# Photocatalytic Degradation of Phenolics by N-Doped Mesoporous Titania under Solar Radiation

Authors: Priti A. Mangrulkar; Sanjay P. Kamble; Meenal M. Joshi; Jyotsna S.  Meshram; Nitin K. Labhsetwar; Sadhana S. Rayalu
Journal: International Journal of Photoenergy
 (2012)

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## Abstract

In this study, nitrogen-doped mesoporous titania was synthesized by templating method using chitosan. This biopolymer chitosan plays the dual role of acting as a template (which imparts mesoporosity) and precursor for nitrogen.  BET-SA, XRD, UV-DRS, SEM, and FTIR were used to characterize the photocatalyst. The doping of nitrogen into TiO2 lattice and its state was substantiated and measured by XPS. The photocatalytic activity of the prepared N-doped mesoporous titania for phenol and o-chlorophenol degradation was investigated under solar and artificial radiation. The rate of photocatalytic degradation was observed to be higher for o-chlorophenol than that of phenol. The photodegradation of o-chlorophenol was 98.62% and 72.2%, while in case of phenol, degradation to the tune of 69.25% and 30.58% was achieved in solar and artificial radiation. The effect of various operating parameters, namely, catalyst loading, pH, initial concentration and the effect of coexisting ions on the rate of photocatalytic degradation were studied in detail.


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## Body

## 1. Introduction

Photocatalysis is a rapidly evolving and efficient technology for purification of water. It plays a vital role in degrading several toxic organic pollutants into less toxic or nontoxic and safe compounds by their partial and/or by their complete mineralization. Photocatalytic degradation process can be defined broadly as an aqueous phase oxidation process, which is based primarily on the attack of the hydroxyl radical, resulting in the destruction of the target pollutant or contaminant compound. Phenol and its derivatives have been listed by EPA as priority pollutants [1]. Recently, photocatalytic treatment of organic contaminants over titanium dioxide has been reviewed by Gaya and Abdullah [2]. It was reported that TiO2 is the best photocatalyst among all the photocatalysts. Moreover, TiO2 has been the most widely used photocatalyst owing to its nontoxicity, high stability, and its cost effectiveness. But there are few drawbacks associated with it like conventional TiO2 which has very low surface area (55 m2/g for Degussa P-25 TiO2) and low porosity and it can be activated only by irradiating with ultraviolet light (wide band gap energies, 3.0 eV for rutile and 3.2 eV for anatase) which is around 4–8% of solar radiation that reaches the earth surface. It is therefore of utmost importance to make TiO2 active in visible region. Sensitization of TiO2 by metal and nonmetal doping is one of the attempts in this direction. Nitrogen-doped titania has proved to be an effective means to extend the light absorption of titania from UV to visible region as in case of nitrogen doped titania there is substitution of lattice oxygen with nitrogen which tends to lower the band gap [3–6]. In recent years several efforts have been made to improve the surface area of titania by synthesizing mesoporous titania which possess high surface area and porosity. The preparation of mesoporous titania is reported by using a templating method. Templates are soft like surfactant or block polymer or they could be hard templates like porous silica and carbon [7–10]. Biological templates like insect wings, plant leaves, bacterial threads, and so forth, have also been reported for the synthesis of mesoporous titania [11–13]. Mesoporous titania with visible light absorption ability are promising as efficient photocatalysts. However, the usual preparation route of mesoporous titania and nitrogen doping is different, hence it is difficult to synthesize nitrogen-doped mesoporous titania by a simple route. Synthesizing mesoporous titania with nonmetal doping like nitrogen to enhance visible light activity seems to be promising area of research. Recently, one step-template-free solvothermal method to synthesize N-doped mesoporous titania microspheres was reported by Chi et al. [14], whereby mesoporous spheres were formed by crystallite aggregation from controlled alcoholysis of titania precursor and then reacting urea with titania to dope nitrogen in mesostructure. Horikawa et al. [15] also reported the synthesis of N-doped mesoporous titania by supercritical drying technique.In continuation with our previous work wherein we had reported the photo reduction of methyl orange dye by N-doped mesoporous titania, herein we investigated the photo oxidation properties of the synthesized photocatalyst. The photocatalyst has shown promising activity in phenol ando-chlorophenol photodegradation under visible light.


## 2. Experimental

### 2.1. Materials

All the reagents used for experimental studies were of analytical reagent grade. Methanol, acetic acid, ammonia, phenol,o-chlorophenol, sodium chloride, sodium carbonate, and sodium bicarbonate were obtained from Merck India ltd. Chitosan was procured from Chemchito India. Titanium isopropoxide was obtained from Acros India ltd. The stock solutions of phenol and o-chlorophenol were prepared in deionized water obtained from Millipore waters progard2 purification system. Plain solar intensity was measured in Watts per square meter using Lutron LX-102 light meter working on photocell principle.


### 2.2. Method

All the experiments were carried out in a cylindrical borosilicate glass reactor of 500 cm3capacity (Figure 1). The reactor was assembled with centrally mounted sparger surrounded by cooling coil. The same experimental setup was employed in the present investigation which was previously used by Kamble et al. [16]. The temperature of the reaction mixture was maintained near ambient by passing water through the cooling coil. 400 cm3 of solution (phenol/o-chlorophenol) was taken in the reactor and a known weight of the photocatalyst was added to the reactor. The solution was stirred in dark before exposing the reactor to concentrated sunlight from a compound parabolic reflector in order to find out the substrate adsorption effect. The concentration of phenol or o-chlorophenol in this filtered sample was treated as the zero time concentration (Ct=0) in each experiment before exposure to radiation. Air was sparged in the reactor through central sparger in order to keep the photocatalyst particles in uniform suspension. The position of the reflector was changed after a fixed interval of time with respect to the position of sunlight in order to maintain a constant band of light around the reactor. Samples were withdrawn at regular intervals of time for their analysis.Figure 1
Experimental setup of the solar reactor for photocatalytic degradation experiment.


### 2.3. Analysis

All the samples were withdrawn using a syringe, centrifuged, and then were immediately filtered through 0.45μ cellulose nitrate membranes. The phenol and o-chlorophenol concentration was measured on Knauer HPLC system equipped with Eurospher 100-10 C-18 column. The wavelength for detection of phenol and o-chlorophenol was 270 nm and 274 nm, respectively. The mobile phase used for analysis was methanol : water (50 : 50) v/v% and the flow rate was 1.2 cm3 min−1. The elution time for phenol and o-chlorophenol was 4.2 and 8.3 min, respectively. The solar experiments were carried out in the months of January 2008 to April 2008 in Nagpur, India (79°09′N, 21°09′E). During this period, the sky was brilliant blue, and the average solar intensity was approximately (±2%) constant at 950 Wm-2 as measured at the ground level. The experiments in artificial radiations were also carried out during the same period using Tungsten lamp (500 W).


### 2.4. Synthesis of N-Doped Mesoporous Titania

The synthesis of N-doped mesoporous titania has been previously reported by us and detailed elsewhere [17]. The ratio of chitosan and titania was changed to obtain mesoporous titania with different nitrogen content namely, N-doped M-TiO2 (1 : 1) and N-doped M-TiO2 (1 : 2) and N-doped M-TiO2 (1 : 3). The photocatalytic activity of all the three synthesized photocatalysts was evaluated for o-chlorophenol degradation. The % degradation of o-chlorophenol under solar radiation is as shown in Figure 2. It can be seen that highest percentage degradation was observed in case of N-doped M-TiO2 (1 : 2) followed by N-doped M-TiO2 (1 : 3) and N-doped M-TiO2 (1 : 1). The visible light activity of these photocatalysts is attributed to the nitrogen doping. The nitrogen partially replaces oxygen sites in TiO2. This replacement causes oxygen vacancies and amount of Ti3+ (TiO2 is reduced). These defects on the surface or in the bulk suppresses recombination reaction. The presence of optimal nitrogen content is crucial because excessive oxygen vacancies and Ti3+ may act as recombination centre. Thus, further studies were carried out by N-doped M-TiO2 (1 : 2).Figure 2
Comparison of the percentage degradation ofo-chlorophenol by N-doped mesoporous titania (1 : 1), N-doped mesoporous titania (1 : 2) and N-doped mesoporous titania (1 : 3).


## 2.1. Materials

All the reagents used for experimental studies were of analytical reagent grade. Methanol, acetic acid, ammonia, phenol,o-chlorophenol, sodium chloride, sodium carbonate, and sodium bicarbonate were obtained from Merck India ltd. Chitosan was procured from Chemchito India. Titanium isopropoxide was obtained from Acros India ltd. The stock solutions of phenol and o-chlorophenol were prepared in deionized water obtained from Millipore waters progard2 purification system. Plain solar intensity was measured in Watts per square meter using Lutron LX-102 light meter working on photocell principle.


## 2.2. Method

All the experiments were carried out in a cylindrical borosilicate glass reactor of 500 cm3capacity (Figure 1). The reactor was assembled with centrally mounted sparger surrounded by cooling coil. The same experimental setup was employed in the present investigation which was previously used by Kamble et al. [16]. The temperature of the reaction mixture was maintained near ambient by passing water through the cooling coil. 400 cm3 of solution (phenol/o-chlorophenol) was taken in the reactor and a known weight of the photocatalyst was added to the reactor. The solution was stirred in dark before exposing the reactor to concentrated sunlight from a compound parabolic reflector in order to find out the substrate adsorption effect. The concentration of phenol or o-chlorophenol in this filtered sample was treated as the zero time concentration (Ct=0) in each experiment before exposure to radiation. Air was sparged in the reactor through central sparger in order to keep the photocatalyst particles in uniform suspension. The position of the reflector was changed after a fixed interval of time with respect to the position of sunlight in order to maintain a constant band of light around the reactor. Samples were withdrawn at regular intervals of time for their analysis.Figure 1
Experimental setup of the solar reactor for photocatalytic degradation experiment.


## 2.3. Analysis

All the samples were withdrawn using a syringe, centrifuged, and then were immediately filtered through 0.45μ cellulose nitrate membranes. The phenol and o-chlorophenol concentration was measured on Knauer HPLC system equipped with Eurospher 100-10 C-18 column. The wavelength for detection of phenol and o-chlorophenol was 270 nm and 274 nm, respectively. The mobile phase used for analysis was methanol : water (50 : 50) v/v% and the flow rate was 1.2 cm3 min−1. The elution time for phenol and o-chlorophenol was 4.2 and 8.3 min, respectively. The solar experiments were carried out in the months of January 2008 to April 2008 in Nagpur, India (79°09′N, 21°09′E). During this period, the sky was brilliant blue, and the average solar intensity was approximately (±2%) constant at 950 Wm-2 as measured at the ground level. The experiments in artificial radiations were also carried out during the same period using Tungsten lamp (500 W).


## 2.4. Synthesis of N-Doped Mesoporous Titania

The synthesis of N-doped mesoporous titania has been previously reported by us and detailed elsewhere [17]. The ratio of chitosan and titania was changed to obtain mesoporous titania with different nitrogen content namely, N-doped M-TiO2 (1 : 1) and N-doped M-TiO2 (1 : 2) and N-doped M-TiO2 (1 : 3). The photocatalytic activity of all the three synthesized photocatalysts was evaluated for o-chlorophenol degradation. The % degradation of o-chlorophenol under solar radiation is as shown in Figure 2. It can be seen that highest percentage degradation was observed in case of N-doped M-TiO2 (1 : 2) followed by N-doped M-TiO2 (1 : 3) and N-doped M-TiO2 (1 : 1). The visible light activity of these photocatalysts is attributed to the nitrogen doping. The nitrogen partially replaces oxygen sites in TiO2. This replacement causes oxygen vacancies and amount of Ti3+ (TiO2 is reduced). These defects on the surface or in the bulk suppresses recombination reaction. The presence of optimal nitrogen content is crucial because excessive oxygen vacancies and Ti3+ may act as recombination centre. Thus, further studies were carried out by N-doped M-TiO2 (1 : 2).Figure 2
Comparison of the percentage degradation ofo-chlorophenol by N-doped mesoporous titania (1 : 1), N-doped mesoporous titania (1 : 2) and N-doped mesoporous titania (1 : 3).


## 3. Results and Discussion

### 3.1. Characterization of N-Doped Mesoporous Titania

The BET surface area of the synthesized photocatalyst was determined by specific surface area analyzer (ASAP 2000, micrometics) with nitrogen gas as the adsorbate. The surface area of N-doped mesoporous titania was found to be 132.36 m2/g which is significantly higher as compared to the conventional titania Degussa P-25 (55 m2/g). The pore size was determined by BJH method and the pore size was found to be 49.68 Å´. It can be clearly seen that the photocatalyst is mesoporous in nature and possesses high surface area.Powder XRD diffraction patterns of N-doped mesoporous titania were carried out on Rigaku Miniflex II desktop X-ray diffractometer with CuKα radiation, as shown in Figure 3. The scanning range of 2θ was set to between 20° and 80°. It can be seen from the X-ray diffraction patterns that all peaks can be indexed as the anatase phase (25.6°, 37.08°, 48°, 55.4°, and 63.32°) of titania. The low angle peaks (1°–3°) characteristic of ordered mesoporous structure were not observed [18].Figure 3
XRD spectra of N-doped mesoporous titania.The Fourier Transform Infrared (FTIR) analysis was carried on Bruker Vertex-70 by Diffuse Reflectance Accessory technique. The FTIR spectra of N-doped mesoporous titania are as shown in Figure4. The peaks corresponding to N–H stretching (3690.73 cm−1) and NH2 (1573.12 cm−1) indicate the presence of nitrogen in the synthesized photocatalyst. The peak at 2918.44 cm−1 is attributed to =C–H2 stretching vibrations, while the peak at 1676.52 cm−1 corresponds to C=C stretching vibrations.Figure 4
FTIR spectra  of N-doped mesoporous titania.Diffuse reflectance UV-Vis spectra of the synthesized photocatalyst was recorded using a Perkin Elmer spectrophotometer lambda 900 equipped with an integrating sphere. BaSO4 was used as a reference material. The spectrum is as shown in Figure 5. The absorption maxima of N-doped mesoporous titania was found to be 466.66 nm, which corresponds to the visible range of the spectrum indicating that N-doped mesoporous titania is active in visible light. The prominent red shift of the photocatalyst as compared to Degussa P-25 TiO2 can be attributed to the presence of nitrogen. The band gap energy was calculated from the absorption maxima by using following equation: (1)Eg(eV)=1240/λgnm
(see [19]), where λg is absorption maxima. The band gap energy was found to be 2.65 eV.Figure 5
UV-Vis spectra of N-doped mesoporous titania.Chemical composition analysis using energy dispersive X-ray (EDX) spectroscopy is as shown in Figure6. From the EDX spectra the nitrogen content of N-doped mesoporous titania was found to be 0.72 mass percent.Figure 6
EDX spectra of N-doped mesoporous titania.The morphology of the sample was investigated by scanning electron microscopy (SEM). Figure7 shows the SEM images of N-doped mesoporous titania with different magnifications. As it can be seen from the images, N-doped mesoporous titania particles exhibit an irregular morphology. The particle size for synthesized mesoporous titanai was measured by using CILAS-1180 instrument and it was observed to be 3.450 μm.SEM  of N-doped mesoporous titania.
(a)(b)(c)(d)The X-ray photoelectron spectroscopy measurements were carried out on VG Microtech ESCA 3000 instrument at a pressure of >1×10-9 Torr. The general scan, C1s, O1s, N1s, and Ti2p core level spectra were recorded with non-monochromatized Mg Kα radiation (photon energy 1253.6 eV) at a pass energy of 50 eV and an electron takeoff angle (angle between electron emission direction and surface plane) of 55°. The overall resolution was 0.2 eV for XPS measurements. The core level spectra were background-corrected using the Shirley algorithm, and chemically distinct species were resolved using nonlinear least-squares fitting procedure. Baseline correction and peak fitting for the sample was done using the software package XPS peak 41. The core level binding energies (BEs) were aligned with respect to the C1s binding energy of 285 eV.The doping of nitrogen into TiO2 lattice, and its state was substantiated and measured by XPS. Figure 8 illustrates the O1s, Ti2p, N1s, and C1s spectra of N-doped mesoporous titania (1 : 2). In N1s XPS spectra two signals at BE=394.2 eV and 400.9 eV can be observed. The peak at 394.2 eV belongs  to βN state, and it generally attributes to the presence of Ti–N bond whereby the N atoms replace the oxygen atoms in TiO2 lattice, while the second peak at 400.9 eV may be due to molecularly adsorbed nitrogen containing compound on the surface. The spectra obtained are quite consistent with those observed by Horikawa et al. [15]. The presence of titania ion in an octahedral environment is indicated by major peak which is centred at 462.3 eV in the Ti2p spectra. There is a single major peak that is observed at 534.5 eV in case of O1s, which corresponds to Ti–O bond.  In case of C spectra two major peaks are seen at 285.6 eV and 289.8 eV which are indicative of the presence of C–O and C=O bond. The characteristic peak at 281 eV which corresponds to Ti–C bond was not observed which suggests that carbon atoms do not replace the oxygen atoms in the TiO2 lattice.XPS  of N-doped mesoporous titania.
(a)(b)(c)(d)Comparison of N-Doped Mesoporous Titania with Degussa P-25 TiO2
The preliminary photodegradation experiments were carried out under identical set of conditions under solar radiation using commercially available TiO2 (Degussa P-25) and N-doped mesoporous titania. The photocatalytic degradation activities of this nondoped TiO2 (Degussa P-25) were then compared with those of N-doped mesoporous titania. It was observed that N-doped mesoporous titania has significantly higher activity for both phenol as well as o-chlorophenol as compared to Degussa P-25. The comparison of N-doped mesoporous titania with Degussa P-25 is as shown in Figure 9: It was observed that 28.59 mg of phenol degraded/g of TiO2 in case of N-doped mesoporous titania as compared to 24.75 mg phenol degraded/g of TiO2 for Degussa P-25 in solar radiation, while 40.71 mgo-chlorophenol degraded/g of TiO2 in case of N-doped mesoporous titania as compared to 24.75 mgo-chlorophenol degraded/g of TiO2 for Degussa P-25. The difference in the photodegradation activities in case of o-chlorophenol for TiO2 and N-doped TiO2 is significant as compared to phenol.(1)
In case of N-doped mesoporous titania, there is an  intense absorption in the visible light range and there is a red shift in the case of N-doped TiO2, resulting in the generation of more photogenerated electrons and holes participating in the photocatalytic reactions under visible light. In case of o-chlorophenol the aryl–Cl bond, is a weak bond and it is cleaved with relative ease which further facilitates the attack of ∙OH radical and hence o-chlorophenol is degraded to a greater extent. In case of phenol, as it is resonance stabilized, the photodegradation is to a lesser extent.(2)
Adsorption of the substrate on the photocatalyst has a major role in its photocatalytic degradation. According to the mechanism suggested, the attack of∙OH radicals takes place on the adsorbed substrate [20]. The equilibrium adsorption studies were carried out for both phenol and o-chlorophenol. In case of dark adsorption studies, 50 mL (phenol/o-chlorophenol) were mixed with both TiO2 and N-doped TiO2 and shaken for 24 h for equilibrium. The adsorption of o-chlorophenol was 36% on N-doped as compared to 15% for TiO2  resulting in more photodegradation.Figure 9
Comparison of N-doped mesoporous titania with Degussa P-25 for photodegradation  ofo-chlorophenol and phenol.


### 3.2. Effect of Various Parameters on Photocatalytic Degradation

#### 3.2.1. Effect of Catalyst Loading

The effect of catalyst loading on photocatalytic degradation of phenol ando-chlorophenol by N-doped mesoporous titania was studied. The catalyst loading was varied from 0.1% w/v to 0.3% w/v. The photocatalytic degradation of phenol and   o-chlorophenol is as shown in Figures 10(a) and 10(b). It can be seen that initially the photocatalytic degradation for both phenol and o-chlorophenol increases linearly as the catalyst loading is increased from 0.1% w/v  to 0.2% w/v but when the catalyst loading is increased further to 0.3% w/v, the rate of degradation decreases in case of both phenol and  o-chlorophenol. However, the increase in degradation rate is marginal for phenol as compared to o-chlorophenol. The decrease in degradation rate with increase in catalyst loading can be attributed to the increased opacity of the solution which hinders the light transmission through the solution. As a result of decreased effective light intensity, the photo generation of electrons and positive holes would be reduced and then the rate of photocatalytic degradation  is also reduced.Effect of catalyst loading on photocatalytic degradation: (a) phenol, (b)o-chlorophenol.
(a)(b)


#### 3.2.2. Effect of Initial Concentration

Effect of initial concentration on the rate of photocatalytic degradation was studied at different initial concentrations of phenol ando-chlorophenol and is as shown in Figures 11(a) and 11(b). It was found that with the increase in initial concentration of phenol and o-chlorophenol the rate of degradation decreases. This is because with the increase in concentration the amount of organic species to be degraded increases but the rate of generation of OH radical, photocatalyst loading, dissolved oxygen concentration, intensity of illumination and illumination time are constant during the photodegradation. Hence with increase in initial concentration the rate of photocatalytic degradation decreases.Effect of initial concentration on photocatalytic degradation: (a) phenol, (b)o-chlorophenol.
(a)(b)


#### 3.2.3. Effect of Initial pH

The pH of the solution is an important factor which affects the degradation rate. The effect of initial pH of solution on the photocatalytic degradation of phenol ando-chlorophenol by N-doped mesoporous titania was studied. The pH of initial solution was varied from 3 to 11. In acidic range the pH was varied using 0.1 M HCl while in alkaline range the pH was varied using 0.1 M NaOH. The rate of degradation for both phenol and   o-chlorophenol is as shown in Figures 12(a) and 12(b). It can be seen that in case of both phenol and o-chlorophenol, maximum degradation was found to be at pH 7. In both acidic as well as alkaline ranges the rate of degradation decreases. This can be explained from the fact that TiO2 is amphoteric in nature and the zero point charge of TiO2 is at pH-6. At acidic pH, the surface of TiO2 is positively charged while it is negatively charged at alkaline pH. In case of both phenol and o-chlorophenol the photocatalytic degradation decreases in acidic pH as the adsorption is less at acidic pH, while at alkaline pH, the negatively charged phenolate ions are repelled by the negatively charged surface of TiO2 and hence photocatalytic degradation decreases.Effect of initial pH on photocatalytic degradation (a) phenol (b)o-chlorophenol.
(a)(b)


#### 3.2.4. Effect of Coexisting Anions

The industrial effluent may contain several salts at different concentrations. These salts may exert negative or positive influence on the rate of photocatalytic degradation.  The effect of various ions like chloride, carbonate, and bicarbonate on the photocatalytic degradation of phenol ando-chlorophenol were studied by adding 0.1 M solution of their salts to 50 mgL−1 of phenol and o-chlorophenol. The effect of the presence of coexisting anions on photocatalytic degradation of phenol and o-chlorophenol is shown in Figures 13(a) and 13(b).  It can be clearly seen from these figures that the coions have a detrimental effect on the photocatalytic degradation. In case of phenol, the photocatalytic degradation in the absence of salts was 69.5%, while the photocatalytic degradation in case of sodium chloride, sodium carbonate, and sodium bicarbonate was 49.72%, 31.14%, and 35.98%, respectively. Similarly, in case of o-chlorophenol the photocatalytic degradation in the absence of salts was 98.62%, while the photocatalytic degradation in case of sodium chloride, sodium carbonate, and sodium bicarbonate was 87.09%, 79.34%, and 81.90%, respectively. It can be seen that the presence of chloride, carbonate, and bicarbonate has substantial detrimental effect on photocatalytic degradation of phenolics. The negative effect of these anions is attributed to following two reasons: (i) change in pH after addition of salts in aqueous solution of substrate (from acidic to alkaline).This contributes to inhibition of photocatalytic degradation of phenol and o-chlorophenol (Figures 12(a) and 12(b) also show the same trend.). (ii) Carbonate and bicarbonate anions basically act as hydroxyl radical scavengers, which affect photocatalytic degradation of phenol and o-chlorophenol. The decrease in the degradation rate in case of NaCl may be attributed to the poor adsorption.Effect of presence of coexisting ions on photocatalytic degradation (a) phenol (b)o-chlorophenol.
(a)(b)


### 3.3. Identification of Intermediates

The intermediates formed during the photocatalytic degradation of phenol ando-chlorophenol were identified by High Pressure Liquid Chromatograph. The intermediates formed in case of photocatalytic degradation of phenol were catechol (1 to 8 mg/L), hydroquinol (0.2 to 0.7 mg/L), and benzoquinone (0.5 to 2 mg/L), while in case of o-chlorophenol the major intermediates formed were chlorohydroquinone (concentration ranges from 0.2 to 0.5 mg/L), catechol concentration ranges from 1 to 16 mg/L),  and hydroxyhydroquinol concentration ranges from (0.2 to 0.7 mg/L).


### 3.4. Possible Reaction Mechanism

The reaction taking place at the surface of the photocatalyst is a redox reaction. The photocatalytic degradation of phenol ando-chlorophenol takes place via ∙OH radical attack. Several intermediates are formed during the process of degradation. Generally, after the attachment of two OH groups, the aromatic ring breaks. The subsequent products are rapidly oxidized to CO2 and H2O, as evidenced by the absence of aliphatic moieties [15]. In case of phenol, the ∙OH radical mainly attacks the orthoandparaposition of benzene ring and hence catechol and hydroquinol were the major intermediates formed. Generally, intermediates with 2 or at the most 3 OH groups were observed after which the cleavage of ring takes place.In case ofo-chlorophenol, the two main reaction pathways are orthoaddition resulting into formation of catechol and hydroxyhydroquinol and paraaddition which results in the formation of chlorohydroquinol as the major intermediates.


## 3.1. Characterization of N-Doped Mesoporous Titania

The BET surface area of the synthesized photocatalyst was determined by specific surface area analyzer (ASAP 2000, micrometics) with nitrogen gas as the adsorbate. The surface area of N-doped mesoporous titania was found to be 132.36 m2/g which is significantly higher as compared to the conventional titania Degussa P-25 (55 m2/g). The pore size was determined by BJH method and the pore size was found to be 49.68 Å´. It can be clearly seen that the photocatalyst is mesoporous in nature and possesses high surface area.Powder XRD diffraction patterns of N-doped mesoporous titania were carried out on Rigaku Miniflex II desktop X-ray diffractometer with CuKα radiation, as shown in Figure 3. The scanning range of 2θ was set to between 20° and 80°. It can be seen from the X-ray diffraction patterns that all peaks can be indexed as the anatase phase (25.6°, 37.08°, 48°, 55.4°, and 63.32°) of titania. The low angle peaks (1°–3°) characteristic of ordered mesoporous structure were not observed [18].Figure 3
XRD spectra of N-doped mesoporous titania.The Fourier Transform Infrared (FTIR) analysis was carried on Bruker Vertex-70 by Diffuse Reflectance Accessory technique. The FTIR spectra of N-doped mesoporous titania are as shown in Figure4. The peaks corresponding to N–H stretching (3690.73 cm−1) and NH2 (1573.12 cm−1) indicate the presence of nitrogen in the synthesized photocatalyst. The peak at 2918.44 cm−1 is attributed to =C–H2 stretching vibrations, while the peak at 1676.52 cm−1 corresponds to C=C stretching vibrations.Figure 4
FTIR spectra  of N-doped mesoporous titania.Diffuse reflectance UV-Vis spectra of the synthesized photocatalyst was recorded using a Perkin Elmer spectrophotometer lambda 900 equipped with an integrating sphere. BaSO4 was used as a reference material. The spectrum is as shown in Figure 5. The absorption maxima of N-doped mesoporous titania was found to be 466.66 nm, which corresponds to the visible range of the spectrum indicating that N-doped mesoporous titania is active in visible light. The prominent red shift of the photocatalyst as compared to Degussa P-25 TiO2 can be attributed to the presence of nitrogen. The band gap energy was calculated from the absorption maxima by using following equation: (1)Eg(eV)=1240/λgnm
(see [19]), where λg is absorption maxima. The band gap energy was found to be 2.65 eV.Figure 5
UV-Vis spectra of N-doped mesoporous titania.Chemical composition analysis using energy dispersive X-ray (EDX) spectroscopy is as shown in Figure6. From the EDX spectra the nitrogen content of N-doped mesoporous titania was found to be 0.72 mass percent.Figure 6
EDX spectra of N-doped mesoporous titania.The morphology of the sample was investigated by scanning electron microscopy (SEM). Figure7 shows the SEM images of N-doped mesoporous titania with different magnifications. As it can be seen from the images, N-doped mesoporous titania particles exhibit an irregular morphology. The particle size for synthesized mesoporous titanai was measured by using CILAS-1180 instrument and it was observed to be 3.450 μm.SEM  of N-doped mesoporous titania.
(a)(b)(c)(d)The X-ray photoelectron spectroscopy measurements were carried out on VG Microtech ESCA 3000 instrument at a pressure of >1×10-9 Torr. The general scan, C1s, O1s, N1s, and Ti2p core level spectra were recorded with non-monochromatized Mg Kα radiation (photon energy 1253.6 eV) at a pass energy of 50 eV and an electron takeoff angle (angle between electron emission direction and surface plane) of 55°. The overall resolution was 0.2 eV for XPS measurements. The core level spectra were background-corrected using the Shirley algorithm, and chemically distinct species were resolved using nonlinear least-squares fitting procedure. Baseline correction and peak fitting for the sample was done using the software package XPS peak 41. The core level binding energies (BEs) were aligned with respect to the C1s binding energy of 285 eV.The doping of nitrogen into TiO2 lattice, and its state was substantiated and measured by XPS. Figure 8 illustrates the O1s, Ti2p, N1s, and C1s spectra of N-doped mesoporous titania (1 : 2). In N1s XPS spectra two signals at BE=394.2 eV and 400.9 eV can be observed. The peak at 394.2 eV belongs  to βN state, and it generally attributes to the presence of Ti–N bond whereby the N atoms replace the oxygen atoms in TiO2 lattice, while the second peak at 400.9 eV may be due to molecularly adsorbed nitrogen containing compound on the surface. The spectra obtained are quite consistent with those observed by Horikawa et al. [15]. The presence of titania ion in an octahedral environment is indicated by major peak which is centred at 462.3 eV in the Ti2p spectra. There is a single major peak that is observed at 534.5 eV in case of O1s, which corresponds to Ti–O bond.  In case of C spectra two major peaks are seen at 285.6 eV and 289.8 eV which are indicative of the presence of C–O and C=O bond. The characteristic peak at 281 eV which corresponds to Ti–C bond was not observed which suggests that carbon atoms do not replace the oxygen atoms in the TiO2 lattice.XPS  of N-doped mesoporous titania.
(a)(b)(c)(d)Comparison of N-Doped Mesoporous Titania with Degussa P-25 TiO2
The preliminary photodegradation experiments were carried out under identical set of conditions under solar radiation using commercially available TiO2 (Degussa P-25) and N-doped mesoporous titania. The photocatalytic degradation activities of this nondoped TiO2 (Degussa P-25) were then compared with those of N-doped mesoporous titania. It was observed that N-doped mesoporous titania has significantly higher activity for both phenol as well as o-chlorophenol as compared to Degussa P-25. The comparison of N-doped mesoporous titania with Degussa P-25 is as shown in Figure 9: It was observed that 28.59 mg of phenol degraded/g of TiO2 in case of N-doped mesoporous titania as compared to 24.75 mg phenol degraded/g of TiO2 for Degussa P-25 in solar radiation, while 40.71 mgo-chlorophenol degraded/g of TiO2 in case of N-doped mesoporous titania as compared to 24.75 mgo-chlorophenol degraded/g of TiO2 for Degussa P-25. The difference in the photodegradation activities in case of o-chlorophenol for TiO2 and N-doped TiO2 is significant as compared to phenol.(1)
In case of N-doped mesoporous titania, there is an  intense absorption in the visible light range and there is a red shift in the case of N-doped TiO2, resulting in the generation of more photogenerated electrons and holes participating in the photocatalytic reactions under visible light. In case of o-chlorophenol the aryl–Cl bond, is a weak bond and it is cleaved with relative ease which further facilitates the attack of ∙OH radical and hence o-chlorophenol is degraded to a greater extent. In case of phenol, as it is resonance stabilized, the photodegradation is to a lesser extent.(2)
Adsorption of the substrate on the photocatalyst has a major role in its photocatalytic degradation. According to the mechanism suggested, the attack of∙OH radicals takes place on the adsorbed substrate [20]. The equilibrium adsorption studies were carried out for both phenol and o-chlorophenol. In case of dark adsorption studies, 50 mL (phenol/o-chlorophenol) were mixed with both TiO2 and N-doped TiO2 and shaken for 24 h for equilibrium. The adsorption of o-chlorophenol was 36% on N-doped as compared to 15% for TiO2  resulting in more photodegradation.Figure 9
Comparison of N-doped mesoporous titania with Degussa P-25 for photodegradation  ofo-chlorophenol and phenol.


## 3.2. Effect of Various Parameters on Photocatalytic Degradation

### 3.2.1. Effect of Catalyst Loading

The effect of catalyst loading on photocatalytic degradation of phenol ando-chlorophenol by N-doped mesoporous titania was studied. The catalyst loading was varied from 0.1% w/v to 0.3% w/v. The photocatalytic degradation of phenol and   o-chlorophenol is as shown in Figures 10(a) and 10(b). It can be seen that initially the photocatalytic degradation for both phenol and o-chlorophenol increases linearly as the catalyst loading is increased from 0.1% w/v  to 0.2% w/v but when the catalyst loading is increased further to 0.3% w/v, the rate of degradation decreases in case of both phenol and  o-chlorophenol. However, the increase in degradation rate is marginal for phenol as compared to o-chlorophenol. The decrease in degradation rate with increase in catalyst loading can be attributed to the increased opacity of the solution which hinders the light transmission through the solution. As a result of decreased effective light intensity, the photo generation of electrons and positive holes would be reduced and then the rate of photocatalytic degradation  is also reduced.Effect of catalyst loading on photocatalytic degradation: (a) phenol, (b)o-chlorophenol.
(a)(b)


### 3.2.2. Effect of Initial Concentration

Effect of initial concentration on the rate of photocatalytic degradation was studied at different initial concentrations of phenol ando-chlorophenol and is as shown in Figures 11(a) and 11(b). It was found that with the increase in initial concentration of phenol and o-chlorophenol the rate of degradation decreases. This is because with the increase in concentration the amount of organic species to be degraded increases but the rate of generation of OH radical, photocatalyst loading, dissolved oxygen concentration, intensity of illumination and illumination time are constant during the photodegradation. Hence with increase in initial concentration the rate of photocatalytic degradation decreases.Effect of initial concentration on photocatalytic degradation: (a) phenol, (b)o-chlorophenol.
(a)(b)


### 3.2.3. Effect of Initial pH

The pH of the solution is an important factor which affects the degradation rate. The effect of initial pH of solution on the photocatalytic degradation of phenol ando-chlorophenol by N-doped mesoporous titania was studied. The pH of initial solution was varied from 3 to 11. In acidic range the pH was varied using 0.1 M HCl while in alkaline range the pH was varied using 0.1 M NaOH. The rate of degradation for both phenol and   o-chlorophenol is as shown in Figures 12(a) and 12(b). It can be seen that in case of both phenol and o-chlorophenol, maximum degradation was found to be at pH 7. In both acidic as well as alkaline ranges the rate of degradation decreases. This can be explained from the fact that TiO2 is amphoteric in nature and the zero point charge of TiO2 is at pH-6. At acidic pH, the surface of TiO2 is positively charged while it is negatively charged at alkaline pH. In case of both phenol and o-chlorophenol the photocatalytic degradation decreases in acidic pH as the adsorption is less at acidic pH, while at alkaline pH, the negatively charged phenolate ions are repelled by the negatively charged surface of TiO2 and hence photocatalytic degradation decreases.Effect of initial pH on photocatalytic degradation (a) phenol (b)o-chlorophenol.
(a)(b)


### 3.2.4. Effect of Coexisting Anions

The industrial effluent may contain several salts at different concentrations. These salts may exert negative or positive influence on the rate of photocatalytic degradation.  The effect of various ions like chloride, carbonate, and bicarbonate on the photocatalytic degradation of phenol ando-chlorophenol were studied by adding 0.1 M solution of their salts to 50 mgL−1 of phenol and o-chlorophenol. The effect of the presence of coexisting anions on photocatalytic degradation of phenol and o-chlorophenol is shown in Figures 13(a) and 13(b).  It can be clearly seen from these figures that the coions have a detrimental effect on the photocatalytic degradation. In case of phenol, the photocatalytic degradation in the absence of salts was 69.5%, while the photocatalytic degradation in case of sodium chloride, sodium carbonate, and sodium bicarbonate was 49.72%, 31.14%, and 35.98%, respectively. Similarly, in case of o-chlorophenol the photocatalytic degradation in the absence of salts was 98.62%, while the photocatalytic degradation in case of sodium chloride, sodium carbonate, and sodium bicarbonate was 87.09%, 79.34%, and 81.90%, respectively. It can be seen that the presence of chloride, carbonate, and bicarbonate has substantial detrimental effect on photocatalytic degradation of phenolics. The negative effect of these anions is attributed to following two reasons: (i) change in pH after addition of salts in aqueous solution of substrate (from acidic to alkaline).This contributes to inhibition of photocatalytic degradation of phenol and o-chlorophenol (Figures 12(a) and 12(b) also show the same trend.). (ii) Carbonate and bicarbonate anions basically act as hydroxyl radical scavengers, which affect photocatalytic degradation of phenol and o-chlorophenol. The decrease in the degradation rate in case of NaCl may be attributed to the poor adsorption.Effect of presence of coexisting ions on photocatalytic degradation (a) phenol (b)o-chlorophenol.
(a)(b)


## 3.2.1. Effect of Catalyst Loading

The effect of catalyst loading on photocatalytic degradation of phenol ando-chlorophenol by N-doped mesoporous titania was studied. The catalyst loading was varied from 0.1% w/v to 0.3% w/v. The photocatalytic degradation of phenol and   o-chlorophenol is as shown in Figures 10(a) and 10(b). It can be seen that initially the photocatalytic degradation for both phenol and o-chlorophenol increases linearly as the catalyst loading is increased from 0.1% w/v  to 0.2% w/v but when the catalyst loading is increased further to 0.3% w/v, the rate of degradation decreases in case of both phenol and  o-chlorophenol. However, the increase in degradation rate is marginal for phenol as compared to o-chlorophenol. The decrease in degradation rate with increase in catalyst loading can be attributed to the increased opacity of the solution which hinders the light transmission through the solution. As a result of decreased effective light intensity, the photo generation of electrons and positive holes would be reduced and then the rate of photocatalytic degradation  is also reduced.Effect of catalyst loading on photocatalytic degradation: (a) phenol, (b)o-chlorophenol.
(a)(b)


## 3.2.2. Effect of Initial Concentration

Effect of initial concentration on the rate of photocatalytic degradation was studied at different initial concentrations of phenol ando-chlorophenol and is as shown in Figures 11(a) and 11(b). It was found that with the increase in initial concentration of phenol and o-chlorophenol the rate of degradation decreases. This is because with the increase in concentration the amount of organic species to be degraded increases but the rate of generation of OH radical, photocatalyst loading, dissolved oxygen concentration, intensity of illumination and illumination time are constant during the photodegradation. Hence with increase in initial concentration the rate of photocatalytic degradation decreases.Effect of initial concentration on photocatalytic degradation: (a) phenol, (b)o-chlorophenol.
(a)(b)


## 3.2.3. Effect of Initial pH

The pH of the solution is an important factor which affects the degradation rate. The effect of initial pH of solution on the photocatalytic degradation of phenol ando-chlorophenol by N-doped mesoporous titania was studied. The pH of initial solution was varied from 3 to 11. In acidic range the pH was varied using 0.1 M HCl while in alkaline range the pH was varied using 0.1 M NaOH. The rate of degradation for both phenol and   o-chlorophenol is as shown in Figures 12(a) and 12(b). It can be seen that in case of both phenol and o-chlorophenol, maximum degradation was found to be at pH 7. In both acidic as well as alkaline ranges the rate of degradation decreases. This can be explained from the fact that TiO2 is amphoteric in nature and the zero point charge of TiO2 is at pH-6. At acidic pH, the surface of TiO2 is positively charged while it is negatively charged at alkaline pH. In case of both phenol and o-chlorophenol the photocatalytic degradation decreases in acidic pH as the adsorption is less at acidic pH, while at alkaline pH, the negatively charged phenolate ions are repelled by the negatively charged surface of TiO2 and hence photocatalytic degradation decreases.Effect of initial pH on photocatalytic degradation (a) phenol (b)o-chlorophenol.
(a)(b)


## 3.2.4. Effect of Coexisting Anions

The industrial effluent may contain several salts at different concentrations. These salts may exert negative or positive influence on the rate of photocatalytic degradation.  The effect of various ions like chloride, carbonate, and bicarbonate on the photocatalytic degradation of phenol ando-chlorophenol were studied by adding 0.1 M solution of their salts to 50 mgL−1 of phenol and o-chlorophenol. The effect of the presence of coexisting anions on photocatalytic degradation of phenol and o-chlorophenol is shown in Figures 13(a) and 13(b).  It can be clearly seen from these figures that the coions have a detrimental effect on the photocatalytic degradation. In case of phenol, the photocatalytic degradation in the absence of salts was 69.5%, while the photocatalytic degradation in case of sodium chloride, sodium carbonate, and sodium bicarbonate was 49.72%, 31.14%, and 35.98%, respectively. Similarly, in case of o-chlorophenol the photocatalytic degradation in the absence of salts was 98.62%, while the photocatalytic degradation in case of sodium chloride, sodium carbonate, and sodium bicarbonate was 87.09%, 79.34%, and 81.90%, respectively. It can be seen that the presence of chloride, carbonate, and bicarbonate has substantial detrimental effect on photocatalytic degradation of phenolics. The negative effect of these anions is attributed to following two reasons: (i) change in pH after addition of salts in aqueous solution of substrate (from acidic to alkaline).This contributes to inhibition of photocatalytic degradation of phenol and o-chlorophenol (Figures 12(a) and 12(b) also show the same trend.). (ii) Carbonate and bicarbonate anions basically act as hydroxyl radical scavengers, which affect photocatalytic degradation of phenol and o-chlorophenol. The decrease in the degradation rate in case of NaCl may be attributed to the poor adsorption.Effect of presence of coexisting ions on photocatalytic degradation (a) phenol (b)o-chlorophenol.
(a)(b)


## 3.3. Identification of Intermediates

The intermediates formed during the photocatalytic degradation of phenol ando-chlorophenol were identified by High Pressure Liquid Chromatograph. The intermediates formed in case of photocatalytic degradation of phenol were catechol (1 to 8 mg/L), hydroquinol (0.2 to 0.7 mg/L), and benzoquinone (0.5 to 2 mg/L), while in case of o-chlorophenol the major intermediates formed were chlorohydroquinone (concentration ranges from 0.2 to 0.5 mg/L), catechol concentration ranges from 1 to 16 mg/L),  and hydroxyhydroquinol concentration ranges from (0.2 to 0.7 mg/L).


## 3.4. Possible Reaction Mechanism

The reaction taking place at the surface of the photocatalyst is a redox reaction. The photocatalytic degradation of phenol ando-chlorophenol takes place via ∙OH radical attack. Several intermediates are formed during the process of degradation. Generally, after the attachment of two OH groups, the aromatic ring breaks. The subsequent products are rapidly oxidized to CO2 and H2O, as evidenced by the absence of aliphatic moieties [15]. In case of phenol, the ∙OH radical mainly attacks the orthoandparaposition of benzene ring and hence catechol and hydroquinol were the major intermediates formed. Generally, intermediates with 2 or at the most 3 OH groups were observed after which the cleavage of ring takes place.In case ofo-chlorophenol, the two main reaction pathways are orthoaddition resulting into formation of catechol and hydroxyhydroquinol and paraaddition which results in the formation of chlorohydroquinol as the major intermediates.


## 4. Comparative Evaluation of Photodegradation of Phenolics

In general the photocatalytic degradation rate ofo-chlorophenol is higher as compared to phenol and may be attributed to the following.(1)
The adsorption ofo-chlorophenol is more as compared to phenol which in turn leads to high photodegradation rate.(2)
The aryl–Cl bond is a weak bond and it is cleaved with relative ease which further facilitates the attack of∙OH radical.


## 5. Mechanistic Aspects of the Photocatalytic Degradation of Phenolics

A possible mechanistic pathway illustrating the various sequence of events taking place at the semiconductor photocatalyst is as follows.(1)
Irradiation of the semiconductor photocatalyst leads to the generation of electron/hole pair which can either recombine or dissociate to give a conduction band electron and valence band hole.(2)
Oxygen that is sparged is omnipresent on the surface of the catalyst and acts as an electron acceptor whereas OH− groups and H2O molecules available as electron  donors interact with the photogenerated hole to yield highly reactive ∙OH radicals.(3)
The phenol molecule reacts with the highly reactive hydroxyl radical and according to the substitution rule the∙OH radical attacks the ortho and para position of the aromatic ring due to the existing OH group on it.(4)
The major intermediates in case of phenol are catechol and hydroquinol.(5)
After the addition of 2-3 OH groups on the aromatic ring, the cleavage of ring  takes place leading to further mineralization.(6)
In case ofo-chlorophenol, the ∙OH  radical attacks at orthoposition  leading to the formation of  hydroxyhydroquinol, and the cleavage of aryl–Cl  and further addition of ∙OH radical lead to the formation of chlorohydroquinol.(7)
Subsequent reactions further lead to mineralization of intermediates into carbondioxide and water.


## 6. Conclusions

In the present study, we have explored the photo-oxidation properties of  N-doped mesoporous titania in photodegradation of phenolics under visible light. It was observed that the catalyst shows significant activity in the solar radiation as compared to artificial light. It was seen that initial pH and   coexisting ions have a significant influence on the photocatalytic degradation rates. Maximum degradation was observed at neutral pH while the presence of coions has a detrimental effect on the degradation rates in case of both phenol ando-chlorophenol. The detailed studies pertaining to reuse and regeneration of the photocatalyst will be investigated in the latter part of this research work. Further improvement in photocatalytic activity of N-doped mesoporous titania is envisaged by codoping with nonmetal or metal ions.



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*Source: 780562-2011-06-09.xml*