner H, Mahyar A, et al. Degradation of Perfluorosurfactant in Aqueous Solution Using Non-Thermal Plasma Generated by Nano-Second Pulse Corona Discharge Reactor. Arab J Chem. 2021;14(10)103366 https://doi.org/10.1016/j.arabjc.2021.103366

9. Pavithra C, Madhuri W. Electrical and Magnetic Properties of NiTiO3 Nanoparticles Synthesized by the Sol-Gel Synthesis Method and Microwave Sintering. J Mater Res Technol. 2019;8(3)3097–3101. https://doi.org/10.1016/j.jmrt.2017.07.007

10. Blanco-Vega MP, Guzmán-Mar JL, Villanueva-Rodríguez M, et al. Photocatalytic Elimination of Bisphenol A under Visible Light Using Ni-Doped TiO2 Synthesized by Microwave Assisted Sol-Gel Method. Mater Sci Semicond Process. 2017;71:275–282. https://doi.org/10.1016/j.mssp.2017.08.013

11. Al Gabal MAEF, Angari YM, Obaid AY. Structural Characterization and Activation Energy of NiTiO3 Nanopowders Prepared by the Co-Precipitation and Impregnation with Calcinations. Comptes Rendus Chim. 2013;16(8)704–711. https://doi.org/10.1016/j.crci.2013.01.009

12. Kumari S, Jose S, Tyagi M, Jagadevan S. A Holistic and Sustainable Approach for Recovery of Phosphorus via Struvite Crystallization from Synthetic Distillery Wastewater. J Clean Prod. 2020;254:120037 https://doi.org/10.1016/j.jclepro.2020.120037

13. Priya T, Mohanta VL, Mishra BK. Performance Evaluation of Zirconium Oxychloride for Reduction of Hydrophobic Fractions of Natural Organic Matter. Sep Purif Technol. 2017;174:104–108. https://doi.org/10.1016/j.seppur.2016.10.003

14. Tu X, Meng X, Pan Y, Crittenden JC, Wang Y. Degradation Kinetics of Target Compounds and Correlations with Spectral Indices during UV/H2O2 Post-Treatment of Biologically Treated Acrylonitrile Wastewater. Chemosphere. 2020;243:125384 https://doi.org/10.1016/j.chemosphere.2019.125384

15. Guan B, Yu J, Guo S, Yu S, Han S. Porous Nickel Doped Titanium Dioxide Nanoparticles with Improved Visible Light Photocatalytic Activity. Nanoscale Adv. 2020;2(3)1352–1357. https://doi.org/10.1039/c9na00760a

16. Kumari V, Tripathi AK. Characterization of Pharmaceuticals Industrial Effluent Using GC–MS and FT-IR Analyses and Defining Its Toxicity. Appl Water Sci. 2019;9(8)1–8. https://doi.org/10.1007/s13201-019-1064-z

17. Priyanka K, Remya N, Behera M. Comparison of Titanium Dioxide Based Catalysts Preparation Methods in the Mineralization and Nutrients Removal from Greywater by Solar Photocatalysis. J Clean Prod. 2019;235:1–10. https://doi.org/10.1016/j.jclepro.2019.06.314.18

18. Nasseh N, Taghavi L, Barikbin B, Nasseri MA. Synthesis and characterizations of a novel FeNi3/SiO2/CuS magnetic nanocomposite for photocatalytic degradation of tetracycline in simulated wastewater. J Clean Prod. 2018;179:42–54. https://doi.org/10.1016/j.jclepro.2018.01.052

19. Priya T, Prakash P, Mishra BK. Understanding the Coagulant Activity of Zirconium Oxychloride to Control THMs Formation Using Response Surface Methodology. Ecotoxicol Environ Saf. 2018;159:28–37. https://doi.org/10.1016/j.ecoenv.2018.04.036

20. Karlsson . Metallic Oxides with the Structure of High-Speed Steel Carbide. Nature. 1951;1

21. Rodríguez-González V, Ruiz-Gómez MA, Torres-Martínez LM, Gómez R. Photocatalytic Decomposition of Synthetic Alizarin Red S by Nickel Doped TiO2. Top Catal. 2011;54(8–9)490–495. https://doi.org/10.1007/s11244-011-9612-2.22

22. Sharma SD, Singh D, Saini KK, et al. Sol-Gel-Derived Super-Hydrophilic Nickel Doped TiO2 Film as Active Photo-Catalyst. Appl Catal A Gen. 2006;314(1)40–46. https://doi.org/10.1016/j.apcata.2006.07.029

23. Sharma A, Chakraborty M, Thangavel R. Enhanced Photoelectrochemical Performance of Hydrothermally Grown Tetravalent Impurity (Si4+) Doped Zinc Oxide Nanostructures for Solar Water Splitting Applications. J Mater Sci Mater Electron. 2018;29(17)14710–14722. https://doi.org/10.1007/s10854-018-9608-9

24. Sahoo P, Sharma A, Padhan S, Udayabhanu G, Thangavel R. UV-Assisted Water Splitting of Stable Cl-Doped ZnO Nanorod Photoanodes Grown via Facile Sol-Gel Hydrothermal Technique for Enhanced Solar Energy Harvesting Applications. Sol Energy. 2019;193:148–163. https://doi.org/10.1016/j.solener.2019.09.045

25. Shao GN, Jeon SJ, Haider MS, Abbass N, Kim HT. Investigation of the Influence of Vanadium, Iron and Nickel Dopants on the Morphology, and Crystal Structure and Photocatalytic Properties of Titanium Dioxide Based Nanopowders. J Colloid Interface Sci. 2016;474:179–189. https://doi.org/10.1016/j.jcis.2016.04.024

26. Zhou X, Wang L, Liu X, Xu M, Liu X. Organic/Inorganic Hybrid Consisting of Supportive Poly(Arylene Ether Nitrile) Microspheres and Photocatalytic Titanium Dioxide Nanoparticles for the Adsorption and Photocatalysis of Methylene Blue. Compos Part B Eng. 2019;177:107414 https://doi.org/10.1016/j.compositesb.2019.107414

27. Fan J, Liu E, Tian L, Hu X, He Q, Sun T. Synergistic Effect of N and Ni2+ on Nanotitania in Photocatalytic Reduction of CO2. J Environ Eng. 2011;137(3)171–176. https://doi.org/10.1061/(asce)ee.1943-7870.0000311

28. She H, Zhou H, Li L, Wang L, Huang J, Wang Q. Nickel-Doped Excess Oxygen Defect Titanium Dioxide for Efficient Selective Photocatalytic Oxidation of Benzyl Alcohol. ACS Sustain Chem Eng. 2018;6(9)11939–11948. https://doi.org/10.1021/acssuschemeng.8b02217

29. Yoshinaga M, Yamamoto K, Sato N, Aoki K, Morikawa T, Muramatsu A. Remarkably Enhanced Photocatalytic Activity by Nickel Nanoparticle Deposition on Sulfur-Doped Titanium Dioxide Thin Film. Appl Catal B Environ. 2009;87:239–244. https://doi.org/10.1016/j.apcatb.2008.08.023

30. Wang Y, Zhang L, Li S, Jena P. Polyol-Mediated Synthesis of Ultrafine TiO 2 Nanocrystals and Tailored Physiochemical Properties by Ni Doping. J Phys Chem C. 2009;113(21)9210–9217. https://doi.org/10.1021/jp902306h

31. Li J, Zeng HC. Hollowing Sn-Doped TiO2nanospheres via Ostwald Ripening. J Am Chem Soc. 2007;129(51)15839–15847. https://doi.org/10.1021/ja073521w

32. Nagaveni K, Hegde MS, Ravishankar N, Subbanna GN, Madras G. Synthesis and Structure of Nanocrystalline TiO2 with Lower Band Gap Showing High Photocatalytic Activity. Langmuir. 2004;20(7)2900–2907. https://doi.org/10.1021/la035777v

33. Randeniya LK, Bendavid A, Martin PJ, Preston EW. Photoelectrochemical and Structural Properties of TiO2 and N-Doped TiO2 Thin Films Synthesized Using Pulsed Direct Current Plasma-Activated Chemical Vapor Deposition. J Phys Chem. 2007;111(49)18334–18340. https://doi.org/10.1021/jp075938u

34. Pelaez M, Nolan NT, Pillai SC, et al. A Review on the Visible Light Active Titanium Dioxide Photocatalysts for Environmental Applications. Appl Catal B Environ. 2012;125:331–349. https://doi.org/10.1016/j.apcatb.2012.05.036

35. Singla P, Pandey OP, Singh K. Study of photocatalytic degradation of environmentally harmful phthalate esters using Ni-doped TiO2 nanoparticles. Int J Environ Sci Technol. 2016;13(3)849–856. https://doi.org/10.1007/s13762-015-0909-8

36. Sun B, Zhou W, Li H, et al. Synthesis of Particulate Hierarchical Tandem Heterojunctions toward Optimized Photocatalytic Hydrogen Production. Adv Mater. 2018;30(43)1–8. https://doi.org/10.1002/adma.201804282

37. Zhang W, Gong Y, Mellott NP, Liu D, Li J. Synthesis of Nickel Doped Anatase Titanate as High Performance Anode Materials for Lithium Ion Batteries. J Power Sources. 2015;276:39–45. https://doi.org/10.1016/j.jpowsour.2014.11.098

38. Sonal S, Singh A, Mishra BK. Decolorization of Reactive Dye Remazol Brilliant Blue R by Zirconium Oxychloride as a Novel Coagulant: Optimization through Response Surface Methodology. Water Sci Technol. 2018;78(2)379–389. https://doi.org/10.2166/wst.2018.307

39. Hanaor DAH, Sorrell CC. Review of the Anatase to Rutile Phase Transformation. J Mater Sci. 2011;46(4)855–874. https://doi.org/10.1007/s10853-010-5113-0

40. Lawin AE, Niyongendako M, Manirakiza C. Solar Irradiance and Temperature Variability and Projected Trends Analysis in Burundi. Climate. 2019;7(6)1–20. https://doi.org/10.3390/CLI7060083.41

41. He D, Su H, Li X, et al. Heterostructure TiO2 Polymorphs Design and Structure Adjustment for Photocatalysis. Sci Bull. 2018;63(5)314–321. https://doi.org/10.1016/j.scib.2018.02.008

42. Sarkar S, Bhattacharjee C, Curcio S. Studies on Adsorption, Reaction Mechanisms and Kinetics for Photocatalytic Degradation of CHD, a Pharmaceutical Waste. Ecotoxicol Environ Saf. 2015;121:154–163. https://doi.org/10.1016/j.ecoenv.2015.04.036

43. Etacheri V, Roshan R, Kumar V. Mg-Doped ZnO Nanoparticles for Efficient Sunlight-Driven Photocatalysis. ACS Appl Mater Interfaces. 2012;4(5)2717–2725. https://doi.org/10.1021/am300359h

44. Rizzo L, Meric S, Guida M, Kassinos D, Belgiorno V. Heterogenous Photocatalytic Degradation Kinetics and Detoxification of an Urban Wastewater Treatment Plant Effluent Contaminated with Pharmaceuticals. Water Res. 2009;43(16)4070–4078. https://doi.org/10.1016/j.watres.2009.06.046

45. Ha Y, Cheung AP. New Stability-Indicating High Performance Liquid Chromatography Assay and Proposed Hydrolytic Pathways of Chlorhexidine. J Pharm Biomed Anal. 1996;14(8–10)1327–1334. https://doi.org/10.1016/S0731-7085(96)01763-3

46. Purdy KR. University of Bath. Palgrave Macmillan, Macmillan Publishers Ltd.. The Grants Register. 2021. London: Palgrave Macmillan; 1987. p. 897–898. https://doi.org/10.1057/978-1-349-95988-4_903

47. Alam U, Khan A, Bahnemann D, Muneer M. Synthesis of Co Doped ZnWO4 for Simultaneous Oxidation of RhB and Reduction of Cr(VI) under UV-Light Irradiation. J Environ Chem Eng. 2018;6(4)4885–4898. https://doi.org/10.1016/j.jece.2018.07.028

##### Fig 1
(a) XRD;(b) magnified XRD; (c) Nyquist plot; (d) FTIR; (e) DRS-spectra; and (f) Kubelka–Munk function photocatalysts TiO2 and Ni-TiO2.
##### Fig. 2
(a), (b) SEM, TEM, SAED and EDS images of photocatalysts TiO2; and (c)~(h) Ni-TiO2.
##### Fig. 3
XPS spectra of photocatalysts TiO2; and Ni-TiO2.
##### Fig 4
Photocatalytic removal of (a) CHD under solar and visible light; (b) pseudo-first order kinetic model under solar light; (c) pseudo-first order kinetic model under visible light; (d) TOC removal; (e) UV absorbance reduction and (f) Trapping experiment of photocatalysts TiO2; and Ni-TiO2.
##### Fig 5
(a) Cycle experiment of Ni-TiO2 in photocatalytic degradation of CHD under optimized condition; (b)Zeta potential of TiO2 and Ni-TiO2 at different pH and (c) Effect of pH on CHD degradation Ni-TiO2.
##### Fig. 6
Photocatalytic removal of formulated wastewater (a) CHD; (b) pseudo-first order kinetic model under solar light; (c) pseudo-first order kinetic model under visible light; (d) TOC removal; (e) UV absorbance reduction using TiO2; and Ni-TiO2.
##### Table 1
PFO Model Kinetic Parameters of Chlorhexidine Digluconate (CHD) Degradation by Different Photocatalyst during UV, Visible and Solar Photocatalysis
Photocatalysts Experimental conditions Removal efficiency R2 kobs value (min−1) Light source
TiO2 Co = 30 mgL−1, S/C = 1.8, pH = 7.6, Synthetic water 23.64 0.974 0.003 visible light
Co = 30 mgL−1, S/C = 1.63, pH = 8.2, Synthetic water 15.69 0.92 0.001 sunlight
Co = 30 mgL−1, S/C = 1.8, pH = 7.6, formulated wastewater 20.07 0.97 0.0028 visible light
Co = 30 mgL−1, S/C = 1.63, pH = 8.2, formulated wastewater 9.45 0.962 0.0035 sunlight

Ni-TiO2 Co = 30 mgL−1, S/C = 1.54, pH = 9.2, Synthetic water 90.34 0.982 0.0245 visible light
Co = 30 mgL−1, S/C = 1.98, pH = 7.89, Synthetic water 79.26 0.986 0.0119 sunlight
Co = 30 mgL−1, S/C = 1.54, pH = 9.2, formulated wastewater 90.34 0.976 0.022 visible light
Co = 30 mgL−1, S/C = 1.98, pH = 7.89, formulated wastewater 79.26 0.986 0.239 sunlight
##### Table 2
Energy Consumption in Synthetic and Formulated Wastewater Treatment Using Photocatalyst under Different Treatment Condition
Photocatalysts Experimental conditions Removal efficiency Working volume (L) Reaction time (h) Power Consumption (W) Power consumed/CHD removal (kWhkg−1)
TiO2 Co = 30 mgL−1, S/C = 1.8, pH = 7.6, Synthetic water and visible light 23.64 0.2 0.003 0.2 7.55
Co = 30 mgL−1, S/C = 1.63, pH = 8.2, Synthetic water and sunlight 15.69 0.2 0.001 1.17 70.66
Co = 30 mgL−1, S/C = 1.8, pH = 7.6, formulated wastewater and Visible light 18.79 0.2 0.0028 0.2 11.96
Co = 30 mgL−1, S/C = 1.63, pH = 8.2, formulated wastewater and sunlight 9.49 0.2 0.0035 1.17 44.58

Ni-TiO2 Co = 30 mgL−1, S/C = 1.54, pH = 9.2, Synthetic water and visible light 90.34 0.2 0.0245 0.2 1.88
Co = 30 mgL−1, S/C = 1.98, pH = 7.89, Synthetic water and Sunlight 79.26 0.2 0.0119 1.17 14.59
Co = 30 mgL−1, S/C = 1.54, pH = 9.2, formulated wastewater and visible light 84.34 0.2 0.022 0.2 1.94
Co = 30 mgL−1, S/C = 1.98, pH = 7.89, formulated wastewater and sunlight 71.51 0.2 0.239 1.17 14.68
TOOLS
Full text via DOI
Supplement
E-Mail
Print
Share:
METRICS
 0 Crossref
 0 Scopus
 564 View