Document Type : Original Article
1 Department of Environmental Engineering, Ahvaz Branch, Islamic Azad University, Ahvaz, Iran.
2 Department of Chemistry, Faculty of Science, Shahrekord Branch, Islamic Azad University, Shahrekord, Iran.
3 Department of Environmental Health Engineering ,School of Health, Shahrekord University of Medical Sciences, Rahmatieh Shahrekord, Iran.
henols are among the important pollutants listed by the US Environmental Protection Agency and the European Union . 1-Naphthol, one of the derivatives of naphthalene, is the most significant industrial chemical that is widely used in the production of dyes, pharmaceuticals, and biochemical processes . Because of its oxidation through chemical and biological processes, naphthalene (the main coal tar constituent) enters the environment . The presence of hydroxyl group in the backbone of 1-naphthalene increases its solubility and mobility in natural aquifers. 1-Naphthalene toxicity is higher than naphthalene and derived aromatic hydrocarbons . Various treatment methods for wastewater containing phenolic compounds have been investigated using chemical and biological methods [5, 6].
Nevertheless, the aforementioned methods have their limitations and disadvantages . Recently, new advanced oxidation processes have been considered [8-12]. Titanium dioxide (TiO2) as a semiconductor is a highly effective and reflective catalyst compared to other semiconductors. TiO2 is non-toxic, photo corrosion-resistant, cheap, and suitable for working with sunlight. Pure TiO2 is a weak photon absorber within the visible part of the solar spectrum because of its large distance of the energy bond (Anatase; 3.2 eV, Rutile; 3.05 eV) [13-16]. This property has led to the development of TiO2 nanoparticles with several novel strategies to alter their ultraviolet and optical response to the visible spectral range so that visible light can be efficiently used in the solar spectrum main part . Therefore, some methods like noble metals and anions (S, F, N, C)-doping are being used to convert this inherent property of TiO2 and produce a new photocatalyst capable of maintaining its photocatalytic activity under sunlight [18-20]. Sulfur anions-nitrogen doped with TiO2 creates a gap between the two capacitance bands and a narrower conductivity, leading to adsorption in the visible region .
Recently, TiO2 powder nanoparticles have been extensively used. Many studies report that the TiO2 photocatalysts are immobilized on surfaces such as glass Microspheres (MS) [22, 23], silica , zeolites, and nanotubes because of problems such as repetitive mixing throughout work, the expensive filtration and centrifugation of solutions for catalyst recovery, nanoparticles dispersion in solution and blockage of light, and the like. In the literature, the use of glass beads for catalyst deposition has been of considerable interest [25, 26]. In this study, the new catalyst N, S-TiO2 coated on Silica Sulfuric Acid (SSA) was prepared. The SSA was synthesized according to previous studies and should be prepared by reaction of silica glass beads with chlorosulforic acid . The immobilized N,S-TiO2 nanoparticles on SSA were evaluated using Energy-Dispersive X-ray (EDX), Scanning Electron Microscope (SEM), and X-Ray Diffraction (XRD). In addition, the optimal removal conditions of 1-naphthol are investigated using pH, irradiation time, and 1-naphthol concentration under visible light. Then, 1-naphthol removal reaction kinetics is measured.
2. Materials and Methods
Synthesis of photocatalyst
The chemicals used in the experiments were obtained without further purification. 1-Naphthol was obtained from Merck Co. in Germany. The water employed in all studies was double distilled. Because of the immobilization of the prepared sol of tetrabutyl orthotitanate on a substrate, the glass MS with 500 µ in diameter made of glass beads was used. SSA was prepared according to previous studies  through silica glass beads reaction with chlorosulforic acid (Figure 1). N,S-TiO2 thin film coated on SSA was prepared via tetrabutyl orthotitanate hydrolysis in the presence of SSA instead of glass beads using the sol-gel method following previous work.
Study of photocatalyst properties
The crystallinity and particle size of the prepared N,S-TiO2 thin film on SSA and pure SSA (as compared) were studied using XRD patterns gathered within the range of 20-80 (2θ) with a Philips X (X-Ray Tube Anode: Cu Wavelength: 1.540598 °A [Cu Kα] Filter: Ni). Using the Scherrer equation, the mean size of crystalline particles of the anatase phase was calculated. The bandgap of N,S-TiO2/SSA was calculated by UV-Vis with Shimadzu UV-1800 spectrophotometer and compared with a band gap of N,S-TiO2 coated on glass beads. The surface morphology of N,S-TiO2 thin film on SSA was investigated using Zeiss EVO 15 SEM equipped with an XRD spectrometer to analyze its elements.
Optical activity of photocatalyst investigation
In the experiments, 1 g of 1-naphthol was dissolved in 500 mL of naturally distilled water (pH 7) and diluted to 1000 mL to prepare different solution concentrations. The solution was spun using a peristaltic pump within a reactor with a flow rate of 20 mL/min. The primary concentrations of 1-naphthol solution were as follows: 5, 15, 25, 40, 50 mg/L. The solutions were prepared to replicate each concentration at least three times, and only one catalyst bed was recycled for each of the three replicates. Each usage was followed by washing the catalyst multiple times with distilled water, sonicating, and drying in an oven at 90°C for 90 min and using it again. The glass MS containing N,S-TiO2/SSA thin layer is distributed in four optical quartz tubes (0.8 cm in inner diameter and 20 cm in height). They are then exposed to visible light in a dark room (70×70×100 cm) using a 400 W lamp source. Then, 4.5 g of glass MS containing N,S-TiO2/SSA thin film was used in each phototube. Next, they were immobilized in a mirror. There was a 20 cm distance between glass tubes and lamps in the dark chamber. An air conditioner pump and a cold water tank, including a valve, were employed to maintain constant the temperature at 30°C within the reactor. The heat of the lamp produced a maximum temperature of 40°C in the dark chamber. The reactor used for photocatalytic investigation is shown in Figure 2.
Using a UV-Vis spectrophotometer (PerkinElmer, America), the remaining concentration of the 1-naphthol solution was obtained at a maximum wavelength of 213 nm. Then, the 1-naphthol degradation yield was computed via Equation 1.
C0 is the 1-naphthol primary concentration, Ct is the 1-naphthol remaining concentration after time t, and ƞ is the 1-naphthol elimination percentage. The trials were done triplicate, and the average value was considered.
1-naphthol extraction and Gas Chromatography-Mass Spectrometry (GC-MS) analysis
To recognize the intermediate compounds created by photo-oxidation reactions of 1-naphthol with N,S-TiO2/SSA catalyst, 1-naphthol was extracted from an aqueous environment after irradiation, and the solution was injected into the Gas Chromatography-Mass Spectrometry (GC-MS) device . We used a gas chromatography (Agilent Technologies 7890A model GC) device connected to the mass spectrometer (Agilent Technologies 5975C model) with a 30 m long, 0.25 m in outer diameter, and 0.25 in inner diameter HP5-MS column. As a carrier, helium was applied at a flow rate of 2 mL/min. Then, a total volume of 0.1 µL of the extracted solution sample was injected into the GC-MS.
3. Results and Discussion
Properties of photocatalyst
To do the initial analysis and calculate the weight and atomic percentage of the elements contained in the N,S-TiO2/SSA nanocatalyst, we employed EDX analysis. Figure 3, parts a and b show EDX analysis of N,S-TiO2/SSA thin film. Also, Figure 3, parts c, d, and e display their corresponding SEM images. Figure 3, parts f, g, and h show SEM images of N,S-TiO2 thin film on pure glass MS. Figure 3b shows the peaks of the N,S-TiO2 thin film coated on SSA, confirming the existence of Ti and Si in the presence of N and S in the TiO2 thin film structure. It is noteworthy that the presence of magnesium, sodium, and calcium elements in the EDX analysis spectrum is associated with the glass MS structure. EDX analysis (Figure 3b) displays the peaks associated with the presence of N at 0.5 keV and S at 2.2 keV. The peak of Ti is exhibited at about 4.5-5 keV. As shown in Figure 3b, the elemental analysis of N,S-TiO2/SSA thin film indicates that the sample is composed of oxygen (36.11 wt%), silicon (18.35 wt.%), sodium (3.91 wt%), magnesium (1.32 wt%), calcium (5.13 wt%, which can be attributed to glass MS), titanium (24.74 wt.%), sulfur (0.89 wt%), and nitrogen (9.54 wt%), indicating the presence of doped N,S atoms in the new TiO2 photocatalytic layer. The EDX analysis results show that the percentage of sulfur atoms in the N,S-TiO2/SSA catalyst is higher than that of the N,S-TiO2 coated on pure glass MS, which can be attributed to the existence of sulfuric functional groups containing sulfur atoms on SSA. Figure 3, parts c, d, and e show the SEM images of N,S-TiO2/SSA.
Compared to the previous studies, the thickness of N,S-TiO2 thin film coated on SSA (3.32 µm) is higher than that of N,S-TiO2 thin film coated on pure glass MS (809.93 nm) (Figure 3g). The sulfonic acid groups made a covalent bond with a hydroxyl group on the glass MS surface. The hydroxyl group of sulfuric acid on the surface of the glass MS establishes a good interaction with the prepared sol of tetrabutyl orthotitanate via hydrogen bonding. As a result, a thicker layer of N,S-TiO2 immobilized on the surface of the SSA is created and causes the 1-naphthol molecule to be more adsorbed on the catalyst surface and increases the time required for the photocatalytic degradation process on the surface. Figure 3e illustrates the 5-10 nm nanosized N,S-TiO2 particles coated on SSA, which are smaller than the nanosized N,S-TiO2 particles coated on pure glass MS, i.e., 35-50 nm.
Figure 4 parts a and b display the XRD pattern of pure SSA and N-S-TiO2/SSA, respectively. Figure 4a illustrates the XRD pattern of pure SSA, showing the amorphous solid (blank). The XRD pattern of Ti element in synthesized photocatalyst is shown in Figure 4b for the anatase phase (red line) and rutile (blue line) phase, respectively. The crystal nanoparticles’ average size in N,S-TiO2 thin film-coated at peak 101 Å on SSA (based on XRD pattern) was obtained at 10 nm via the Scherrer equation. The characteristic peak at 2θ was obtained to be 25.348, signifying the anatase phase, and the characteristic peak at 2θ=27.32 is a trace of the rutile phase in the structure of N,S-TiO2 coated on SSA. The comparison of the XRD results of N,S-TiO2/SSA, and N,S-TiO2 coated on the glass MS indicates that the rutile phase is observed in the N,S-TiO2/SSA structure, while no rutile phase is seen in the N,S-TiO2 catalyst immobilized on the glass MS.
Differential Reflectance Spectroscopy (DRS) spectrum analysis of pure TiO2 and N,S-TiO2/SSA is displayed in Figure 5. Tauc plot technique (Tauc) was used to calculate the nanostructures’ optical bandgap energy using the Kubelka-Munk model . These separately measured values were equal to an energy gap of 2.72 eV for N,S-TiO2/SSA thin film, 3.2 eV for TiO2 thin film, while the energy gap for the thin film of N,S-TiO2 coated on glass MS is 2.98 eV . As can be observed, the effect of the addition of sulfur and nitrogen to the TiO2 crystal structure causes a narrower energy gap and transfers the TiO2 photocatalytic activity to the visible region . The comparison of the energy gap of N,S-TiO2/SSA (2.72 eV) and N,S-TiO2 coated on glass MS (2.98 eV) shows that the activity of N,S-TiO2/SSA in the visible light will be greater than that of the N,S-TiO2 coated on glass MS.
Photocatalytic degradation of 1-naphthol
Figure 6 shows the overlay UV-Vis spectrum of 1-naphthol concentration removal within 60 minutes (0-60). It should be noted that 1-naphthol has two maximum wavelengths of 213 nm and 230 nm. As a result, from the 55th minute onwards, the overall shape of the spectrum changes, showing the production of products other than 1-naphthol. It was found that from the 55 minutes onwards, the 1-naphthol molecule was converted to another intermediate product. The optimal time for 1-naphthol elimination via this photocatalyst was thus evaluated within 50 minutes. All statistical calculations for removing the 1-naphthol were then considered for up to 50 minutes. To identify the produced compounds in photodegradation, the samples were injected into GC-MS. All kinetic results between adsorption and concentration at 213 nm have been achieved due to the linear relationship between absorbance and 1-naphthol concentration at 213 nm based on Beer Lambert’s law.
To obtain the optimum pH factor for 1-naphthol degradation, the impact of different pH values on the removal efficiency of 1-naphthol under visible light was investigated. The preparation of samples with a primary 1-naphthol solution concentration of 5 mg/L was done at pH values of 3, 5, 7, and 9. The samples were obtained and investigated at times of 0, 5, 10, 15, 20, 25, 30, 35, 40, 45, and 50 min on the catalyst’s surface. To eliminate the effect of adsorption on removing 1-naphthol, all solutions were rotated for 45 minutes without the presence of light in the chamber. Then, according to the standard method, the samples absorption rate was read using a spectrophotometer at 213 nm, and the removal percentage of 1-naphthol was calculated by Equation 1. The results are shown in Figure 7. According to Figure 7, the optimum pH factor for degradation of 1-naphthol is equal to 5. The higher removal efficiency of 1-naphthol happens in an acidic environment owing to the accelerated formation of hydroxyl radicals and being absorbed on the N,S-TiO2 nanocatalyst surface. The 1-naphthol contains hydroxyl groups that TiO2 can absorb. TiO2 surface is thus positively charged and easily exposed to photo-oxidation, but in the basic pH conditions, the TiO2 surface is negatively charged, the hydroxyl functional group 1-naphthol is converted to hydroxyl anion and repels TiO2.
Then, 1-naphthol solutions were made with concentrations of 5, 15, 25, 40, and 50 mg/L at constant pH of 5 (as optimum pH). Figure 8 shows the greatest concentration of 1-naphthol removal obtained under visible light at 25 mg/L for N,S-TiO2 coated on glass MS with efficiency removal of 71% (8a) and 25 mg/L for N,S-TiO2/SSA with efficiency removal of 92.12% (8b) (P<0.05).
Kinetic of 1-naphthol photocatalytic degradation
The kinetic of 1-naphthol degradation by N,S-TiO2/SSA was shown to follow the quadratic Equation 2.
Where, t is the time of reaction (minute), K shows reaction rate constant (1/min), and C0 and Ct denote the primary and secondary concentration of 1-naphthol post-reaction in mg/L at t=0 and t=t, respectively.
The contact time was changed up to 50 min with different concentrations of 1-naphthol in the exposure of N,S-TiO2/SSA to perform the kinetics experiments. Using the correlation coefficient, the proportionality of the regression equation of the samples with the data was displayed. By comparing between R2 coefficients of all samples, the kinetic model analysis of 1-naphthol degradation was carried out. Figure 9 shows the kinetics graphs of 1-naphthol removal in 1/C versus irradiation time. Considering the line 1/C slope versus time, the rate constants were obtained. The R2 regression coefficient for the second-order kinetic graph was greater than 0.9. It is noteworthy that in the present study, the total time of 1-naphthol removal is 50 min. This result is evident because the 1-naphthol adsorption pattern disappears entirely within 50 minutes. From 50 min onward, the quinoline compound is characterized by adsorption spectrum as an intermediate because of the optical decomposition of 1-naphthol. The 1-naphthol kinetic reaction was thus investigated from 0 to 50 min and assessed based on the second-order kinetics. The previous literature has reported photo-oxidation degradation kinetics of 1-naphthol during degradation time and they report second order kinetics which is in good agreement with the results of this study [31-33].
The N,S-TiO2/SSA reusability was investigated for the 1-naphthol degradation at a primary concentration of 25 mg/L under visible light. The catalyst was used five times, and the results of 1-naphthol degradation show the ability to stabilize light as a percentage of 1-naphthol degradation under visible light. After the destruction was completed, the catalyst was isolated and washed with an excess of deionized water.
Intermediate compounds produced through naphthalene degradation
Using Agilent 5975C model GC-MS, we investigated the intermediate compounds produced through 1-naphthol photodegradation in the exposure of N,S-TiO2/SSA. For this purpose, the samples were extracted by dichloromethane solvent and then injected into GC-MS. Figure 10 shows the GC spectrum for intermediate compounds produced from photo-oxidation of 1-naphthol using N,S-TiO2/SSA catalyst during irradiation at 0, 10, 40, and 90 minutes. The intermediate compounds were described by considering the retention time and device library assessment based on the interpretation of the mass spectrum.
Jafari et al.  reported 1-naphthol as one of the intermediate compounds produced post naphthalene photo-oxidation. They proposed the oxidation mechanism by OH radicals for 1-naphthol removal, which corresponds to the compounds identified from the mass spectrum in this study. The photo-oxidation mechanism for 1-naphthol removal in the presence of OH radicals is presented in Figure 11.
The intermediate compounds include phthalic acid (9), 1, 2-naphthalenedione (12) 1, 4-naphthalenedione (4) and 2-carboxy-cinnamaldehyde (13). The GC-MS results after 90 minutes confirmed the removal of many intermediates and their eventual conversion to CO2 and H2O gases (Figure 11).
Studies on the removal of naphthalene have been performed by various methods, as shown in Table 1. Adsorption, oxidation, and photocatalytic processes are common methods in that order.
In this study, N,S-TiO2/SSA photocatalyst synthesis was successfully performed using the sol-gel method. The SEM analysis revealed the nanosized thin film of N,S-TiO2/SSA to be about 5-10 nm. Moreover, the DRS results of N,S-TiO2/SSA indicated the reduction of the energy gap (0.48 eV). The obtained results indicated that the energy gap band was narrowed, and the N,S-TiO2/SSA optical activity was directed towards visible light. The results of the study of 1-naphthalene solutions at various concentrations in the exposure of N,S-TiO2/SSA show that the kinetic equation of 1-naphthol removal follows the second-order model and the best removal conditions of 1-naphthol happen at pH=5, 1-naphthol primary concentration of 25 mg/L, under visible light within 50 minutes. The maximum removal efficiency of 1-naphthol under visible light was 92.12%. The GC/MS study results show the production of some intermediate compounds that are mineralized after another 100 minutes of contact time. It is suggested that the efficiency of N,S-TiO2/SSA photocatalysis for eliminating the total polycyclic aromatic hydrocarbons.
Compliance with ethical guidelines
There was no ethical consideration to be considered in this research.
This study was supported by Ahvaz Branch, Islamic Azad University, Ahvaz.
Conceptualization and Supervision: Farhad Mahmoodi: Study design and concept, literature review, structuring; Methodology: Farhang Tirgir and Mehraban Sadeghi; Data analysis and Writing-original draft, and Writing-review & editing, and project administration: Jalilzadeh.
Conflict of interest
The authors declared no conflict of interest.
The authors would like to thank the Research Council for their generous support regarding this research.