# Mineralization of Azo Dye Using Combined Photo-Fenton and Photocatalytic Processes under Visible Light

Authors: Selma K. Kuriechen; Sepperumal Murugesan; Samuel Paul Raj
Journal: Journal of Catalysts
 (2013)

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## Abstract

Visible-light-assisted photodegradation of an azo dye, Reactive Red 180 (RR180), in the presence of nitrogen-doped TiO2 (N-TiO2) has been studied. The photodegradation of RR180 is evaluated through decolorization studies and total organic carbon analysis. The efficacy of hydrogen peroxide (H2O2), potassium peroxomonosulfate (oxone or PMS), and potassium peroxodisulfate (PDS) in improving the photodegradation of the dye in the N-TiO2-RR180 system is also examined. The effect of combining photo-Fenton-like reaction with N-TiO2-mediated photodegradation of RR180 under visible light has been investigated. The photoactivity of N-TiO2-RR180-Fe3+/Cu2+-oxidant systems is compared with the individual techniques of photocatalysis and photo-Fenton-like reactions. The coupled system possesses superior photomineralization ability towards the abatement of RR180.


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## Body

## 1. Introduction

Now a days, combining several oxidation systems for the degradation and mineralization of organic pollutants has become a common practice, for the reason that a single process usually cannot reach a desirable effectiveness in the degradation and mineralization of organic pollutants. Heterogeneous photocatalysis using titania photocatalyst has been established as a principal advanced oxidation process (AOP) for wastewater treatment. For a century, photo-Fenton reactions were also considered widely for the removal of organic pollutants [1–7]. The combination of heterogeneous photocatalysis with another AOP can be cost-effective as long as this combination produces a synergic effect. In the earlier efforts to increase the photodegradation efficiency through combined systems, photocatalysis coupled with ultrasonic treatment [8], integrating photocatalysis with membrane filtration [9], or combinations of photo-electro-Fenton [10], sono-Fenton [11], and electro-Fenton [12] processes were carried out, and better performances were observed. Not many attempts were made in pairing photocatalysis and photo-Fenton-like reactions for wastewater treatment. In general, the rate of photodegradation of pollutants is proportional to the efficiency of reactive radical formation. In photocatalysis- and photo-Fenton-coupled systems, two independent sources of hydroxyl radicals exist: (a) occurrence of hydroxyl radicals in photocatalytic reactions on titanium dioxide and (b) Fe(III) aqua complexes are independent and are more efficient sources of hydroxyl radicals through the photoredox reaction [13]. But the efficiency of photocatalytic process is limited by the recombination of photogenerated electrons and holes in the semiconductor phase. However, it can be suppressed by the addition of suitable scavengers of particular charge carriers.In the present investigation, effect of adding metal ions (Fe3+ or Cu2+) into the TiO2-mediated photodegradation of Reactive Red 180, an azo dye, under visible light is studied. The potential of coupled systems composed of nitrogen-doped titania or pure TiO2 (Degussa P25), metal ions (Fe3+ or Cu2+) and oxidants, namely, potassium peroxomonosulfate (PMS), potassium peroxodisulfate (PDS), and hydrogen peroxide (H2O2) towards the mineralization of RR180 under visible light is examined.


## 2. Experimental Details

### 2.1. Preparation and Characterization of Nitrogen-Doped Titania Catalyst

The nitrogen-doped TiO2 (N-TiO2) was synthesized through hydrolysis of TiCl4 followed by the addition of a solution of hydrazine hydrate [14]. Briefly, TiCl4 (0.05 mol) was added dropwise into 400 mL double distilled water while it was surrounded by an ice bath. After repeated stirring, 5 M solution of hydrazine hydrate was added dropwise so as to adjust the pH of the solution to 5.5. It was then kept overnight for aging. The resulting precipitate was centrifuged and filtered, washed with double distilled water for several times (to remove the chloride content), dried at 343 K, and then calcined at 673 K for 3 h to get the pale yellow-colored nitrogen-doped TiO2 powder.The crystal structure and phase purity of the prepared samples were analyzed by recording powder X-ray diffraction (XRD) patterns on a XPERT-PRO diffractometer with Cu Kα radiation (λ=1.5405Å) in the 2θ range of 10–80° at a scan rate of 0.02° s−1. A Shimadzu 2550 UV-visible spectrophotometer equipped with a diffuse reflectance accessory (ISR 2200) was used to obtain the diffuse reflectance spectra of the catalyst over a range of 300–600 nm.


### 2.2. Photocatalytic Degradation Studies

The photodegradation experiments were carried out in a photocatalytic chamber illuminated with three tungsten-halogen lamps (250 W, Philips, India;λ= 360–2000 nm). The UV radiation (λ<395nm) was filtered using a 2 Mil (50 μm thick) CU clear sun control film (Garware, India). A known amount of the photocatalyst, namely, TiO2 (Degussa P25) or nitrogen-doped TiO2  (N-TiO2), was added to a mixture containing appropriate concentrations of the dye (RR180, Figure 1) and ferric or cupric ion solutions in the photoreactor made of borosilicate glass and stirred continuously in dark for 45 min. Finally, oxidants (PMS, PDS, or H2O2) were introduced into the above suspension, just before irradiation. The dye concentration (measured from the absorbance of the dye at its λmax=542nm; εmax=19,466M-1cm-1) in the bulk solution at this condition (just before starting light irradiation) is used as the initial concentration (C0). During the irradiation, 5 mL aliquots were withdrawn at appropriate time intervals, and the photocatalyst was removed immediately by centrifugation followed by filtration through syringe filter (0.22 μm, Pall Corporation, India), and then the concentration of the dye was determined spectrophotometrically using a UV-vis spectrophotometer (Shimadzu 2550). The concentration obtained at a certain irradiation time (t) is denoted as Ct.  The total organic carbon (TOC) content of the reaction mixture was measured using a TOC analyzer (Shimadzu TOC-VCPH model).Figure 1
Structure of RR180.


## 2.1. Preparation and Characterization of Nitrogen-Doped Titania Catalyst

The nitrogen-doped TiO2 (N-TiO2) was synthesized through hydrolysis of TiCl4 followed by the addition of a solution of hydrazine hydrate [14]. Briefly, TiCl4 (0.05 mol) was added dropwise into 400 mL double distilled water while it was surrounded by an ice bath. After repeated stirring, 5 M solution of hydrazine hydrate was added dropwise so as to adjust the pH of the solution to 5.5. It was then kept overnight for aging. The resulting precipitate was centrifuged and filtered, washed with double distilled water for several times (to remove the chloride content), dried at 343 K, and then calcined at 673 K for 3 h to get the pale yellow-colored nitrogen-doped TiO2 powder.The crystal structure and phase purity of the prepared samples were analyzed by recording powder X-ray diffraction (XRD) patterns on a XPERT-PRO diffractometer with Cu Kα radiation (λ=1.5405Å) in the 2θ range of 10–80° at a scan rate of 0.02° s−1. A Shimadzu 2550 UV-visible spectrophotometer equipped with a diffuse reflectance accessory (ISR 2200) was used to obtain the diffuse reflectance spectra of the catalyst over a range of 300–600 nm.


## 2.2. Photocatalytic Degradation Studies

The photodegradation experiments were carried out in a photocatalytic chamber illuminated with three tungsten-halogen lamps (250 W, Philips, India;λ= 360–2000 nm). The UV radiation (λ<395nm) was filtered using a 2 Mil (50 μm thick) CU clear sun control film (Garware, India). A known amount of the photocatalyst, namely, TiO2 (Degussa P25) or nitrogen-doped TiO2  (N-TiO2), was added to a mixture containing appropriate concentrations of the dye (RR180, Figure 1) and ferric or cupric ion solutions in the photoreactor made of borosilicate glass and stirred continuously in dark for 45 min. Finally, oxidants (PMS, PDS, or H2O2) were introduced into the above suspension, just before irradiation. The dye concentration (measured from the absorbance of the dye at its λmax=542nm; εmax=19,466M-1cm-1) in the bulk solution at this condition (just before starting light irradiation) is used as the initial concentration (C0). During the irradiation, 5 mL aliquots were withdrawn at appropriate time intervals, and the photocatalyst was removed immediately by centrifugation followed by filtration through syringe filter (0.22 μm, Pall Corporation, India), and then the concentration of the dye was determined spectrophotometrically using a UV-vis spectrophotometer (Shimadzu 2550). The concentration obtained at a certain irradiation time (t) is denoted as Ct.  The total organic carbon (TOC) content of the reaction mixture was measured using a TOC analyzer (Shimadzu TOC-VCPH model).Figure 1
Structure of RR180.


## 3. Results and Discussion

### 3.1. Crystal Structure of N-TiO2

Figure2 illustrates the X-ray diffractogram of nitrogen-doped TiO2 calcined at 400°C for 3 h. All the observed peaks can be indexed to those corresponding to (101), (004), (200), (105), (213), (116), (220), and (301) planes of anatase phase of TiO2 (JCPDS file no. 21-1272), confirming the formation of particles with pure anatase phase. The average size of the anatase crystallites estimated using the Scherrer equation, D=0.9λ/βcosθ, (D—the grain diameter; λ—wavelength of  X-ray used;  β—full width at half maximum of the peak in radians; θ—the angle of diffraction in degree) is about 10 nm. It is to be noted that the doped samples exhibit the typical structure of anatase TiO2 crystal without any detectable dopant-related peaks. This may be due to the low concentration of the doped species, since limited amount of dopant may have moved either into the interstitial positions or into the substitutional sites of the TiO2 crystal structure [14, 15].Figure 2
XRD pattern of N-TiO2 calcined at 400°C for 3 h.


### 3.2. Optical Properties

Figure3 shows the diffuse reflectance spectrum of nitrogen-doped TiO2 particles together with that of Degussa P25 TiO2. Degussa P25 shows the fundamental absorbance stopping edge at 385 nm. A noticeable shift in the absorption edge towards the visible-light region (λ>400 nm) observed for the nitrogen-doped TiO2 catalyst may be due to the incorporation of nitrogen atoms into the lattice of TiO2.  The photoresponse of N-TiO2 in the visible light can be ascribed to the presence of oxygen vacancy states, due to the formation of Ti3+ species, between the valence and the conduction bands in the TiO2 band structure [16]. The vacant oxygen sites may have been substituted by nitrogen atoms and these nitrogen sites are responsible for the visible-light sensitivity. The pale yellow color of nitrogen-doped TiO2 also implied that the N-TiO2 absorbs some lower wavelength portion of the visible spectrum with low absorption intensity.Figure 3
UV-vis absorption spectra of TiO2 (P25) and N-TiO2 calcined at 400°C for 3 h.


### 3.3. Photodegradation of RR180

There was no conspicuous decolorization of RR180 when the experiments were carried out with (i) RR180 + light, (ii) RR180 + PDS + light, (iii) RR180 + PMS + light, and (iv) RR180 + H2O2  + light which indicated that neither photolysis nor simple oxidation by the strong oxidants occurred (Figure 4). But when similar experiments were performed in the presence of N-TiO2 (each of the above combinations with N-TiO2), a drastic increase in the degradation of RR180 (appreciable decrease in the concentration of dye with time) was observed (Figure 4). This reveals that the RR180 degradation takes place through photocatalytic process.Figure 4
Experimental data for the photodegradation of RR180 in the presence of oxidants.CN-TiO2=1.428 g L−1; CRR180=5×10-5 M; CPMS=CPDS=CH2O2=1 mM. CPMS, CPDS, and CH2O2 represent the amount of oxidants used.A set of experiments were carried out at natural pH of the solutions which were observed as 3.2 for TiO2-Fe3+ and 5.5 for TiO2-Cu2+ suspensions. It was noted that complete adsorption of dye molecules on the catalyst surface occurred in TiO2-Fe3+ system leading to catalyst poisoning since acidic pH is not favorable for TiO2. But, in TiO2-Cu2+ system, initial adsorption noticed was moderate. Likewise, when oxidants were introduced into the solution containing TiO2-Fe3+-dye, the initial adsorption noted was increased slightly and the reaction rate decreased. When oxidants were introduced in TiO2-Cu2+ system, better reaction rates were observed than photocatalysis as well as photo-Fenton-like processes. The pH of the colloidal solution where maximum reaction rate attained with TiO2 photocatalysis was 5.8. In case of Fe3+- and Cu2+-based studies (photo-Fenton-like reaction) with oxidants, highest activity was observed at pH 3.2 and 5.5, respectively. Hence, to improve the rate of reaction as well as to minimize the adsorption, the pH of the TiO2-Fe3+-oxidant system was altered to 5.6, and interestingly, it was found that the initial adsorption was reduced to minimum with simultaneous enhancement in the rate of reaction compared to individual photocatalysis as well as photo-Fenton-like reactions. Raising the pH above 6 in combined systems had shown a negative impact on the photodegradation of RR180. Therefore, further studies were carried out by maintaining pH at 5.6.Addition of Fe3+ or Cu2+ alone into titania resulted in detrimental effects on decolorization efficacy. It was observed that the decolorization of RR180 attained after 1 h visible-light irradiation was less than 15 percent in Titania-metal ions-based systems which are much less than those obtained with individual systems (Figure 5). Though coupled system with N-TiO2 was showing better performance than pure titania-based system, its photocatalytic activity seems to be less when compared to individual photocatalysis under similar experimental conditions. The strong negative effect on the photodegradation of dye observed upon addition of Fe3+ is due to the competitive adsorption of iron species with organic compounds on TiO2 surface. Thus, addition of Fe3+ and Cu2+ alone to TiO2 colloidal solution has shown decrement in the catalytic activity under visible light. It should be noticed that the combination of heterogeneous and homogeneous photocatalytic oxidation constitutes a very complex system in which several processes occur at the same time contributing to the overall reaction rate. The retardation of photodegradation rate on addition of Fe3+ or Cu2+ in TiO2-based systems can also be attributed to the quenching of photogenerated electrons by adsorbed metal ions which act as recombination centers that in turn reduce the generation of active radicals [17, 18].Figure 5
Decolorization of RR180 in the presence of  TiO2 or N-TiO2 and metal ions. [TiO2] = [N-TiO2] = 1.428 g L−1;  [Fe3+] = [Cu2+] = 0.2 mM;  [RR180] = 5  × 10−5 M.An increase in the pseudo first-order rate constants (compared to individual processes) was observed when TiO2-Fe3+ or TiO2-Cu2+ photocatalysis was performed in the presence of oxidants, namely, oxone, PDS, and H2O2 as shown in Table 1. The increment in the rate of reaction in Cu2+-based coupled system when compared to its performance in photo-Fenton-like reactions was much noticeable than the enhancement recorded with ferric ions. The enhanced degradation observed in the coupled systems (TiO2  + Fe3+  + Dye + oxidant or TiO2  + Cu2+  + Dye + oxidant) may be attributed to the enhanced generation of active radicals through decomposition of oxidants by both TiO2(e-) and metal ions. Therefore, both the processes are active enough to favor the degradation of azo dyes by promoting the generation of reactive radicals.Table 1
Pseudo first-order rate constant values and extent of mineralization obtained in     photocatalysis, photo-Fenton-like reactions, and combined systems (TiO2 or N-TiO2-Fe3+-oxidant and TiO2 or N-TiO2-Cu2+-oxidant).
Catalyst
Photodegradation rate constantk1×104 (s−1)
Extent of mineralization after 4 h (%)
TiO2
2.54
36
N-TiO2
5.85
51
TiO2+ PMS
23.7
75
N-TiO2+ PMS
27.1
78
Fe3+ + PMS
22.85
74
Cu2+ + PMS
16.95
70
TiO2+ Fe3+ + PMS
30.13
91
TiO2+ Cu2+ + PMS
26.52
89
N-TiO2+ Fe3+ + PMS
34.35
95
N-TiO2+ Cu2+ + PMS
28.82
90
TiO2+ PDS
4.10
65
N-TiO2+ PDS
7.05
68
Fe3+ + PDS
6.95
71
Cu2+ + PDS
6.67
58
TiO2+ Fe3+ + PDS
14.71
80
TiO2+ Cu2+ + PDS
22.10
86
N-TiO2+ Fe3+ + PDS
19.38
84
N-TiO2+ Cu2+ + PDS
26.45
87
TiO2+ H2O2
5.70
63
N-TiO2+ H2O2
9.25
67
Fe3+ + H2O2
11.1
72
Cu2+ + H2O2
6.18
62
TiO2+ Fe3+ + H2O2
21.45
77
TiO2+ Cu2+ + H2O2
17.30
76
N-TiO2+ Fe3+ + H2O2
23.06
86
N-TiO2+ Cu2+ + H2O2
20.85
76
[TiO2] = [N-TiO2] = 1.428 g L−1; [Fe3+] = [Cu2+] = 0.2 mM; [RR180] = 5×10-5 M; [Oxidants] = 2 mM.


#### 3.3.1. Effect of Oxidant Concentration

When the experiments were carried out at various oxidant concentrations (with constant dye, TiO2 or N-TiO2 catalyst, and Fe3+ or Cu2+ concentration), an initial raise in the first-order rate constants was noted till an optimum oxidant concentration and beyond this a slight decrement in rate constants were noted (Figures 6 and 7). Among the three oxidants chosen, PMS was showing better activity in all the coupled systems based on titania and N-TiO2 (Table 1). PDS performed well with cupric ion-based systems in the presence of titania and N-TiO2. In the coupled systems with H2O2, the enhancement in the reaction rate when compared to its activity in individual systems was rather low.Figure 6
Effect of PDS concentration on the pseudo first-order rate constants for the  photodegradation of RR180 in the coupled systems. [TiO2] = [N-TiO2] = 1.428 g L−1; [Fe3+] = [Cu2+] = 0.2 mM;  [RR180] = 5 × 10−5 M.Figure 7
Effect of H2O2 concentration on the pseudo first-order rate constants for the  photodegradation of RR180 in the coupled systems. [TiO2] = [N-TiO2] = 1.4280 g L−1;  [Fe3+] = [Cu2+] = 0.2 mM;  [RR180] = 5 × 10−5 M.The positive effect of coupling photo-Fenton-like reactions with semiconductor photocatalysis can be attributed to the increased production of active radicals through decomposition of oxidants by both heterogeneous and homogeneous catalysts. Introducing potassium peroxomonosulfate into the solution leads to the formation ofSO4•- and SO5•- radicals as well as hydroxyl radicals through radical chain reactions. Peroxomonosulfate often oxidizes faster than hydrogen peroxide and is slightly more powerful as an oxidant. PDS, a powerful oxidizing agent with a standard potential of E0=2.01V, can be decomposed to SO42- ion and SO4•- by the photogenerated e- present in TiO2 as well as by the metal ions. The generated sulfate radical anion, SO4•- (E0=2.6V), has the ability to attack organic compounds by abstraction of a hydrogen atom or addition on unsaturated molecules. The initial increase in the reaction efficiency that accompanies with the addition of H2O2 can be attributed to the increased formation of •OH radicals [19]. Higher oxidant concentration reduces the apparent rate constant due to the scavenging effect of hydroxyl radicals themselves as well as by the Fe2+ ions in the solution [20]. The reduction in the rate constants noted in the presence of oxone after optimum concentration may be due to the destruction of sulfate and hydroxyl radicals by the excess HSO5- ions [21, 22]. The excess radicals generated may undergo recombination or may get involved in the side reactions. At high persulfate concentration, the degradation rate decreases due to the adsorption of the excess sulfate ions (formed during the reaction) on the catalyst surface which reduces the activity of the catalyst [23].In the paired system with oxidants (N-TiO2-oxidant dye + Fe3+/Cu2+ oxidant dye coupled system), complete decolorization of RR180 was achieved within 30 min visible-light illumination whereas in the individual systems (photocatalysis experiments and photo-Fenton-like reactions carried out in the presence of oxidants) longer duration was required for attaining complete decolorization. It was also noted that cupric ions, which were having less photocatalytic activity in photo-Fenton-like reactions, show better activity in coupled system along with doped as well as undoped catalyst and oxidants for the chosen compound.


#### 3.3.2. TOC Analysis

The conversion of parent molecule into mineralized products (CO2  + H2O) was monitored through TOC analysis. While nearly 75% TOC reduction only was observed during the degradation of RR180 using individual photocatalysis (N-TiO2-PMS-RR180) or photo-Fenton-like (Fe3+-PMS-RR180) processes, the coupled system  (TiO2-Fe3+-Dye-PMS) exhibits 95% mineralization within 4 h continuous visible-light irradiation (Table 1). As observed in the decolorization studies, the coupled systems perform better than TiO2-mediated photocatalytic reactions and photo-Fenton-like reactions in the presence of oxidants. The requirement of prolonged irradiation for proper mineralization may be due to the formation of stable intermediate products which needs more time for their breakdown. The decolorization mechanism might proceed predominantly through the destruction of the azo group, by oxidation via reaction with positive holes and by reduction from conduction band electrons, while TOC was decreased only by the complete oxidation of the organic material into carbon dioxide [8].


## 3.1. Crystal Structure of N-TiO2

Figure2 illustrates the X-ray diffractogram of nitrogen-doped TiO2 calcined at 400°C for 3 h. All the observed peaks can be indexed to those corresponding to (101), (004), (200), (105), (213), (116), (220), and (301) planes of anatase phase of TiO2 (JCPDS file no. 21-1272), confirming the formation of particles with pure anatase phase. The average size of the anatase crystallites estimated using the Scherrer equation, D=0.9λ/βcosθ, (D—the grain diameter; λ—wavelength of  X-ray used;  β—full width at half maximum of the peak in radians; θ—the angle of diffraction in degree) is about 10 nm. It is to be noted that the doped samples exhibit the typical structure of anatase TiO2 crystal without any detectable dopant-related peaks. This may be due to the low concentration of the doped species, since limited amount of dopant may have moved either into the interstitial positions or into the substitutional sites of the TiO2 crystal structure [14, 15].Figure 2
XRD pattern of N-TiO2 calcined at 400°C for 3 h.


## 3.2. Optical Properties

Figure3 shows the diffuse reflectance spectrum of nitrogen-doped TiO2 particles together with that of Degussa P25 TiO2. Degussa P25 shows the fundamental absorbance stopping edge at 385 nm. A noticeable shift in the absorption edge towards the visible-light region (λ>400 nm) observed for the nitrogen-doped TiO2 catalyst may be due to the incorporation of nitrogen atoms into the lattice of TiO2.  The photoresponse of N-TiO2 in the visible light can be ascribed to the presence of oxygen vacancy states, due to the formation of Ti3+ species, between the valence and the conduction bands in the TiO2 band structure [16]. The vacant oxygen sites may have been substituted by nitrogen atoms and these nitrogen sites are responsible for the visible-light sensitivity. The pale yellow color of nitrogen-doped TiO2 also implied that the N-TiO2 absorbs some lower wavelength portion of the visible spectrum with low absorption intensity.Figure 3
UV-vis absorption spectra of TiO2 (P25) and N-TiO2 calcined at 400°C for 3 h.


## 3.3. Photodegradation of RR180

There was no conspicuous decolorization of RR180 when the experiments were carried out with (i) RR180 + light, (ii) RR180 + PDS + light, (iii) RR180 + PMS + light, and (iv) RR180 + H2O2  + light which indicated that neither photolysis nor simple oxidation by the strong oxidants occurred (Figure 4). But when similar experiments were performed in the presence of N-TiO2 (each of the above combinations with N-TiO2), a drastic increase in the degradation of RR180 (appreciable decrease in the concentration of dye with time) was observed (Figure 4). This reveals that the RR180 degradation takes place through photocatalytic process.Figure 4
Experimental data for the photodegradation of RR180 in the presence of oxidants.CN-TiO2=1.428 g L−1; CRR180=5×10-5 M; CPMS=CPDS=CH2O2=1 mM. CPMS, CPDS, and CH2O2 represent the amount of oxidants used.A set of experiments were carried out at natural pH of the solutions which were observed as 3.2 for TiO2-Fe3+ and 5.5 for TiO2-Cu2+ suspensions. It was noted that complete adsorption of dye molecules on the catalyst surface occurred in TiO2-Fe3+ system leading to catalyst poisoning since acidic pH is not favorable for TiO2. But, in TiO2-Cu2+ system, initial adsorption noticed was moderate. Likewise, when oxidants were introduced into the solution containing TiO2-Fe3+-dye, the initial adsorption noted was increased slightly and the reaction rate decreased. When oxidants were introduced in TiO2-Cu2+ system, better reaction rates were observed than photocatalysis as well as photo-Fenton-like processes. The pH of the colloidal solution where maximum reaction rate attained with TiO2 photocatalysis was 5.8. In case of Fe3+- and Cu2+-based studies (photo-Fenton-like reaction) with oxidants, highest activity was observed at pH 3.2 and 5.5, respectively. Hence, to improve the rate of reaction as well as to minimize the adsorption, the pH of the TiO2-Fe3+-oxidant system was altered to 5.6, and interestingly, it was found that the initial adsorption was reduced to minimum with simultaneous enhancement in the rate of reaction compared to individual photocatalysis as well as photo-Fenton-like reactions. Raising the pH above 6 in combined systems had shown a negative impact on the photodegradation of RR180. Therefore, further studies were carried out by maintaining pH at 5.6.Addition of Fe3+ or Cu2+ alone into titania resulted in detrimental effects on decolorization efficacy. It was observed that the decolorization of RR180 attained after 1 h visible-light irradiation was less than 15 percent in Titania-metal ions-based systems which are much less than those obtained with individual systems (Figure 5). Though coupled system with N-TiO2 was showing better performance than pure titania-based system, its photocatalytic activity seems to be less when compared to individual photocatalysis under similar experimental conditions. The strong negative effect on the photodegradation of dye observed upon addition of Fe3+ is due to the competitive adsorption of iron species with organic compounds on TiO2 surface. Thus, addition of Fe3+ and Cu2+ alone to TiO2 colloidal solution has shown decrement in the catalytic activity under visible light. It should be noticed that the combination of heterogeneous and homogeneous photocatalytic oxidation constitutes a very complex system in which several processes occur at the same time contributing to the overall reaction rate. The retardation of photodegradation rate on addition of Fe3+ or Cu2+ in TiO2-based systems can also be attributed to the quenching of photogenerated electrons by adsorbed metal ions which act as recombination centers that in turn reduce the generation of active radicals [17, 18].Figure 5
Decolorization of RR180 in the presence of  TiO2 or N-TiO2 and metal ions. [TiO2] = [N-TiO2] = 1.428 g L−1;  [Fe3+] = [Cu2+] = 0.2 mM;  [RR180] = 5  × 10−5 M.An increase in the pseudo first-order rate constants (compared to individual processes) was observed when TiO2-Fe3+ or TiO2-Cu2+ photocatalysis was performed in the presence of oxidants, namely, oxone, PDS, and H2O2 as shown in Table 1. The increment in the rate of reaction in Cu2+-based coupled system when compared to its performance in photo-Fenton-like reactions was much noticeable than the enhancement recorded with ferric ions. The enhanced degradation observed in the coupled systems (TiO2  + Fe3+  + Dye + oxidant or TiO2  + Cu2+  + Dye + oxidant) may be attributed to the enhanced generation of active radicals through decomposition of oxidants by both TiO2(e-) and metal ions. Therefore, both the processes are active enough to favor the degradation of azo dyes by promoting the generation of reactive radicals.Table 1
Pseudo first-order rate constant values and extent of mineralization obtained in     photocatalysis, photo-Fenton-like reactions, and combined systems (TiO2 or N-TiO2-Fe3+-oxidant and TiO2 or N-TiO2-Cu2+-oxidant).
Catalyst
Photodegradation rate constantk1×104 (s−1)
Extent of mineralization after 4 h (%)
TiO2
2.54
36
N-TiO2
5.85
51
TiO2+ PMS
23.7
75
N-TiO2+ PMS
27.1
78
Fe3+ + PMS
22.85
74
Cu2+ + PMS
16.95
70
TiO2+ Fe3+ + PMS
30.13
91
TiO2+ Cu2+ + PMS
26.52
89
N-TiO2+ Fe3+ + PMS
34.35
95
N-TiO2+ Cu2+ + PMS
28.82
90
TiO2+ PDS
4.10
65
N-TiO2+ PDS
7.05
68
Fe3+ + PDS
6.95
71
Cu2+ + PDS
6.67
58
TiO2+ Fe3+ + PDS
14.71
80
TiO2+ Cu2+ + PDS
22.10
86
N-TiO2+ Fe3+ + PDS
19.38
84
N-TiO2+ Cu2+ + PDS
26.45
87
TiO2+ H2O2
5.70
63
N-TiO2+ H2O2
9.25
67
Fe3+ + H2O2
11.1
72
Cu2+ + H2O2
6.18
62
TiO2+ Fe3+ + H2O2
21.45
77
TiO2+ Cu2+ + H2O2
17.30
76
N-TiO2+ Fe3+ + H2O2
23.06
86
N-TiO2+ Cu2+ + H2O2
20.85
76
[TiO2] = [N-TiO2] = 1.428 g L−1; [Fe3+] = [Cu2+] = 0.2 mM; [RR180] = 5×10-5 M; [Oxidants] = 2 mM.


### 3.3.1. Effect of Oxidant Concentration

When the experiments were carried out at various oxidant concentrations (with constant dye, TiO2 or N-TiO2 catalyst, and Fe3+ or Cu2+ concentration), an initial raise in the first-order rate constants was noted till an optimum oxidant concentration and beyond this a slight decrement in rate constants were noted (Figures 6 and 7). Among the three oxidants chosen, PMS was showing better activity in all the coupled systems based on titania and N-TiO2 (Table 1). PDS performed well with cupric ion-based systems in the presence of titania and N-TiO2. In the coupled systems with H2O2, the enhancement in the reaction rate when compared to its activity in individual systems was rather low.Figure 6
Effect of PDS concentration on the pseudo first-order rate constants for the  photodegradation of RR180 in the coupled systems. [TiO2] = [N-TiO2] = 1.428 g L−1; [Fe3+] = [Cu2+] = 0.2 mM;  [RR180] = 5 × 10−5 M.Figure 7
Effect of H2O2 concentration on the pseudo first-order rate constants for the  photodegradation of RR180 in the coupled systems. [TiO2] = [N-TiO2] = 1.4280 g L−1;  [Fe3+] = [Cu2+] = 0.2 mM;  [RR180] = 5 × 10−5 M.The positive effect of coupling photo-Fenton-like reactions with semiconductor photocatalysis can be attributed to the increased production of active radicals through decomposition of oxidants by both heterogeneous and homogeneous catalysts. Introducing potassium peroxomonosulfate into the solution leads to the formation ofSO4•- and SO5•- radicals as well as hydroxyl radicals through radical chain reactions. Peroxomonosulfate often oxidizes faster than hydrogen peroxide and is slightly more powerful as an oxidant. PDS, a powerful oxidizing agent with a standard potential of E0=2.01V, can be decomposed to SO42- ion and SO4•- by the photogenerated e- present in TiO2 as well as by the metal ions. The generated sulfate radical anion, SO4•- (E0=2.6V), has the ability to attack organic compounds by abstraction of a hydrogen atom or addition on unsaturated molecules. The initial increase in the reaction efficiency that accompanies with the addition of H2O2 can be attributed to the increased formation of •OH radicals [19]. Higher oxidant concentration reduces the apparent rate constant due to the scavenging effect of hydroxyl radicals themselves as well as by the Fe2+ ions in the solution [20]. The reduction in the rate constants noted in the presence of oxone after optimum concentration may be due to the destruction of sulfate and hydroxyl radicals by the excess HSO5- ions [21, 22]. The excess radicals generated may undergo recombination or may get involved in the side reactions. At high persulfate concentration, the degradation rate decreases due to the adsorption of the excess sulfate ions (formed during the reaction) on the catalyst surface which reduces the activity of the catalyst [23].In the paired system with oxidants (N-TiO2-oxidant dye + Fe3+/Cu2+ oxidant dye coupled system), complete decolorization of RR180 was achieved within 30 min visible-light illumination whereas in the individual systems (photocatalysis experiments and photo-Fenton-like reactions carried out in the presence of oxidants) longer duration was required for attaining complete decolorization. It was also noted that cupric ions, which were having less photocatalytic activity in photo-Fenton-like reactions, show better activity in coupled system along with doped as well as undoped catalyst and oxidants for the chosen compound.


### 3.3.2. TOC Analysis

The conversion of parent molecule into mineralized products (CO2  + H2O) was monitored through TOC analysis. While nearly 75% TOC reduction only was observed during the degradation of RR180 using individual photocatalysis (N-TiO2-PMS-RR180) or photo-Fenton-like (Fe3+-PMS-RR180) processes, the coupled system  (TiO2-Fe3+-Dye-PMS) exhibits 95% mineralization within 4 h continuous visible-light irradiation (Table 1). As observed in the decolorization studies, the coupled systems perform better than TiO2-mediated photocatalytic reactions and photo-Fenton-like reactions in the presence of oxidants. The requirement of prolonged irradiation for proper mineralization may be due to the formation of stable intermediate products which needs more time for their breakdown. The decolorization mechanism might proceed predominantly through the destruction of the azo group, by oxidation via reaction with positive holes and by reduction from conduction band electrons, while TOC was decreased only by the complete oxidation of the organic material into carbon dioxide [8].


## 3.3.1. Effect of Oxidant Concentration

When the experiments were carried out at various oxidant concentrations (with constant dye, TiO2 or N-TiO2 catalyst, and Fe3+ or Cu2+ concentration), an initial raise in the first-order rate constants was noted till an optimum oxidant concentration and beyond this a slight decrement in rate constants were noted (Figures 6 and 7). Among the three oxidants chosen, PMS was showing better activity in all the coupled systems based on titania and N-TiO2 (Table 1). PDS performed well with cupric ion-based systems in the presence of titania and N-TiO2. In the coupled systems with H2O2, the enhancement in the reaction rate when compared to its activity in individual systems was rather low.Figure 6
Effect of PDS concentration on the pseudo first-order rate constants for the  photodegradation of RR180 in the coupled systems. [TiO2] = [N-TiO2] = 1.428 g L−1; [Fe3+] = [Cu2+] = 0.2 mM;  [RR180] = 5 × 10−5 M.Figure 7
Effect of H2O2 concentration on the pseudo first-order rate constants for the  photodegradation of RR180 in the coupled systems. [TiO2] = [N-TiO2] = 1.4280 g L−1;  [Fe3+] = [Cu2+] = 0.2 mM;  [RR180] = 5 × 10−5 M.The positive effect of coupling photo-Fenton-like reactions with semiconductor photocatalysis can be attributed to the increased production of active radicals through decomposition of oxidants by both heterogeneous and homogeneous catalysts. Introducing potassium peroxomonosulfate into the solution leads to the formation ofSO4•- and SO5•- radicals as well as hydroxyl radicals through radical chain reactions. Peroxomonosulfate often oxidizes faster than hydrogen peroxide and is slightly more powerful as an oxidant. PDS, a powerful oxidizing agent with a standard potential of E0=2.01V, can be decomposed to SO42- ion and SO4•- by the photogenerated e- present in TiO2 as well as by the metal ions. The generated sulfate radical anion, SO4•- (E0=2.6V), has the ability to attack organic compounds by abstraction of a hydrogen atom or addition on unsaturated molecules. The initial increase in the reaction efficiency that accompanies with the addition of H2O2 can be attributed to the increased formation of •OH radicals [19]. Higher oxidant concentration reduces the apparent rate constant due to the scavenging effect of hydroxyl radicals themselves as well as by the Fe2+ ions in the solution [20]. The reduction in the rate constants noted in the presence of oxone after optimum concentration may be due to the destruction of sulfate and hydroxyl radicals by the excess HSO5- ions [21, 22]. The excess radicals generated may undergo recombination or may get involved in the side reactions. At high persulfate concentration, the degradation rate decreases due to the adsorption of the excess sulfate ions (formed during the reaction) on the catalyst surface which reduces the activity of the catalyst [23].In the paired system with oxidants (N-TiO2-oxidant dye + Fe3+/Cu2+ oxidant dye coupled system), complete decolorization of RR180 was achieved within 30 min visible-light illumination whereas in the individual systems (photocatalysis experiments and photo-Fenton-like reactions carried out in the presence of oxidants) longer duration was required for attaining complete decolorization. It was also noted that cupric ions, which were having less photocatalytic activity in photo-Fenton-like reactions, show better activity in coupled system along with doped as well as undoped catalyst and oxidants for the chosen compound.


## 3.3.2. TOC Analysis

The conversion of parent molecule into mineralized products (CO2  + H2O) was monitored through TOC analysis. While nearly 75% TOC reduction only was observed during the degradation of RR180 using individual photocatalysis (N-TiO2-PMS-RR180) or photo-Fenton-like (Fe3+-PMS-RR180) processes, the coupled system  (TiO2-Fe3+-Dye-PMS) exhibits 95% mineralization within 4 h continuous visible-light irradiation (Table 1). As observed in the decolorization studies, the coupled systems perform better than TiO2-mediated photocatalytic reactions and photo-Fenton-like reactions in the presence of oxidants. The requirement of prolonged irradiation for proper mineralization may be due to the formation of stable intermediate products which needs more time for their breakdown. The decolorization mechanism might proceed predominantly through the destruction of the azo group, by oxidation via reaction with positive holes and by reduction from conduction band electrons, while TOC was decreased only by the complete oxidation of the organic material into carbon dioxide [8].


## 4. Conclusions

Combination of titania-based photocatalysis and Fe3+- or Cu2+-oxidant (photo-Fenton-like) systems produces a synergic effect that leads to an increase in the rate of photodegradation of RR180. In the coupled system, complete decolorization of RR180 was achieved within 30 min visible-light illumination. A two fold increase in the TOC reduction was achieved in the coupled systems than TiO2-based photocatalysis of RR180. Enhanced degradation of RR180 may be due to the interaction of oxidants (PMS, PDS, or H2O2) with both excited titania and metal ions to produce more radicals. The degradation is favored at a pH of 5.6 by TiO2-Fe3+-oxidant and TiO2-Cu2+-oxidant systems.



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*Source: 104019-2013-04-04.xml*