# Titanium Dioxide Supported on Different Porous Materials as Photocatalyst for the Degradation of Methyl Green in Wastewaters

Authors: Haithem Bel Hadjltaief; Abdessalem Omri; Mourad Ben Zina; Patrick Da Costa; Maria Elena Galvez
Journal: Advances in Materials Science and Engineering
 (2015)

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## Abstract

TiO2 nanoparticles were immobilized on two porous materials used as catalyst supports, namely, activated carbon (AC) and natural clay (NC), through an impregnation process using TiO2 (P25) as precursor. The so-prepared composite materials were characterized by X-ray diffraction (XRD), scanning electron microscopy (SEM), transition electron microscopy (TEM), and nitrogen physisorption, that is, Brunauer-Emmett-Teller (BET) surface area determination. SEM and TEM observation evidenced that TiO2 was deposited on AC and NC surface. XRD results confirmed that TiO2 existed in a mixture of anatase and rutile phases. The specific surface area of photocatalysts decreased drastically in comparison with the original materials. The photocatalytic activity of these materials was assayed in the oxidation of Methyl Green (MG) dye in aqueous medium under UV irradiation. TiO2/AC exhibited higher photocatalytic oxidation activity than TiO2 at neutral pH. Total mineralization of MG was confirmed by means of COD analysis, pointing to these materials as an efficient, cost-effective, and environment friendly alternative for water treatment.


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## Body

## 1. Introduction

Water pollution has become a subject of global environmental concern in recent years. Dyes from different industries such as dye synthesis, paper, printing, electroplating, food, and cosmetics are one of the major sources of water pollution [1]. Various types of dyes exist such as azo, anthraquinone, reactive, acidic, basic, neutral, disperse, and direct dyes. Azo and anthraquinone dyes are however the most commonly used ones [1–3]. Methyl Green (MG) is a basic triphenylmethane and a dicationic type dye usually used for staining of solutions in medicine and biology [4]. It is also used as a photochromophore to sensitize gelatinous film [5].Advanced oxidation processes (AOPs) involve the generation of highly reactive radical species by several ways [6–9]. These techniques are based on the production of reactive species such as hydroxyl radicals (HO•), which are powerful oxidizing agents and are capable of attacking a wide variety of organic molecules. AOPs photocatalysis systems include combination of semiconductors and light and semiconductor and oxidants. Heterogeneous photocatalysis is the most promising method of AOPs for toxic components in wastewater, such as phenols, herbicides, pesticides, dyes, and surfactants [7, 8]. Titanium dioxide (TiO2) is the most widely used photocatalyst owing to its efficiency, low cost, and chemical stability [6, 10]. TiO2 powders such as Degussa P25 have been commercially available for several years. Nevertheless, after degradation tests, photocatalysts in the powder form must be removed from the suspension and this step is an important factor that may cause important problems in industrial applications [6, 11]. To solve these problems, photocatalysts (e.g., TiO2) have been immobilized on various supports such as silica [12], silicon carbide [13], perlite [14], fly ash [15], zeolites [16], clay [17], and activated carbon [10, 18]. Also, several preparation methods for TiO2 on these supports, such as hydrothermal method, sol-gel method, boil deposition, dip coating, metal organic chemical vapor deposition (MOCVD), and impregnation, have been reported [19, 20].The advantages of using TiO2 supported photocatalysts were summarized as follows: (i) The support adsorbs a high amount of pollutants around the loaded TiO2. Then, the rate of photooxidation is improved [20]. (ii) The adsorbed pollutants (organic substances) are oxidized at the surface of the photocatalyst, and the resulting intermediates are also adsorbed and then further oxidized. Toxic intermediates, if formed, are not released in the air atmosphere and/or in solution phase, thus preventing secondary pollution. (iii) Since the pollutants are finally oxidized into CO2, the lifetime of the hybrid photocatalysts is long [15].The purpose of the present work is to load TiO2 on the surface of both porous materials, that is, activated carbon (AC) and natural clay (NC), in order to prepare active and stable catalysts for the photocatalytic degradation of Methyl Green dye in wastewaters.


## 2. Experimental

### 2.1. Materials

The clay used in this study was sampled in Jebel Tejera-Esghira deposits located in the southeast of Tunisia from the area of Medenine. The natural clay was first purified by dispersion in water, decantation, and extraction of the fraction with a particle size smaller than 2μm. Then, the natural clay was modified by sodium exchange described in our previous work [3, 21]. Activated carbon (AC) was prepared from the physical activation ofLawsonia inermis wood, which was obtained from the field in Gabès (Tunisia). The preparation process has been described in detail elsewhere [22]. Commercial TiO2 (Degussa P25, Degussa Chemical) was used as titanium source for the preparation of photocatalysts. Methyl Green (MG, dicationic dye, chemical formula C27H35Cl2N3·ZnCl2, M
W
=
608.8 g/mol, Sigma-Aldrich) was used to evaluate the photocatalytic efficiency of synthesized photocatalysts.


### 2.2. Synthesis of Photocatalytic Materials

TiO2/AC and TiO2/NC photocatalytic materials were prepared through an impregnation method. First, different weights of AC or NC were added under stirring to a TiO2 (P25) aqueous suspension (mixing 30 mg of TiO2 (P25) and 100 mL of distilled water). After the impregnation process, the samples obtained were washed by double-distilled water, filtered, and then dried at 110°C for 24 h. Finally, the dried material was calcined to 500°C for 3 h in a nitrogen-purged reactor tube with a heating rate of 5°C/min. The steps of the photocatalysts preparation are presented in Figure 1.Figure 1
Scheme of the preparation method of photocatalysts by the impregnation method.


### 2.3. Characterization of Photocatalysts

Several techniques were employed for the characterization of the samples. Samples were also examined under a scanning electron microscope (SEM, Hitachi SU-70). The structural feature of these samples was observed at the accelerated voltage of 1.0 kV. High resolution transmission electron microscopy (HRTEM) images were thus acquired (JEOL JEM 2011) equipped with LaB6 filament and operating at 200 kV. The images were collected with a4008
×
2672 pixels’ CCD camera (Gatan Orius SC1000) coupled with the Digital Micrograph software. Chemical analyses were obtained by an EDX microanalyzer (PGT IMIX PC) mounted on the microscope. The catalysts were dispersed in ethanol and sonicated. A drop of the dispersion was deposited on a carbon-coated copper grid for the TEM observations.Nitrogen adsorption-desorption isotherms were measured at −196°C (Fisons Sorptomatic 1990) after outgassing (10−5 Pa) for 24 h at ambient temperature. The specific surface area, S
B
E
T, was determined according to the Brunauer-Emmett-Teller (BET) method at the relative pressure, p
/
p
0, in the range of 0.05–0.1.The porosity of the photocatalysts was measured by pycnometry. In order to determine the real density (ρ
s), water was chosen since it can penetrate pores [23], whereas, for the apparent density (ρ
p), mercury was chosen since it does not penetrate into the porous network. The porosity (P) can be calculated by the following equation:(1)
P
=
ρ
s
-
ρ
p
ρ
s
×
100
%
.For the crystal phase composition and the crystallite size of the photocatalysts, X-ray diffraction measurements were carried out at room temperature using an X-ray diffractometer (Philips PW 1710 diffractometer) (Cu Kα, 40 kV/40 mA, scanning rate of 2
Θ per min). The crystallite size was calculated by X-ray line-broadening analysis using Scherrer equation [17, 19].


### 2.4. Photoreactor and Photodegradation Procedure

Photocatalytic oxidation experiments were performed in an open Pyrex-glass cell with 250 mL capacity (of 5 cm inside diameter and 11 cm height). The design description of photocatalytic reactor was reported in our earlier study [3]. Irradiation was carried out using an UV-lamp (Black-Ray B 100 W UV-lamp, V-100AP series) with a wavelength of 365 nm.A suspension was prepared by adding appropriate amount of support TiO2/AC or TiO2/NC to 200 mL of MG aqueous solution (75 mg/L) at pH 7. The pH of suspension was measured using PH-035 digital pH meter from Changlilai Technology Co., Ltd. (Shenzhen, China), by adding H2SO4 (0.1 mol/L) or NaOH (0.1 mol/L). All the experiments were performed at an ambient temperature (25 ± 1°C) and atmospheric pressure. During the experiment, air was continuously bubbled into the catalyst suspension. Prior to irradiation, the suspension was magnetically stirred in the dark for at least 60 min to ensure the establishment of an adsorption/desorption equilibrium. The experimental work of this study involved several parameters such as the pH, catalyst loading, initial dye concentration, and H2O2 concentration. Firstly, for examining the effect of pH, the pH of MG solution was adjusted using 0.1 HCl and 0.1 NaOH aqueous solutions to be 3 to 11, while fixing the MG concentration at 75 mg/L and the dosages at 1 g/L of the photocatalysts. Catalyst concentration was chosen from 0.25 to 1.75 g/L, for 75 mg/L of MG solution, at p
H
=
7. The influence of the MG dye concentration was also evaluated by varying its concentration range from 25 mg/L to 150 mg/L, at a fixed pH of 7 in the presence of 0.75 g/L. Finally, the influence of the H2O2 amount added to the MG solution was evaluated by both dosages 8 mL and 16 mL (1000 mg L−1 of H2O2 solution, prepared from H2O2 (30%) Merck reagent), at a fixed pH of 7 and MG concentration of 75 mg/L, in the presence of 0.75 g/L.During reaction, about 4 mL of aliquots was sampled and separated by filtration using PTFE filters (0.45μm) to determine the residual MG concentration using UV-Vis spectrophotometer (Shimadzu 2450, Japan) at the maximal adsorption wavelength of MG λ
m
a
x
=
631 nm. Chemical Oxygen Demand (COD) was determined using the reactor digestion method based on the method of acidic oxidation by bichromate [24].Discoloration efficiency and mineralization efficiency were calculated as follows:(2)
χ
=
C
0
-
C
t
C
0
×
100
%
,where C
t and C
0 denote the time-dependent concentration/COD and the initial concentration/COD, respectively.


## 2.1. Materials

The clay used in this study was sampled in Jebel Tejera-Esghira deposits located in the southeast of Tunisia from the area of Medenine. The natural clay was first purified by dispersion in water, decantation, and extraction of the fraction with a particle size smaller than 2μm. Then, the natural clay was modified by sodium exchange described in our previous work [3, 21]. Activated carbon (AC) was prepared from the physical activation ofLawsonia inermis wood, which was obtained from the field in Gabès (Tunisia). The preparation process has been described in detail elsewhere [22]. Commercial TiO2 (Degussa P25, Degussa Chemical) was used as titanium source for the preparation of photocatalysts. Methyl Green (MG, dicationic dye, chemical formula C27H35Cl2N3·ZnCl2, M
W
=
608.8 g/mol, Sigma-Aldrich) was used to evaluate the photocatalytic efficiency of synthesized photocatalysts.


## 2.2. Synthesis of Photocatalytic Materials

TiO2/AC and TiO2/NC photocatalytic materials were prepared through an impregnation method. First, different weights of AC or NC were added under stirring to a TiO2 (P25) aqueous suspension (mixing 30 mg of TiO2 (P25) and 100 mL of distilled water). After the impregnation process, the samples obtained were washed by double-distilled water, filtered, and then dried at 110°C for 24 h. Finally, the dried material was calcined to 500°C for 3 h in a nitrogen-purged reactor tube with a heating rate of 5°C/min. The steps of the photocatalysts preparation are presented in Figure 1.Figure 1
Scheme of the preparation method of photocatalysts by the impregnation method.


## 2.3. Characterization of Photocatalysts

Several techniques were employed for the characterization of the samples. Samples were also examined under a scanning electron microscope (SEM, Hitachi SU-70). The structural feature of these samples was observed at the accelerated voltage of 1.0 kV. High resolution transmission electron microscopy (HRTEM) images were thus acquired (JEOL JEM 2011) equipped with LaB6 filament and operating at 200 kV. The images were collected with a4008
×
2672 pixels’ CCD camera (Gatan Orius SC1000) coupled with the Digital Micrograph software. Chemical analyses were obtained by an EDX microanalyzer (PGT IMIX PC) mounted on the microscope. The catalysts were dispersed in ethanol and sonicated. A drop of the dispersion was deposited on a carbon-coated copper grid for the TEM observations.Nitrogen adsorption-desorption isotherms were measured at −196°C (Fisons Sorptomatic 1990) after outgassing (10−5 Pa) for 24 h at ambient temperature. The specific surface area, S
B
E
T, was determined according to the Brunauer-Emmett-Teller (BET) method at the relative pressure, p
/
p
0, in the range of 0.05–0.1.The porosity of the photocatalysts was measured by pycnometry. In order to determine the real density (ρ
s), water was chosen since it can penetrate pores [23], whereas, for the apparent density (ρ
p), mercury was chosen since it does not penetrate into the porous network. The porosity (P) can be calculated by the following equation:(1)
P
=
ρ
s
-
ρ
p
ρ
s
×
100
%
.For the crystal phase composition and the crystallite size of the photocatalysts, X-ray diffraction measurements were carried out at room temperature using an X-ray diffractometer (Philips PW 1710 diffractometer) (Cu Kα, 40 kV/40 mA, scanning rate of 2
Θ per min). The crystallite size was calculated by X-ray line-broadening analysis using Scherrer equation [17, 19].


## 2.4. Photoreactor and Photodegradation Procedure

Photocatalytic oxidation experiments were performed in an open Pyrex-glass cell with 250 mL capacity (of 5 cm inside diameter and 11 cm height). The design description of photocatalytic reactor was reported in our earlier study [3]. Irradiation was carried out using an UV-lamp (Black-Ray B 100 W UV-lamp, V-100AP series) with a wavelength of 365 nm.A suspension was prepared by adding appropriate amount of support TiO2/AC or TiO2/NC to 200 mL of MG aqueous solution (75 mg/L) at pH 7. The pH of suspension was measured using PH-035 digital pH meter from Changlilai Technology Co., Ltd. (Shenzhen, China), by adding H2SO4 (0.1 mol/L) or NaOH (0.1 mol/L). All the experiments were performed at an ambient temperature (25 ± 1°C) and atmospheric pressure. During the experiment, air was continuously bubbled into the catalyst suspension. Prior to irradiation, the suspension was magnetically stirred in the dark for at least 60 min to ensure the establishment of an adsorption/desorption equilibrium. The experimental work of this study involved several parameters such as the pH, catalyst loading, initial dye concentration, and H2O2 concentration. Firstly, for examining the effect of pH, the pH of MG solution was adjusted using 0.1 HCl and 0.1 NaOH aqueous solutions to be 3 to 11, while fixing the MG concentration at 75 mg/L and the dosages at 1 g/L of the photocatalysts. Catalyst concentration was chosen from 0.25 to 1.75 g/L, for 75 mg/L of MG solution, at p
H
=
7. The influence of the MG dye concentration was also evaluated by varying its concentration range from 25 mg/L to 150 mg/L, at a fixed pH of 7 in the presence of 0.75 g/L. Finally, the influence of the H2O2 amount added to the MG solution was evaluated by both dosages 8 mL and 16 mL (1000 mg L−1 of H2O2 solution, prepared from H2O2 (30%) Merck reagent), at a fixed pH of 7 and MG concentration of 75 mg/L, in the presence of 0.75 g/L.During reaction, about 4 mL of aliquots was sampled and separated by filtration using PTFE filters (0.45μm) to determine the residual MG concentration using UV-Vis spectrophotometer (Shimadzu 2450, Japan) at the maximal adsorption wavelength of MG λ
m
a
x
=
631 nm. Chemical Oxygen Demand (COD) was determined using the reactor digestion method based on the method of acidic oxidation by bichromate [24].Discoloration efficiency and mineralization efficiency were calculated as follows:(2)
χ
=
C
0
-
C
t
C
0
×
100
%
,where C
t and C
0 denote the time-dependent concentration/COD and the initial concentration/COD, respectively.


## 3. Results and Discussion

### 3.1. Characterization of the Prepared Photocatalysts

The structure and morphology of the catalyst are very important parameters since they strongly determine its photocatalytic behavior. SEM images of NC and AC before and after deposition of TiO2 are shown in Figure 2. From the micrograph, it is clear that the surface morphologies of NC (Figure 2(a)) and AC (Figure 2(b)) have a porous nature with uniform structures. After impregnation process, the TiO2 particles are found to be well-dispersed. However, the immobilization of TiO2 in both supports partially blocks the porosity. TEM images also confirm that TiO2 was successfully loaded onto the surface of NC and AC at an average particle size of about 10 nm. The presence of TiO2 in the prepared materials was confirmed by EDX analysis (Table 1). TiO2/AC evidences the highest TiO2 concentration of 23.7 wt.%.Table 1
Textural and structural properties of the samples.
Sample
NC
AC
TiO2/NC
TiO2/AC
V
p (cm3/g)
0,2
0.441
0,107
0.286
P (%)
19
45.6
10.05
37.11
S
B
E
T (m2/g)
64
584
49.11
420
Crystallite size,D (nm)
—
—
18.5
21.8 nm
Anatase content,A (%)
—
—
94
89
TiO2 (wt.%)
—
—
19.1
23.7Figure 2
SEM images of (a) NC, (b) AC, (c) TiO2/NC, and (d) TiO2/AC and TEM images of (e) TiO2/NC and (f) TiO2/AC.
(a)
(b)
(c)
(d)
(e)
(f)The BET surface and pore volume of the prepared samples are presented in Table1. The large decrease in the surface area, total pore volume, and porosity of TiO2/NC and TiO2/AC indicates that the pores of AC or NC are remarkably blocked by the loaded TiO2. The presence of an anatase phase for TiO2 can further contribute to this reduction in the surface area and pore volumes due to its presence within the micro-meso texture. Thus, the percentage of anatase can be considered to be proportional to the reduction in surface area and pore volume. Thus, this parameter may be used as an inverse indicator of the loss of surface area and porosity in these materials.The X-ray diffraction (XRD) pattern of pure TiO2 (P25), TiO2/AC, and TiO2/NC is shown in Figure 3. The XRD diffraction patterns for the natural clay evidenced quartz, kaolinite, and illite coexisting as the main crystalline phases [17, 21]. The XRD for the activated carbon evidences two wide diffraction peaks typical of graphitic structures in activated carbon [22]. Upon TiO2 loading, the XRD patterns of TiO2/NC and TiO2/AC photocatalysts show the appearance of peaks at 2θ values of 25.281°, 37.934°, 48.376°, 55.296°, and 62.728° corresponding to the (101), (103), (200), (105), and (213) planes of anatase TiO2 [18], JCPDS number 21-1272. The peaks at 2θ values of 27.4° and 36.1° are characteristic of rutile TiO2, JCPDS number 21-1276. The crystallization of amorphous TiO2 into anatase occurs at about 380°C [25]. The transformation of anatase into rutile takes place between 550°C and 650°C [25]. This is the reason why, upon calcination at 500°C for 3 h, the rutile phase appears in TiO2/AC and TiO2/NC materials. As listed in Table 1, the relative contents of anatase and rutile are estimated using the Spurr-Myers equation [26]:(3)
A
%
=
I
A
I
A
+
1.265
×
I
R
×
100
,where A
(
%
) is the relative content of anatase and I
A and I
R are the intensities of the anatase (101) peak at 2
θ
=
25.281
° and the rutile (101) peak at 2
θ
=
27.234
°. The anatase content of materials is 94% and 89% for TiO2/AC and TiO2/NC, respectively. These values show that the anatase phase is highly predominant in all cases. The main active crystal phases of TiO2 are anatase and rutile. Out of the two TiO2 phases, anatase is typically more active in photocatalytic reactions [18, 19]. According to Ambrus et al. [27], photocatalysts containing the anatase phase are more active than rutile-only catalyst.Figure 3
XRD patterns of TiO2/NC, TiO2/NC, and TiO2 (P25).The TiO2 crystal sizes in TiO2/NC and TiO2/AC materials were calculated using Scherrer’s equation through the XRD line-broadening method:(4)
D
=
k
λ
β
cos
⁡
θ
⁡
.In this equation, D is the crystallite size of the photocatalyst, k is dimensionless constant (0.9), λ is the wavelength of X-ray (Cu Kα radiation λ
=
1.5406 Å), β is the full width at half-maximum (FWHM) of the diffraction peak, and θ is the diffraction angle. The average crystallite size for TiO2/NC was found to be 18.5 nm, whereas a crystallite size of 21.8 nm was estimated for TiO2/AC.


### 3.2. Photocatalytic Degradation of Methyl Green

Figure4 shows the results of the photocatalytic experiments in the presence of the different materials prepared and under different reaction conditions. The photolysis of MG under UV irradiation, without the presence of photocatalysts, results in negligible degradation of the dye, at least during the 180 min duration of the test. Regarding the direct adsorption of MG on the surface of the photocatalysts (tests in the absence of UV irradiation), the amount of MG adsorbed onto TiO2/AC irradiation was found to be higher than for TiO2/NC. This fact can be assigned to the larger surface area of this material and to the well-known good adsorption properties of activated carbon. For the sake of comparison, the nonimpregnated supports were tested in the photocatalytic degradation of MG: 53.7% and 39.5% of the dye were, respectively, removed by the activated carbon and natural clay from 100 mg/L MG solutions after 60 minutes of reaction. These percentages of MG degradation can be only related to enhanced absorption of the organic dye on the support surface. The incorporation of TiO2 results in extensive pore blockage and in a considerable reduction of the adsorption capacity. TiO2 supported on activated carbon or on natural clay is more active than pure TiO2 (P25) powder. It can be seen that the removal of MG using pure TiO2 (P25) reached 52.8% within 60 min irradiation time. In the presence of TiO2/AC and TiO2/NC, MG degradation reached 98.6% and 90.2%, within the same irradiation time. Note that the photocatalytic activity of TiO2/AC is higher than that of TiO2/NC. This result is in correlation with the physicochemical properties of materials; the anatase content and the specific surface area of TiO2/AC were higher than those of TiO2/NC (Table 1). Moreover, better light absorption properties of a “black” material such as activated carbon can be expected.Figure 4
Photocatalytic degradation of MG by the different samples. The inset shows the maximum adsorption in the dark after 60 minutes (initial concentration of MG = 75 mg/L, photocatalyst amount = 1 g/L, and irradiation time = 180 min).It has been established that photocatalyzed degradation of organic pollutants in aqueous solution is initiated by the photoexcitation of TiO2, followed by the formation of an electron-hole pair on the surface of catalyst [7, 18, 19]:(5)
T
i
O
2
+
h
ν
⟶
T
i
O
2
+
h
+
v
b
+
e
-
c
bThe high oxidation potential of the hole (h
+
v
b) allows the oxidation of organic pollutant (dye) to the degradation products:(6)
h
+
v
b
+
pollutant
⟶
pollutant
∗
+
⟶
degradation  of  pollutantHowever, very reactive hydroxyl radicals (•OH) can also be formed either by the decomposition of water or by the reaction of the hole with OH−:(7)
h
+
v
b
+
H
2
O
⟶
H
O
•
+
H
+
(8)
h
+
v
b
+
H
O
-
⟶
H
O
•
•OH is an exclusively strong, nonselective oxidant, which conducts the partial or complete mineralization of organic pollutants [7, 8].Electrons (e
-
c
b) in the conduction bond on the TiO2 surface can reduce molecular oxygen to superoxide anions. These superoxide anions are responsible for the generation of •OH that has been indicated as the primary source of pollutant degradation [19]:(9)
e
-
c
b
+
O
2
⟶
O
2
•
-
(10)
2
O
2
•
-
+
2
H
2
O
⟶
H
O
•
+
2
H
O
-
+
O
2
(11)
H
O
•
+
pollutant
M
G
⟶
C
O
2
+
H
2
O
+
other  degradation  products


### 3.3. Effect of pH

Wastewaters from textile industries usually have a wide range of pH. Thus, pH plays an important role in photodegradation processes [4, 8, 28]. The effect of the initial solution pH on the photocatalytic degradation in the presence of TiO2 supported on AC and NC is presented in Figure 5. MG removal increases with increasing initial pH of the dye solution. The influence of pH on photocatalytic activity has been related to the surface charge properties of the photocatalysts and could be explained based on the point of zero charge (pzc). The point of zero charge (pzc) of TiO2 is 6.8 [28]. In acidic media (pH < 6.8), the surface of TiO2 is positively charged, whereas it is negatively charged under alkaline conditions (pH > 6.8) according to (12)
T
i
O
H
+
H
+
⟷
T
i
O
H
2
+
a
t
p
H
<
p
z
c
(13)
T
i
O
H
+
O
H
-
⟷
T
i
O
-
+
H
2
O
a
t
p
H
>
p
z
cMethyl Green, a cationic dye, is positivity charged due to the ammonium groups which are ionized in water; their electrostatic attraction to the catalyst surface is favorable in basic solution and hindered in acidic media, due to the columbic repulsion between the positively charged photocatalyst surface and the positively charged dye molecules [4, 28, 29]. Thus, interaction and thus reaction might be favored at high pH. Moreover, the generation of HO• radicals by the effect of UV irradiation may also be responsible for increasing reaction rate in a basic environment. In acidic media (pH < 7), such radical species are rapidly scavenged and therefore the reaction rate decreases, thus resulting in favored reaction at high pH.Figure 5
Effect of pH on photocatalytic degradation of MG using TiO2 (P25), TiO2/NC, and TiO2/AC (initial concentration of MG = 75 mg/L, photocatalyst amount = 0.75 g/L, and irradiation time = 180 min).


### 3.4. Effect of Catalytic Concentration

In order to avoid the use of excess catalyst, it is necessary to find out the optimum loading for efficient removal of the organic compounds in wastewaters. Several authors have investigated the reaction rate as a function of catalyst loading in photocatalytic degradation process [10, 29–31]. The effect of catalyst concentration on degradation of the MG dye over TiO2, TiO2/NC, and TiO2/AC is shown in Figure 6. The catalyst loading changed from 0.25 to 1.75 g/L. The figure shows that the percentage of removal of MG is enhanced when the amount of catalyst in the reactor increases up to 1 g/L over TiO2 (P25) and up to 0.75 g/L over both TiO2/NC and TiO2/AC and then decreases for higher catalyst loads. This increase in the degradation efficiency in the presence of an increased amount of catalyst in the solution is obviously due to the increase of the active material and thus TiO2 active sites, resulting in enhanced free hydroxyl radical generation [29–31]. However, for catalyst loads higher than 1 g/L, a steady state is reached in terms of degradation since a plateau is reached considering the experimental errors.Figure 6
Effect of catalyst loading on photocatalytic degradation of MG using TiO2 (P25), TiO2/NC, and TiO2/AC (initial concentration of MG = 75 mg/L and irradiation time = 180 min at pH = 7).


### 3.5. Effect of Initial Dye Concentration

Dye concentration was varied between 25 and 150 mg/L with constant catalyst loading at pH 7. The influence of initial dye concentration is shown in Figures7(a), 7(b), and 7(c), in the presence of TiO2 (P25), TiO2/NC, and TiO2/AC, respectively, where a plot of ln
⁡
C
/
C
0 versus time of irradiation is represented. From the results, the photocatalytic degradation of MG followed pseudo-first-order kinetics (Table 2). A linear relation between dye concentration and irradiation time has been observed. It was found that the increase in the dye concentration decreases the removal rate. The results are listed in Table 2. One can conclude that TiO2/AC catalyst is more efficient than TiO2/NC, with the ratio of apparent rate varying from 1.2 to 1.6 depending on the conditions.Table 2
Degradation reaction rate constants by UV irradiation photocatalytic oxidation of MG dye over TiO2/AC, TiO2/NC, and TiO2 (P25).
Initial concentration (mg/L)
TiO2/AC
TiO2/NC
TiO2 (P25)
k
′
R
2
k
′
R
2
k
′
R
2
25
0,0458
0,9942
0,0306
0,9945
0,0214
0,9944
50
0,0384
0,994
0,0239
0,9898
0,0195
0,9917
75
0,0303
0,987
0,0187
0,9941
0,0146
0,9828
100
0,0253
0,9934
0,0139
0,9915
0,0091
0,9904
150
0,0133
0,9883
0,0106
0,9869
0,0043
0,9564
k
′: estimated rate constant; R
2: correlation factor.Figure 7
(a) Effect of initial dye concentration on photocatalytic degradation of MG using TiO2 (P25) (photocatalyst amount = 0.75 g/L and irradiation time = 180 min at pH = 7). (b) Effect of initial dye concentration on photocatalytic degradation of MG using TiO2/NC (photocatalyst amount = 0.75 g/L and irradiation time = 180 min at pH = 7).
(a)
(b)
(c)Similar results have been reported for the photocatalytic oxidation of other dyes [1, 17, 30]. The rate of degradation relates to the rate of •OH radicals formation and to the probability of •OH radicals to react with the dye molecules. Since the generation of radicals remains constant for each set of reaction conditions, the probability of dye molecule to react with hydroxyl radical decreases as dye concentration decreases, resulting in lower reaction rate. However, at relatively high initial dye concentrations, the path length of the photons entering the solution also decreases. Thus, the photocatalytic degradation efficiency decreases within the range of very high dye concentrations [16, 30, 32].


### 3.6. Effect of Addition of H2O2

Addition of Hydrogen Peroxide (HP) to TiO2 suspensions is a well-known strategy towards increasing the degradation efficiency of organic pollutants in wastewaters [7, 8, 32, 33]. H2O2 is considered to have two functions in the photocatalytic oxidation. It accepts a photogenerated electron from the conduction band of the semiconductor to form •OH radical (reaction (14)), and, in addition, it forms •OH radicals according to reaction (15) [8]:(14)
H
2
O
2
+
e
-
⟶
H
O
•
+
O
H
-
(15)
H
2
O
2
+
O
2
•
-
⟶
H
O
•
+
O
H
-
+
O
2Figure 8 shows the results of the photodegradation experiments carried out at both H2O2 dosages 8 mL and 16 mL, at pH = 7, in the presence of 0.75 g/L photocatalysis and UV irradiation. Results point out an optimal oxidant dosage. Excess of H2O2 can act in fact as •OH scavenger resulting in the generation of perhydroxyl radical (H
O
2
•) (see (16)–(18)), a less strong oxidant as compared to hydroxyl radicals [3, 8]:(16)
H
2
O
2
+
H
O
•
⟶
H
O
2
•
+
H
2
O
(17)
H
O
•
+
H
O
2
•
⟶
O
2
+
H
2
O
(18)
H
2
O
2
+
h
+
⟶
H
+
+
H
O
2
•Figure 8
Effect of HP concentration on photocatalytic degradation of MG using TiO2 (P25), TiO2/NC, and TiO2/AC (initial concentration of MG = 75 mg/L, photocatalyst amount = 0.75 g/L, and irradiation time = 30 min at pH = 7).


### 3.7. UV-Visible Absorption and COD Analysis

Mineralization of MG (complete oxidation) in the presence of the different photocatalytic materials has been evaluated by means of following the evolution of UV-Vis absorption and by means of COD measurements. Degradation experiments were performed at pH of 6.51, 75 mg/L dye concentration, 100 mg of photocatalyst, and 8 mL of H2O2. Solutions were then analyzed every 30 minutes. Figure 9 shows the evolution of the UV-Vis spectra. Four absorption peaks can be observed in the spectrum corresponding to the initial MG solution: the peak observed in the visible region at 631 nm is due to the green color of the chromophore of MG, and three other peaks at 420 nm, 315 nm, and 256 nm correspond to the benzoic rings in the dye structure. Upon 30 min irradiation, in the presence of the TiO2/AC catalyst, the peak corresponding to the dye chromophore completely disappeared. COD analyses were performed to confirm the complete mineralization of MG. The percentage of COD elimination is presented in Table 3. After 60 min irradiation in the presence of TiO2/AC and TiO2/NC, 98.80% and 95.11% of COD elimination are obtained, respectively. These results confirmed that TiO2/AC are more efficient for MG degradation, as already observed from kinetic study (Figure 7).Table 3
COD measurements.
Sample
% of COD reduction
TiO2 (P25)
47.94
TiO2/AC
98.80
TiO2/NC
95.11Figure 9
Evolution of UV-Vis spectra of Methyl Green (MG) aqueous solution with reaction time (initial concentration of MG = 75 mg, photocatalyst amount = 0.75 g, HP = 8 mL, and irradiation time = 30 min at pH = 7).


### 3.8. Reusing of the Photocatalytic Materials

In order to study the reusability of the proposed photocatalysts, repeated degradation experiments were performed under optimized conditions. At the end of the degradation process, the suspension was centrifuged and the catalyst washed with water and dried at 120°C for future uses (Figure10). The decrease in degradation efficiency is not significant for the supported TiO2 materials, TiO2/AC and TiO2/NC, whereas, for the nonsupported titania powder, TiO2 (P25), the decrease in activity is really noticeable. These results prove the positive effect of using a porous support for stabilizing TiO2 particles, resulting not only in higher photocatalytic activity but also in enhancing the stability of the proposed materials.Figure 10
MG degradation by repeated use of the prepared photocatalysts (initial concentration of MG = 75 mg, photocatalyst amount = 0.75 g, and irradiation time = 180 min).


## 3.1. Characterization of the Prepared Photocatalysts

The structure and morphology of the catalyst are very important parameters since they strongly determine its photocatalytic behavior. SEM images of NC and AC before and after deposition of TiO2 are shown in Figure 2. From the micrograph, it is clear that the surface morphologies of NC (Figure 2(a)) and AC (Figure 2(b)) have a porous nature with uniform structures. After impregnation process, the TiO2 particles are found to be well-dispersed. However, the immobilization of TiO2 in both supports partially blocks the porosity. TEM images also confirm that TiO2 was successfully loaded onto the surface of NC and AC at an average particle size of about 10 nm. The presence of TiO2 in the prepared materials was confirmed by EDX analysis (Table 1). TiO2/AC evidences the highest TiO2 concentration of 23.7 wt.%.Table 1
Textural and structural properties of the samples.
Sample
NC
AC
TiO2/NC
TiO2/AC
V
p (cm3/g)
0,2
0.441
0,107
0.286
P (%)
19
45.6
10.05
37.11
S
B
E
T (m2/g)
64
584
49.11
420
Crystallite size,D (nm)
—
—
18.5
21.8 nm
Anatase content,A (%)
—
—
94
89
TiO2 (wt.%)
—
—
19.1
23.7Figure 2
SEM images of (a) NC, (b) AC, (c) TiO2/NC, and (d) TiO2/AC and TEM images of (e) TiO2/NC and (f) TiO2/AC.
(a)
(b)
(c)
(d)
(e)
(f)The BET surface and pore volume of the prepared samples are presented in Table1. The large decrease in the surface area, total pore volume, and porosity of TiO2/NC and TiO2/AC indicates that the pores of AC or NC are remarkably blocked by the loaded TiO2. The presence of an anatase phase for TiO2 can further contribute to this reduction in the surface area and pore volumes due to its presence within the micro-meso texture. Thus, the percentage of anatase can be considered to be proportional to the reduction in surface area and pore volume. Thus, this parameter may be used as an inverse indicator of the loss of surface area and porosity in these materials.The X-ray diffraction (XRD) pattern of pure TiO2 (P25), TiO2/AC, and TiO2/NC is shown in Figure 3. The XRD diffraction patterns for the natural clay evidenced quartz, kaolinite, and illite coexisting as the main crystalline phases [17, 21]. The XRD for the activated carbon evidences two wide diffraction peaks typical of graphitic structures in activated carbon [22]. Upon TiO2 loading, the XRD patterns of TiO2/NC and TiO2/AC photocatalysts show the appearance of peaks at 2θ values of 25.281°, 37.934°, 48.376°, 55.296°, and 62.728° corresponding to the (101), (103), (200), (105), and (213) planes of anatase TiO2 [18], JCPDS number 21-1272. The peaks at 2θ values of 27.4° and 36.1° are characteristic of rutile TiO2, JCPDS number 21-1276. The crystallization of amorphous TiO2 into anatase occurs at about 380°C [25]. The transformation of anatase into rutile takes place between 550°C and 650°C [25]. This is the reason why, upon calcination at 500°C for 3 h, the rutile phase appears in TiO2/AC and TiO2/NC materials. As listed in Table 1, the relative contents of anatase and rutile are estimated using the Spurr-Myers equation [26]:(3)
A
%
=
I
A
I
A
+
1.265
×
I
R
×
100
,where A
(
%
) is the relative content of anatase and I
A and I
R are the intensities of the anatase (101) peak at 2
θ
=
25.281
° and the rutile (101) peak at 2
θ
=
27.234
°. The anatase content of materials is 94% and 89% for TiO2/AC and TiO2/NC, respectively. These values show that the anatase phase is highly predominant in all cases. The main active crystal phases of TiO2 are anatase and rutile. Out of the two TiO2 phases, anatase is typically more active in photocatalytic reactions [18, 19]. According to Ambrus et al. [27], photocatalysts containing the anatase phase are more active than rutile-only catalyst.Figure 3
XRD patterns of TiO2/NC, TiO2/NC, and TiO2 (P25).The TiO2 crystal sizes in TiO2/NC and TiO2/AC materials were calculated using Scherrer’s equation through the XRD line-broadening method:(4)
D
=
k
λ
β
cos
⁡
θ
⁡
.In this equation, D is the crystallite size of the photocatalyst, k is dimensionless constant (0.9), λ is the wavelength of X-ray (Cu Kα radiation λ
=
1.5406 Å), β is the full width at half-maximum (FWHM) of the diffraction peak, and θ is the diffraction angle. The average crystallite size for TiO2/NC was found to be 18.5 nm, whereas a crystallite size of 21.8 nm was estimated for TiO2/AC.


## 3.2. Photocatalytic Degradation of Methyl Green

Figure4 shows the results of the photocatalytic experiments in the presence of the different materials prepared and under different reaction conditions. The photolysis of MG under UV irradiation, without the presence of photocatalysts, results in negligible degradation of the dye, at least during the 180 min duration of the test. Regarding the direct adsorption of MG on the surface of the photocatalysts (tests in the absence of UV irradiation), the amount of MG adsorbed onto TiO2/AC irradiation was found to be higher than for TiO2/NC. This fact can be assigned to the larger surface area of this material and to the well-known good adsorption properties of activated carbon. For the sake of comparison, the nonimpregnated supports were tested in the photocatalytic degradation of MG: 53.7% and 39.5% of the dye were, respectively, removed by the activated carbon and natural clay from 100 mg/L MG solutions after 60 minutes of reaction. These percentages of MG degradation can be only related to enhanced absorption of the organic dye on the support surface. The incorporation of TiO2 results in extensive pore blockage and in a considerable reduction of the adsorption capacity. TiO2 supported on activated carbon or on natural clay is more active than pure TiO2 (P25) powder. It can be seen that the removal of MG using pure TiO2 (P25) reached 52.8% within 60 min irradiation time. In the presence of TiO2/AC and TiO2/NC, MG degradation reached 98.6% and 90.2%, within the same irradiation time. Note that the photocatalytic activity of TiO2/AC is higher than that of TiO2/NC. This result is in correlation with the physicochemical properties of materials; the anatase content and the specific surface area of TiO2/AC were higher than those of TiO2/NC (Table 1). Moreover, better light absorption properties of a “black” material such as activated carbon can be expected.Figure 4
Photocatalytic degradation of MG by the different samples. The inset shows the maximum adsorption in the dark after 60 minutes (initial concentration of MG = 75 mg/L, photocatalyst amount = 1 g/L, and irradiation time = 180 min).It has been established that photocatalyzed degradation of organic pollutants in aqueous solution is initiated by the photoexcitation of TiO2, followed by the formation of an electron-hole pair on the surface of catalyst [7, 18, 19]:(5)
T
i
O
2
+
h
ν
⟶
T
i
O
2
+
h
+
v
b
+
e
-
c
bThe high oxidation potential of the hole (h
+
v
b) allows the oxidation of organic pollutant (dye) to the degradation products:(6)
h
+
v
b
+
pollutant
⟶
pollutant
∗
+
⟶
degradation  of  pollutantHowever, very reactive hydroxyl radicals (•OH) can also be formed either by the decomposition of water or by the reaction of the hole with OH−:(7)
h
+
v
b
+
H
2
O
⟶
H
O
•
+
H
+
(8)
h
+
v
b
+
H
O
-
⟶
H
O
•
•OH is an exclusively strong, nonselective oxidant, which conducts the partial or complete mineralization of organic pollutants [7, 8].Electrons (e
-
c
b) in the conduction bond on the TiO2 surface can reduce molecular oxygen to superoxide anions. These superoxide anions are responsible for the generation of •OH that has been indicated as the primary source of pollutant degradation [19]:(9)
e
-
c
b
+
O
2
⟶
O
2
•
-
(10)
2
O
2
•
-
+
2
H
2
O
⟶
H
O
•
+
2
H
O
-
+
O
2
(11)
H
O
•
+
pollutant
M
G
⟶
C
O
2
+
H
2
O
+
other  degradation  products


## 3.3. Effect of pH

Wastewaters from textile industries usually have a wide range of pH. Thus, pH plays an important role in photodegradation processes [4, 8, 28]. The effect of the initial solution pH on the photocatalytic degradation in the presence of TiO2 supported on AC and NC is presented in Figure 5. MG removal increases with increasing initial pH of the dye solution. The influence of pH on photocatalytic activity has been related to the surface charge properties of the photocatalysts and could be explained based on the point of zero charge (pzc). The point of zero charge (pzc) of TiO2 is 6.8 [28]. In acidic media (pH < 6.8), the surface of TiO2 is positively charged, whereas it is negatively charged under alkaline conditions (pH > 6.8) according to (12)
T
i
O
H
+
H
+
⟷
T
i
O
H
2
+
a
t
p
H
<
p
z
c
(13)
T
i
O
H
+
O
H
-
⟷
T
i
O
-
+
H
2
O
a
t
p
H
>
p
z
cMethyl Green, a cationic dye, is positivity charged due to the ammonium groups which are ionized in water; their electrostatic attraction to the catalyst surface is favorable in basic solution and hindered in acidic media, due to the columbic repulsion between the positively charged photocatalyst surface and the positively charged dye molecules [4, 28, 29]. Thus, interaction and thus reaction might be favored at high pH. Moreover, the generation of HO• radicals by the effect of UV irradiation may also be responsible for increasing reaction rate in a basic environment. In acidic media (pH < 7), such radical species are rapidly scavenged and therefore the reaction rate decreases, thus resulting in favored reaction at high pH.Figure 5
Effect of pH on photocatalytic degradation of MG using TiO2 (P25), TiO2/NC, and TiO2/AC (initial concentration of MG = 75 mg/L, photocatalyst amount = 0.75 g/L, and irradiation time = 180 min).


## 3.4. Effect of Catalytic Concentration

In order to avoid the use of excess catalyst, it is necessary to find out the optimum loading for efficient removal of the organic compounds in wastewaters. Several authors have investigated the reaction rate as a function of catalyst loading in photocatalytic degradation process [10, 29–31]. The effect of catalyst concentration on degradation of the MG dye over TiO2, TiO2/NC, and TiO2/AC is shown in Figure 6. The catalyst loading changed from 0.25 to 1.75 g/L. The figure shows that the percentage of removal of MG is enhanced when the amount of catalyst in the reactor increases up to 1 g/L over TiO2 (P25) and up to 0.75 g/L over both TiO2/NC and TiO2/AC and then decreases for higher catalyst loads. This increase in the degradation efficiency in the presence of an increased amount of catalyst in the solution is obviously due to the increase of the active material and thus TiO2 active sites, resulting in enhanced free hydroxyl radical generation [29–31]. However, for catalyst loads higher than 1 g/L, a steady state is reached in terms of degradation since a plateau is reached considering the experimental errors.Figure 6
Effect of catalyst loading on photocatalytic degradation of MG using TiO2 (P25), TiO2/NC, and TiO2/AC (initial concentration of MG = 75 mg/L and irradiation time = 180 min at pH = 7).


## 3.5. Effect of Initial Dye Concentration

Dye concentration was varied between 25 and 150 mg/L with constant catalyst loading at pH 7. The influence of initial dye concentration is shown in Figures7(a), 7(b), and 7(c), in the presence of TiO2 (P25), TiO2/NC, and TiO2/AC, respectively, where a plot of ln
⁡
C
/
C
0 versus time of irradiation is represented. From the results, the photocatalytic degradation of MG followed pseudo-first-order kinetics (Table 2). A linear relation between dye concentration and irradiation time has been observed. It was found that the increase in the dye concentration decreases the removal rate. The results are listed in Table 2. One can conclude that TiO2/AC catalyst is more efficient than TiO2/NC, with the ratio of apparent rate varying from 1.2 to 1.6 depending on the conditions.Table 2
Degradation reaction rate constants by UV irradiation photocatalytic oxidation of MG dye over TiO2/AC, TiO2/NC, and TiO2 (P25).
Initial concentration (mg/L)
TiO2/AC
TiO2/NC
TiO2 (P25)
k
′
R
2
k
′
R
2
k
′
R
2
25
0,0458
0,9942
0,0306
0,9945
0,0214
0,9944
50
0,0384
0,994
0,0239
0,9898
0,0195
0,9917
75
0,0303
0,987
0,0187
0,9941
0,0146
0,9828
100
0,0253
0,9934
0,0139
0,9915
0,0091
0,9904
150
0,0133
0,9883
0,0106
0,9869
0,0043
0,9564
k
′: estimated rate constant; R
2: correlation factor.Figure 7
(a) Effect of initial dye concentration on photocatalytic degradation of MG using TiO2 (P25) (photocatalyst amount = 0.75 g/L and irradiation time = 180 min at pH = 7). (b) Effect of initial dye concentration on photocatalytic degradation of MG using TiO2/NC (photocatalyst amount = 0.75 g/L and irradiation time = 180 min at pH = 7).
(a)
(b)
(c)Similar results have been reported for the photocatalytic oxidation of other dyes [1, 17, 30]. The rate of degradation relates to the rate of •OH radicals formation and to the probability of •OH radicals to react with the dye molecules. Since the generation of radicals remains constant for each set of reaction conditions, the probability of dye molecule to react with hydroxyl radical decreases as dye concentration decreases, resulting in lower reaction rate. However, at relatively high initial dye concentrations, the path length of the photons entering the solution also decreases. Thus, the photocatalytic degradation efficiency decreases within the range of very high dye concentrations [16, 30, 32].


## 3.6. Effect of Addition of H2O2

Addition of Hydrogen Peroxide (HP) to TiO2 suspensions is a well-known strategy towards increasing the degradation efficiency of organic pollutants in wastewaters [7, 8, 32, 33]. H2O2 is considered to have two functions in the photocatalytic oxidation. It accepts a photogenerated electron from the conduction band of the semiconductor to form •OH radical (reaction (14)), and, in addition, it forms •OH radicals according to reaction (15) [8]:(14)
H
2
O
2
+
e
-
⟶
H
O
•
+
O
H
-
(15)
H
2
O
2
+
O
2
•
-
⟶
H
O
•
+
O
H
-
+
O
2Figure 8 shows the results of the photodegradation experiments carried out at both H2O2 dosages 8 mL and 16 mL, at pH = 7, in the presence of 0.75 g/L photocatalysis and UV irradiation. Results point out an optimal oxidant dosage. Excess of H2O2 can act in fact as •OH scavenger resulting in the generation of perhydroxyl radical (H
O
2
•) (see (16)–(18)), a less strong oxidant as compared to hydroxyl radicals [3, 8]:(16)
H
2
O
2
+
H
O
•
⟶
H
O
2
•
+
H
2
O
(17)
H
O
•
+
H
O
2
•
⟶
O
2
+
H
2
O
(18)
H
2
O
2
+
h
+
⟶
H
+
+
H
O
2
•Figure 8
Effect of HP concentration on photocatalytic degradation of MG using TiO2 (P25), TiO2/NC, and TiO2/AC (initial concentration of MG = 75 mg/L, photocatalyst amount = 0.75 g/L, and irradiation time = 30 min at pH = 7).


## 3.7. UV-Visible Absorption and COD Analysis

Mineralization of MG (complete oxidation) in the presence of the different photocatalytic materials has been evaluated by means of following the evolution of UV-Vis absorption and by means of COD measurements. Degradation experiments were performed at pH of 6.51, 75 mg/L dye concentration, 100 mg of photocatalyst, and 8 mL of H2O2. Solutions were then analyzed every 30 minutes. Figure 9 shows the evolution of the UV-Vis spectra. Four absorption peaks can be observed in the spectrum corresponding to the initial MG solution: the peak observed in the visible region at 631 nm is due to the green color of the chromophore of MG, and three other peaks at 420 nm, 315 nm, and 256 nm correspond to the benzoic rings in the dye structure. Upon 30 min irradiation, in the presence of the TiO2/AC catalyst, the peak corresponding to the dye chromophore completely disappeared. COD analyses were performed to confirm the complete mineralization of MG. The percentage of COD elimination is presented in Table 3. After 60 min irradiation in the presence of TiO2/AC and TiO2/NC, 98.80% and 95.11% of COD elimination are obtained, respectively. These results confirmed that TiO2/AC are more efficient for MG degradation, as already observed from kinetic study (Figure 7).Table 3
COD measurements.
Sample
% of COD reduction
TiO2 (P25)
47.94
TiO2/AC
98.80
TiO2/NC
95.11Figure 9
Evolution of UV-Vis spectra of Methyl Green (MG) aqueous solution with reaction time (initial concentration of MG = 75 mg, photocatalyst amount = 0.75 g, HP = 8 mL, and irradiation time = 30 min at pH = 7).


## 3.8. Reusing of the Photocatalytic Materials

In order to study the reusability of the proposed photocatalysts, repeated degradation experiments were performed under optimized conditions. At the end of the degradation process, the suspension was centrifuged and the catalyst washed with water and dried at 120°C for future uses (Figure10). The decrease in degradation efficiency is not significant for the supported TiO2 materials, TiO2/AC and TiO2/NC, whereas, for the nonsupported titania powder, TiO2 (P25), the decrease in activity is really noticeable. These results prove the positive effect of using a porous support for stabilizing TiO2 particles, resulting not only in higher photocatalytic activity but also in enhancing the stability of the proposed materials.Figure 10
MG degradation by repeated use of the prepared photocatalysts (initial concentration of MG = 75 mg, photocatalyst amount = 0.75 g, and irradiation time = 180 min).


## 4. Conclusions

TiO2 nanoparticles were immobilized on the surface of two different supports, natural clay and activated carbon. The resulting photocatalysts TiO2/AC and TiO2/NC were characterized by means of XRD, SEM, TEM, and N2 physisorption. TiO2/AC was found to be more efficient towards UV-photocatalytic degradation of Methyl Green in aqueous solution than TiO2/NC. This can be due to the particular physicochemical properties of the AC support together with increased light absorption related to its optical properties. Both TiO2 supported catalysts were considerably more efficient than the nonsupported TiO2 (P25) powder, pointing to a positive effect of TiO2 nanoparticle immobilization on both supports. Degradation was found to be slightly more efficient at high pH. The optimum catalyst loading for efficient removal was found to be 0.75 g/L, for both supported catalysts. The evolution of UV-Vis spectra together with COD measurements confirmed the complete mineralization of the organic dye. After 60 min irradiation in the presence of TiO2/AC and TiO2/NC, 98.80% and 95.11% of COD elimination were, respectively, measured. Moreover, using AC and NC as supports for immobilizing TiO2 nanoparticles resulted in enhancement of the stability of the supported photocatalysts, in comparison to nonsupported TiO2 powders.



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*Source: 759853-2015-10-13.xml*