# New Surface Aspects towards Photocatalytic Activity of Doped Supported Titanium Dioxide

Authors: Samia A. Kosa; Eman Z. Hegazy; Saleha S. Maashi; Islam H. Abd El Maksod; Laila M. Al-Harbi
Journal: International Journal of Photoenergy
 (2016)

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## Abstract

The present work aims to synthesize nanoscale well dispersed TiO2/SiO2 and TiO2/Al2O3 nanoparticle photocatalysts via an impregnation method for the removal of methyl orange, which was used as a model compound of organic pollutant in wastewater, from an aqueous medium. Also within this frame work, La and Ce metals were loaded onto the surfaces of TiO2/SiO2 and TiO2/Al2O3 by an impregnation method to enhance the photocatalytic activity of the nanoparticles; the activities and physicochemical properties of the photocatalysts were compared before and after loading of metallic La and Ce. The oxide system was characterized by different techniques, including XRD, UV-Vis spectroscopy, FT-IR spectroscopy, SEM, and EDX spectroscopy. Finally, the optimal conditions to complete the photocatalytic oxidation of methyl orange dye were studied. This work holds promise for the efficient photodegradation of pollutants by nanoparticle photocatalysts.


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## Body

## 1. Introduction

Methyl orange is widely used as an acid-base indicator, and it has also been employed in chemical, technological, and biomedical industries. Its chemical properties have been widely investigated in aqueous solutions and in water and organic mixed solvents [1]. Additionally, this compound has been widely used in printing, paper, food, pharmaceutical, and textile industries, as well as research laboratories [2]. It is an orange-colored, anionic dye that possesses absorbance maximum at 464 nm. Methyl orange is a compound that exists in textile wastewaters and has various harmful effects on humans. For example, it may cause eye or skin irritation, and inhalation may cause gastrointestinal irritation with nausea, vomiting, and diarrhea. There are various technological processes such as adsorption, biodegradation, chemical methods, electrocoagulation, electrochemical reduction and oxidation, indirect electrooxidation with strong oxidants, and photocatalytic degradation that can be used for the treatment of wastewaters, including those containing synthetic dyes [3, 4]. A number of studies have dealt with the heterogeneous photocatalytic decomposition of many types of azo dyes by UV, visible light, and solar irradiation. The dangerous accumulation of dyes in the environment can be avoided by developing effective ways for their removal either by the degradation of such organic pollutants to less harmful compounds [5] or by their complete mineralization [6], such as titanium dioxide, which has been widely used as a photocatalyst for the degradation of МО. The photocatalytic efficiency of a nanocrystalline TiO2 system is strongly influenced by light sources and the recombination of photoinduced electrons and holes. It is known that gold deposited onto TiO2 surface inhibits the recombination of photogenerated electrons and holes. The photocatalytic deposition of metals onto titanium dioxide films is one of the most interesting methods for producing titanium dioxide/metal composites. The pairing of TiO2 with other metals, including Au, Ti, Ce, Fe, and Pt [6], has been used to increase the activity of TiO2 towards the degradation of azo dyes, such as methyl orange.


## 2. Experimental

### 2.1. Materials

All chemicals used in the preparation of TiO2/SiO2, TiO2/Al2O3, La-TiO2/Al2O3, and Ce-TiO2/Al2O3 nanoparticles were analytical grade reagents. The following high purity raw materials were used:(i)
Titanium(IV) oxide, anatase, 325 mesh, ≥99% metals basis, TiO2, Sigma-Aldrich Laboratories Supplies [Canada].
(ii)
Titanium(IV) isopropoxide, 98%, C12H28O4Ti, ACROS Organics.
(iii)
Titanium tetrachloride, TiCl4, Fluka AG Laboratories Supplies.
(iv)
Aluminum oxide, Al2O3, Fluka Laboratories Supplies [Switzerland].
(v)
Silica precipitated, SiO2, BDH Laboratories Supplies [Poole, England].
(vi)
Lanthanum(III) nitrate hexahydrate, La(NO3)3·6H2O, 99.999%, ACROS Organics Laboratories Supplies [New Jersey, USA].
(vii)
Ammonium cerium(IV) nitrate, 99%, H8CeN8O18, ACROS Organics Laboratories Supplies [New Jersey, USA].
(viii)
Methyl orange indicator, Pacegrove Limited Laboratories Supplies [UK].


### 2.2. Procedure and Apparatus

The loading of titanium tetra chloride (TiCl4) or titanium isopropoxide (TIP) into silica (SiO2) or aluminum oxide (Al2O3) was performed by the impregnation method (Img).


#### 2.2.1. Preparation of TiO2/SiO2

Five grams of silica was mixed with a certain amount of titanium isopropoxide (TIP) or titanium tetra chloride (TiCl4). Then, a minimal amount of distilled water was added dropwise to the mixture, under vigorous stirring, to obtain 2.5, 5, 10, and 20 wt.% TiO2, as shown in Table 1. The formed paste was completely mixed to obtain a homogeneous mixture, and it was then dried in an oven at 100°C for 24 h. The resultant powder was ground using a mortar and pestle, followed by calcination at 550°C for 4 h in open air atmosphere.Table 1
Compositions of different TiO2/SiO2 samples.
Concentration of TiO2 (wt.%) in TiO2/SiO2
Source of titanium
Support type
2.5
TiCl4
SiO2
5
10
20
2.5
TIP
5
10
20


#### 2.2.2. Preparation of TiO2/Al2O3

Five grams of aluminum oxide (Al2O3) was mixed with a certain amount of titanium isopropoxide (TIP) or titanium tetra chloride (TiCl4). Then, a minimal amount of distilled water was added dropwise to the mixture, under vigorous stirring, to obtain 2.5, 5, 10, and 20 wt.% TiO2, as shown in Table 2. The formed paste was completely mixed to obtain a homogeneous mixture, which was then dried in an oven at 100°C for 24 h. The powder was ground using a mortar and pestle, followed by calcination at 550°C for 4 h.Table 2
Compositions of different TiO2/Al2O3 samples.
Concentration of TiO2 (wt.%) in TiO2/Al2O3
Source of titanium
Support type
2.5
TiCl4
Al2O3
5
10
20
2.5
TIP
5
10
20


#### 2.2.3. Preparation of La Metal Loaded TiO2/Al2O3

Lanthanum(III) nitrate hexahydrate, La(NO3)3·6H2O, was used as the source of the La(III) dopant. The detailed procedure for the preparation of 4 dopant concentrations (0.05, 0.1, 0.2, and 0.3 mole ratio of La to Ti) by the impregnation method is as follows. An appropriate amount of La(NO3)3·6H2O was dissolved in a small amount of distilled water. This solution was then added dropwise to 5 g of TiO2/Al2O3 (5 wt.% TiO2) with constant stirring, as shown in Table 3. The product was dried in an oven at 100°C for 24 h and was ground to a fine powder. Then, it was calcined at 550°C for 4 h in a muffle furnace.Table 3
Composition of different La-doped samples.
La : Ti mole ratio
wt.% loading
0.05
5
0.1
0.2
0.3


#### 2.2.4. Preparation of Ce-Metal Loaded TiO2/Al2O3

Ammonium cerium(IV) nitrate, (NH4)2Ce(NO3)6, was used as the source of the Ce(IV) dopant. The detailed procedure for the preparation of 4 dopant concentrations (0.05, 0.1, 0.2, and 0.3 mole ratio of Ce to Ti) by the impregnation method is as follows. The appropriate amount of (NH4)2Ce(NO3)6 was dissolved in a small amount of distilled water. This was then added dropwise to 5 g of TiO2/Al2O3 (5 wt.% TiO2) with constant stirring, as shown in Table 4. The product was dried in an oven at 100°C for 24 h and was ground to fine powder. Then, it was calcined at 550°C for 4 h in a muffle furnace.Table 4
Composition of different Ce-doped samples.
Ce : Ti mole ratio
wt.% loading
0.05
5
0.1
0.2
0.3


### 2.3. Characterization Techniques and Control Test

The synthesized samples were evaluated and characterized by determining photocatalytic activity, particle size, and phase using XRD, UV-Vis, FT-IR, SEM, and EDX. Experimental details are as follows.


#### 2.3.1. X-Ray Powder Diffraction (XRD) Analysis

The crystalline phase and crystallite size of all catalyst nanoparticle samples were analyzed by X-ray powder diffraction (XRD) using a Rigaku X-ray diffractometer system equipped with a RINT 2000 wide angle Goniometer and Cu Kα radiation (λ = 0.15478 nm) at a power of 40 kV × 30 mA. The intensity data were collected at room temperature over a range of 2θ from 10 to 80°.


#### 2.3.2. Ultraviolet-Visible (UV-Vis) Spectroscopy

The concentration of the dye was followed up using UV-Vis spectrophotometer (Thermo Fisher Scientific Evolution 300).


#### 2.3.3. Fourier Transform Infrared (FT-IR) Spectroscopy

To study the surface chemical structures of all catalyst nanoparticle samples, Fourier transform infrared (FT-IR) spectra were recorded on a PerkinElmer FT-IR instrument 100 series.


#### 2.3.4. Scanning Electron Microscopy (SEM) and Energy Dispersive X-Ray (EDX) Spectroscopy

Surface morphologies and shapes of all catalyst nanoparticle samples were examined via a field-emission scanning electron microscope (SEM), which was obtained using JEOL JSM-7600F. This system was combined with energy dispersive X-ray spectroscopy for composition and elemental analysis.


### 2.4. Photocatalytic Degradation of Methyl Orange

#### 2.4.1. The Experiment for Photocatalytic Degradation of Methyl Orange

The photocatalytic activity of each prepared sample was evaluated by degradation of a pollutant in water. Methyl orange (MO), a common textile dye, was used as the model pollutant. The activity of the photocatalyst was tested by analyzing the decomposition of MO under UV irradiation. The MO solutions varied in concentration from 1 to 20 ppm and were prepared by dissolving MO powder in distilled water: 250 mL of 1 ppm MO solution was added to a Pyrex beaker (600 mL) and 0.5 g of TiO2/SiO2, TiO2/Al2O3, La-TiO2/Al2O3, or Ce-TiO2/Al2O3 was added to the solution. The suspension was magnetically stirred in the dark for various time intervals. An 8 W Philip’s lamp was used as the UV source at a fixed distance of 25 cm from the top of the magnetic stir bar. All components of the experimental set-up were located inside a box, as shown in Figure 1. A 10 mL sample was taken from the beaker at various time intervals, and the photocatalyst was separated from the solution by filtration. Absorbance measurements were also recorded in the range of 200–600 nm using UV-Vis spectrophotometer.Figure 1
Experimental set-up for the photocatalytic reaction.The concentration of MO solutions was determined by measuring the absorbance at approximately 465 nm using UV-Vis spectrophotometer (Thermo Fisher Scientific Evolution 300, USA).


## 2.1. Materials

All chemicals used in the preparation of TiO2/SiO2, TiO2/Al2O3, La-TiO2/Al2O3, and Ce-TiO2/Al2O3 nanoparticles were analytical grade reagents. The following high purity raw materials were used:(i)
Titanium(IV) oxide, anatase, 325 mesh, ≥99% metals basis, TiO2, Sigma-Aldrich Laboratories Supplies [Canada].
(ii)
Titanium(IV) isopropoxide, 98%, C12H28O4Ti, ACROS Organics.
(iii)
Titanium tetrachloride, TiCl4, Fluka AG Laboratories Supplies.
(iv)
Aluminum oxide, Al2O3, Fluka Laboratories Supplies [Switzerland].
(v)
Silica precipitated, SiO2, BDH Laboratories Supplies [Poole, England].
(vi)
Lanthanum(III) nitrate hexahydrate, La(NO3)3·6H2O, 99.999%, ACROS Organics Laboratories Supplies [New Jersey, USA].
(vii)
Ammonium cerium(IV) nitrate, 99%, H8CeN8O18, ACROS Organics Laboratories Supplies [New Jersey, USA].
(viii)
Methyl orange indicator, Pacegrove Limited Laboratories Supplies [UK].


## 2.2. Procedure and Apparatus

The loading of titanium tetra chloride (TiCl4) or titanium isopropoxide (TIP) into silica (SiO2) or aluminum oxide (Al2O3) was performed by the impregnation method (Img).


### 2.2.1. Preparation of TiO2/SiO2

Five grams of silica was mixed with a certain amount of titanium isopropoxide (TIP) or titanium tetra chloride (TiCl4). Then, a minimal amount of distilled water was added dropwise to the mixture, under vigorous stirring, to obtain 2.5, 5, 10, and 20 wt.% TiO2, as shown in Table 1. The formed paste was completely mixed to obtain a homogeneous mixture, and it was then dried in an oven at 100°C for 24 h. The resultant powder was ground using a mortar and pestle, followed by calcination at 550°C for 4 h in open air atmosphere.Table 1
Compositions of different TiO2/SiO2 samples.
Concentration of TiO2 (wt.%) in TiO2/SiO2
Source of titanium
Support type
2.5
TiCl4
SiO2
5
10
20
2.5
TIP
5
10
20


### 2.2.2. Preparation of TiO2/Al2O3

Five grams of aluminum oxide (Al2O3) was mixed with a certain amount of titanium isopropoxide (TIP) or titanium tetra chloride (TiCl4). Then, a minimal amount of distilled water was added dropwise to the mixture, under vigorous stirring, to obtain 2.5, 5, 10, and 20 wt.% TiO2, as shown in Table 2. The formed paste was completely mixed to obtain a homogeneous mixture, which was then dried in an oven at 100°C for 24 h. The powder was ground using a mortar and pestle, followed by calcination at 550°C for 4 h.Table 2
Compositions of different TiO2/Al2O3 samples.
Concentration of TiO2 (wt.%) in TiO2/Al2O3
Source of titanium
Support type
2.5
TiCl4
Al2O3
5
10
20
2.5
TIP
5
10
20


### 2.2.3. Preparation of La Metal Loaded TiO2/Al2O3

Lanthanum(III) nitrate hexahydrate, La(NO3)3·6H2O, was used as the source of the La(III) dopant. The detailed procedure for the preparation of 4 dopant concentrations (0.05, 0.1, 0.2, and 0.3 mole ratio of La to Ti) by the impregnation method is as follows. An appropriate amount of La(NO3)3·6H2O was dissolved in a small amount of distilled water. This solution was then added dropwise to 5 g of TiO2/Al2O3 (5 wt.% TiO2) with constant stirring, as shown in Table 3. The product was dried in an oven at 100°C for 24 h and was ground to a fine powder. Then, it was calcined at 550°C for 4 h in a muffle furnace.Table 3
Composition of different La-doped samples.
La : Ti mole ratio
wt.% loading
0.05
5
0.1
0.2
0.3


### 2.2.4. Preparation of Ce-Metal Loaded TiO2/Al2O3

Ammonium cerium(IV) nitrate, (NH4)2Ce(NO3)6, was used as the source of the Ce(IV) dopant. The detailed procedure for the preparation of 4 dopant concentrations (0.05, 0.1, 0.2, and 0.3 mole ratio of Ce to Ti) by the impregnation method is as follows. The appropriate amount of (NH4)2Ce(NO3)6 was dissolved in a small amount of distilled water. This was then added dropwise to 5 g of TiO2/Al2O3 (5 wt.% TiO2) with constant stirring, as shown in Table 4. The product was dried in an oven at 100°C for 24 h and was ground to fine powder. Then, it was calcined at 550°C for 4 h in a muffle furnace.Table 4
Composition of different Ce-doped samples.
Ce : Ti mole ratio
wt.% loading
0.05
5
0.1
0.2
0.3


## 2.2.1. Preparation of TiO2/SiO2

Five grams of silica was mixed with a certain amount of titanium isopropoxide (TIP) or titanium tetra chloride (TiCl4). Then, a minimal amount of distilled water was added dropwise to the mixture, under vigorous stirring, to obtain 2.5, 5, 10, and 20 wt.% TiO2, as shown in Table 1. The formed paste was completely mixed to obtain a homogeneous mixture, and it was then dried in an oven at 100°C for 24 h. The resultant powder was ground using a mortar and pestle, followed by calcination at 550°C for 4 h in open air atmosphere.Table 1
Compositions of different TiO2/SiO2 samples.
Concentration of TiO2 (wt.%) in TiO2/SiO2
Source of titanium
Support type
2.5
TiCl4
SiO2
5
10
20
2.5
TIP
5
10
20


## 2.2.2. Preparation of TiO2/Al2O3

Five grams of aluminum oxide (Al2O3) was mixed with a certain amount of titanium isopropoxide (TIP) or titanium tetra chloride (TiCl4). Then, a minimal amount of distilled water was added dropwise to the mixture, under vigorous stirring, to obtain 2.5, 5, 10, and 20 wt.% TiO2, as shown in Table 2. The formed paste was completely mixed to obtain a homogeneous mixture, which was then dried in an oven at 100°C for 24 h. The powder was ground using a mortar and pestle, followed by calcination at 550°C for 4 h.Table 2
Compositions of different TiO2/Al2O3 samples.
Concentration of TiO2 (wt.%) in TiO2/Al2O3
Source of titanium
Support type
2.5
TiCl4
Al2O3
5
10
20
2.5
TIP
5
10
20


## 2.2.3. Preparation of La Metal Loaded TiO2/Al2O3

Lanthanum(III) nitrate hexahydrate, La(NO3)3·6H2O, was used as the source of the La(III) dopant. The detailed procedure for the preparation of 4 dopant concentrations (0.05, 0.1, 0.2, and 0.3 mole ratio of La to Ti) by the impregnation method is as follows. An appropriate amount of La(NO3)3·6H2O was dissolved in a small amount of distilled water. This solution was then added dropwise to 5 g of TiO2/Al2O3 (5 wt.% TiO2) with constant stirring, as shown in Table 3. The product was dried in an oven at 100°C for 24 h and was ground to a fine powder. Then, it was calcined at 550°C for 4 h in a muffle furnace.Table 3
Composition of different La-doped samples.
La : Ti mole ratio
wt.% loading
0.05
5
0.1
0.2
0.3


## 2.2.4. Preparation of Ce-Metal Loaded TiO2/Al2O3

Ammonium cerium(IV) nitrate, (NH4)2Ce(NO3)6, was used as the source of the Ce(IV) dopant. The detailed procedure for the preparation of 4 dopant concentrations (0.05, 0.1, 0.2, and 0.3 mole ratio of Ce to Ti) by the impregnation method is as follows. The appropriate amount of (NH4)2Ce(NO3)6 was dissolved in a small amount of distilled water. This was then added dropwise to 5 g of TiO2/Al2O3 (5 wt.% TiO2) with constant stirring, as shown in Table 4. The product was dried in an oven at 100°C for 24 h and was ground to fine powder. Then, it was calcined at 550°C for 4 h in a muffle furnace.Table 4
Composition of different Ce-doped samples.
Ce : Ti mole ratio
wt.% loading
0.05
5
0.1
0.2
0.3


## 2.3. Characterization Techniques and Control Test

The synthesized samples were evaluated and characterized by determining photocatalytic activity, particle size, and phase using XRD, UV-Vis, FT-IR, SEM, and EDX. Experimental details are as follows.


### 2.3.1. X-Ray Powder Diffraction (XRD) Analysis

The crystalline phase and crystallite size of all catalyst nanoparticle samples were analyzed by X-ray powder diffraction (XRD) using a Rigaku X-ray diffractometer system equipped with a RINT 2000 wide angle Goniometer and Cu Kα radiation (λ = 0.15478 nm) at a power of 40 kV × 30 mA. The intensity data were collected at room temperature over a range of 2θ from 10 to 80°.


### 2.3.2. Ultraviolet-Visible (UV-Vis) Spectroscopy

The concentration of the dye was followed up using UV-Vis spectrophotometer (Thermo Fisher Scientific Evolution 300).


### 2.3.3. Fourier Transform Infrared (FT-IR) Spectroscopy

To study the surface chemical structures of all catalyst nanoparticle samples, Fourier transform infrared (FT-IR) spectra were recorded on a PerkinElmer FT-IR instrument 100 series.


### 2.3.4. Scanning Electron Microscopy (SEM) and Energy Dispersive X-Ray (EDX) Spectroscopy

Surface morphologies and shapes of all catalyst nanoparticle samples were examined via a field-emission scanning electron microscope (SEM), which was obtained using JEOL JSM-7600F. This system was combined with energy dispersive X-ray spectroscopy for composition and elemental analysis.


## 2.3.1. X-Ray Powder Diffraction (XRD) Analysis

The crystalline phase and crystallite size of all catalyst nanoparticle samples were analyzed by X-ray powder diffraction (XRD) using a Rigaku X-ray diffractometer system equipped with a RINT 2000 wide angle Goniometer and Cu Kα radiation (λ = 0.15478 nm) at a power of 40 kV × 30 mA. The intensity data were collected at room temperature over a range of 2θ from 10 to 80°.


## 2.3.2. Ultraviolet-Visible (UV-Vis) Spectroscopy

The concentration of the dye was followed up using UV-Vis spectrophotometer (Thermo Fisher Scientific Evolution 300).


## 2.3.3. Fourier Transform Infrared (FT-IR) Spectroscopy

To study the surface chemical structures of all catalyst nanoparticle samples, Fourier transform infrared (FT-IR) spectra were recorded on a PerkinElmer FT-IR instrument 100 series.


## 2.3.4. Scanning Electron Microscopy (SEM) and Energy Dispersive X-Ray (EDX) Spectroscopy

Surface morphologies and shapes of all catalyst nanoparticle samples were examined via a field-emission scanning electron microscope (SEM), which was obtained using JEOL JSM-7600F. This system was combined with energy dispersive X-ray spectroscopy for composition and elemental analysis.


## 2.4. Photocatalytic Degradation of Methyl Orange

### 2.4.1. The Experiment for Photocatalytic Degradation of Methyl Orange

The photocatalytic activity of each prepared sample was evaluated by degradation of a pollutant in water. Methyl orange (MO), a common textile dye, was used as the model pollutant. The activity of the photocatalyst was tested by analyzing the decomposition of MO under UV irradiation. The MO solutions varied in concentration from 1 to 20 ppm and were prepared by dissolving MO powder in distilled water: 250 mL of 1 ppm MO solution was added to a Pyrex beaker (600 mL) and 0.5 g of TiO2/SiO2, TiO2/Al2O3, La-TiO2/Al2O3, or Ce-TiO2/Al2O3 was added to the solution. The suspension was magnetically stirred in the dark for various time intervals. An 8 W Philip’s lamp was used as the UV source at a fixed distance of 25 cm from the top of the magnetic stir bar. All components of the experimental set-up were located inside a box, as shown in Figure 1. A 10 mL sample was taken from the beaker at various time intervals, and the photocatalyst was separated from the solution by filtration. Absorbance measurements were also recorded in the range of 200–600 nm using UV-Vis spectrophotometer.Figure 1
Experimental set-up for the photocatalytic reaction.The concentration of MO solutions was determined by measuring the absorbance at approximately 465 nm using UV-Vis spectrophotometer (Thermo Fisher Scientific Evolution 300, USA).


## 2.4.1. The Experiment for Photocatalytic Degradation of Methyl Orange

The photocatalytic activity of each prepared sample was evaluated by degradation of a pollutant in water. Methyl orange (MO), a common textile dye, was used as the model pollutant. The activity of the photocatalyst was tested by analyzing the decomposition of MO under UV irradiation. The MO solutions varied in concentration from 1 to 20 ppm and were prepared by dissolving MO powder in distilled water: 250 mL of 1 ppm MO solution was added to a Pyrex beaker (600 mL) and 0.5 g of TiO2/SiO2, TiO2/Al2O3, La-TiO2/Al2O3, or Ce-TiO2/Al2O3 was added to the solution. The suspension was magnetically stirred in the dark for various time intervals. An 8 W Philip’s lamp was used as the UV source at a fixed distance of 25 cm from the top of the magnetic stir bar. All components of the experimental set-up were located inside a box, as shown in Figure 1. A 10 mL sample was taken from the beaker at various time intervals, and the photocatalyst was separated from the solution by filtration. Absorbance measurements were also recorded in the range of 200–600 nm using UV-Vis spectrophotometer.Figure 1
Experimental set-up for the photocatalytic reaction.The concentration of MO solutions was determined by measuring the absorbance at approximately 465 nm using UV-Vis spectrophotometer (Thermo Fisher Scientific Evolution 300, USA).


## 3. Results and Discussion

### 3.1. Characterization of Investigated Samples

For catalyst characterization, knowing the catalyst’s texture and phase, as well as its chemical composition, represents an essential minimum. XRD, FT-IR, SEM, EDX, and UV-Vis are basic methods that provide the required information.


#### 3.1.1. XRD Analysis

The XRD patterns of 5 wt.% loaded samples on Al2O3 only showed the crystalline of corundum phase of the support; there was no indication of any crystalline phase of TiO2. This could be explained by the low detection limit of XRD towards TiO2 or by TiO2 being well dispersed over Al2O3 support (Figure 2) [7, 8]. For high loading percent of TiO2 a small fraction of anatase form was detected (figures not given).Figure 2
XRD pattern of 5 wt.% TiO2/Al2O3 (using TIP as a source of TiO2) nominated with h
k
l values of planes.


#### 3.1.2. FT-IR Analysis

The FT-IR spectra of different doped and undoped samples are shown in Figures3–6. The FT-IR spectra of solids were recorded before and after the reaction. The vibrational mode of Ti–O and Al–O was clearly observed in all samples.Figure 3
FT-IR spectra of 5 wt.% TiO2/Al2O3 (a) before reaction and (b) after reaction (using TIP as a source of TiO2).Figure 4
FT-IR spectra of 0.05, 0.1, 0.2, and 0.3 mole ratio La-TiO2/Al2O3 (a) before reaction and (b) after reaction.Figure 5
FT-IR spectra of 0.05, 0.1, 0.2, and 0.3 mole ratio Ce-TiO2/Al2O3 (a) before reaction and (b) after reaction.Figure 6
FT-IR spectra of La-doped and undoped samples.Doping with La or Ce did not change the Ti–O and Al–O bands; however, after the reaction of most samples, a slight change in the positions and the shapes of these peaks was observed. This could be explained by a physical change of the support after reacting.In Figure6, it can be observed that the lower absorption bands (326 and 418 cm−1), which are assigned to the M–O vibration (M = Ti, La, or Al) [9–12], are well separated in undoped samples; however, even with a doping level of 0.05 wt.%, only unresolved bands are observed.


#### 3.1.3. SEM Analysis of Samples

Figures7–11 show SEM images of different loaded samples on top of Al2O3 support. The shape of Al2O3 support was clearly observed in all samples. No aggregations of TiO2 were observed, as expected from XRD, which leads to the conclusion that TiO2 is well dispersed over Al2O3 support and indicates its presence in nanoscale [13].Figure 7
SEM image of 0.05 mole ratio La-loaded on TiO2/Al2O3.Figure 8
SEM image of 0.3 mole ratio La-loaded on TiO2/Al2O3.Figure 9
SEM image of 0.05 mole ratio Ce-loaded on TiO2/Al2O3.Figure 10
SEM image of 0.3 mole ratio Ce-loaded on TiO2/Al2O3.Figure 11
SEM image of 5 wt.% TiO2/Al2O3 (using TIP as a source of TiO2).


#### 3.1.4. EDX Analysis of Samples

Table5 provides the experimental EDX analysis of some selected samples compared to the theoretical wt.% of same samples.Table 5
EDX analysis of selected samples.
wt.%
Al2O3%
TiO2%
La2O3%
CeO2%
La/TIP (0.05)
99.21061
0.789391
0
0
La/TIP (0.3)
98.41669
1.583311
0
0
Ce/TIP (0.05)
98.98106
1.018944
0
0
Ce/TIP (0.3)
98.18298
0
0
1.817018
Ce/TIP (0.3)
97.56178
0
0
2.438221
Ce/TIP (0.3)
99.25471
0.745288
0
0
Ce/TIP (0.3)
87.76509
0
0
12.23491
TIP/Al2O3 (5%)
97.57552
2.424481
0
0Tables5–7 present the data analysis for all investigated samples obtained by calculating the theoretical and the actual wt.% loading, in addition to determining the excess surface concentration of each component. The excess surface concentration is defined as follows:(1)
Excess surface concentration
=
wt
.
%
2
-
wt
.
%
1
wt
.
%
1
×
100
,where wt
.
%
1 is the theoretical weight percentage of loading and wt
.
%
2 is the surface weight percentage of the metal oxide measured by EDX analysis [13].Table 6
Theoretical wt.% of loading of different samples.
Theoretical (wt.%)
Al2O3%
TiO2%
La2O3%
CeO2%
La/TIP (0.05)
95
4.537242
0.462758
0
La/TIP (0.3)
95
3.101841
1.898159
0
Ce/TIP (0.05)
95
4.513598
0
0.486402
Ce/TIP (0.3)
95
4.513598
0
0.486402
Ce/TIP (0.3)
95
4.513598
0
0.486402
Ce/TIP (0.3)
95
4.513598
0
0.486402
Ce/TIP (0.3)
95
4.513598
0
0.486402
TIP/Al2O3 (5%)
95
5
0
0Table 7
Excess surface concentrations of investigated samples.
wt.%
Surface excess concentration
Al2O3%
TiO2%
La2O3%
CeO2%
La/TIP (0.05)
4.43222
−82.602
−100
0
La/TIP (0.3)
3.596515
−48.9558
−100
0
Ce/TIP (0.05)
4.190585
−77.425
−100
−100
Ce/TIP (0.3)
3.350508
−100
−100
273.5633
Ce/TIP (0.3)
2.696609
−100
−100
401.2774
Ce/TIP (0.3)
4.478644
−83.4879
−100
−100
Ce/TIP (0.3)
−7.61569
−100
−100
2415.392
TIP/Al2O3 (5%)
2.711073
−51.5104
0
0From these tables it could be observed that the presence of La2O3, as a dopant, facilitated the diffusion of TiO2 into the alumina support, as reflected by the remarkably small amount of TiO2 when compared to values for the theoretical load and those observed for undoped samples. The facile diffusion of TiO2 into alumina appeared to exist even in undoped samples. It is suggested that approximately half of TiO2 diffused into undoped samples when compared to the theoretical loading values. The introduction of La2O3 as a dopant with a 0.05 Ti : La mole ratio resulted in a dramatic increase (30%) of TiO2 diffusion. From the data below, we can conclude that there are two types of active sites: one is predominantly a surface site associated with TiO2, and the other is bulk or diffused TiO2. From Figure 16, which indicates the catalytic activity of La-doped and undoped samples, we can observe that the sample with a 0.05 Ti : La mole ratio showed the highest catalytic activity of all samples. Increasing the amount of the dopant, however, did not increase the catalytic activity but decreased it when compared to the undoped samples. This behavior could be explained when we examined the EDX data. This analysis showed that the 0.3 Ti : La mole ratio sample reduced the amount of diffused TiO2 by approximately 30% when compared to the 0.05 sample. The direct conclusion based on the above behavior is that the diffused TiO2 catalytic active site is much higher than that of surface one. The decrease in diffusion of TiO2 observed upon increasing the amount of dopant may be understood as a competition between the affinity of TiO2 for La2O3 and that for alumina. This competition could be further influenced by the intermolecular interactions between molecules of La2O3, which could be favored at high levels of dopant (0.3 mole ratio).This possible interaction was not observed with XRD, due to the detection limit; however, it is well observed from FT-IR spectra in Figure6.In addition, we can discuss the observation of M–O bands in the FT-IR spectra of doped samples (Figure6), which could also result from the dopant facilitating the diffusion of TiO2 into alumina. Hence, the presence of multiple metal-oxygen vibrational bands in the same vicinity could be evidence of a possible interaction between them.Returning to the CeO2-doped samples, the EDX analysis showed nearly the same enhancement of TiO2 diffusion at the low doping concentration (0.05 mole ratio), which was not reflected in its catalytic activity. Moreover, by increasing the dopant level (0.3 mole ratio) and through a different spot analysis, CeO2 seemed to aggregate on the surface. This could be explained as the affinity of CeO2 towards alumina being higher than its affinity for TiO2, which is in contrast to La2O3, which first interacts with TiO2.


### 3.2. Effect of Precursors and Support Type on Catalytic Activity

Figures12–15 showed the photocatalytic activity for differently loaded samples of TiO2/Al2O3 and TiO2/SiO2. From these curves, we could see that the titanium isopropoxide precursor produced TiO2 evenly dispersed across the surfaces of either Al2O3 or SiO2 and yielded samples with high photocatalytic activity. It was also observed that the photocatalytic activity of Al2O3 support was much higher than that of SiO2.Figure 12
Curve of dye concentration (MO) divided by % TiO2/Al2O3 (using TIP as a source of TiO2) versus time during the photocatalytic degradation experiment.Figure 13
Curve of dye concentration (MO) divided by % TiO2/SiO2 (using TIP as a source of TiO2) versus time during the photocatalytic degradation experiment.Figure 14
Curve of dye concentration (MO) divided by % TiO2/Al2O3 (using TiCl4 as a source of TiO2) versus time during the photocatalytic degradation experiment.Figure 15
Curve of dye concentration (MO) divided by % TiO2/SiO2 (using TiCl4 as a source of TiO2) versus time during the photocatalytic degradation experiment.Figure 16
The effect of different doping levels with La 0.05, 0.1, 0.2, and 0.3 mole ratio compared to 5 wt.% TiO2/Al2O3 (using TIP as a source of TiO2).For Al2O3 support it could be concluded that the 5 wt.% loading was the optimum loading with respect to catalytic activity and the decomposition rate of the organic dye.


### 3.3. Effect of Doping with La and Ce

Figure16 showed the effect of different samples doped with La (0.05, 0.1, 0.2, and 0.3 mole ratio), compared to undoped samples. From this figure, it could be observed that as doping decreases, the catalytic activity increases. Photocatalysis reaches a maximum at a doping of 0.05 mole ratio La, which is greater than the activity of the undoped sample.Moreover, Figure17 showed the effect of different doping levels using Ce at the same concentrations. The same trend could be observed for Ce-doped samples as was noted for La-doped samples; however, the doping with Ce leads to a remarkable decrease in catalytic activity compared with the undoped samples.Figure 17
The effect of different doping levels with Ce 0.05, 0.1, 0.2, and 0.3 mole ratio compared to 5 wt.% TiO2/Al2O3 (using TIP as a source of TiO2).


## 3.1. Characterization of Investigated Samples

For catalyst characterization, knowing the catalyst’s texture and phase, as well as its chemical composition, represents an essential minimum. XRD, FT-IR, SEM, EDX, and UV-Vis are basic methods that provide the required information.


### 3.1.1. XRD Analysis

The XRD patterns of 5 wt.% loaded samples on Al2O3 only showed the crystalline of corundum phase of the support; there was no indication of any crystalline phase of TiO2. This could be explained by the low detection limit of XRD towards TiO2 or by TiO2 being well dispersed over Al2O3 support (Figure 2) [7, 8]. For high loading percent of TiO2 a small fraction of anatase form was detected (figures not given).Figure 2
XRD pattern of 5 wt.% TiO2/Al2O3 (using TIP as a source of TiO2) nominated with h
k
l values of planes.


### 3.1.2. FT-IR Analysis

The FT-IR spectra of different doped and undoped samples are shown in Figures3–6. The FT-IR spectra of solids were recorded before and after the reaction. The vibrational mode of Ti–O and Al–O was clearly observed in all samples.Figure 3
FT-IR spectra of 5 wt.% TiO2/Al2O3 (a) before reaction and (b) after reaction (using TIP as a source of TiO2).Figure 4
FT-IR spectra of 0.05, 0.1, 0.2, and 0.3 mole ratio La-TiO2/Al2O3 (a) before reaction and (b) after reaction.Figure 5
FT-IR spectra of 0.05, 0.1, 0.2, and 0.3 mole ratio Ce-TiO2/Al2O3 (a) before reaction and (b) after reaction.Figure 6
FT-IR spectra of La-doped and undoped samples.Doping with La or Ce did not change the Ti–O and Al–O bands; however, after the reaction of most samples, a slight change in the positions and the shapes of these peaks was observed. This could be explained by a physical change of the support after reacting.In Figure6, it can be observed that the lower absorption bands (326 and 418 cm−1), which are assigned to the M–O vibration (M = Ti, La, or Al) [9–12], are well separated in undoped samples; however, even with a doping level of 0.05 wt.%, only unresolved bands are observed.


### 3.1.3. SEM Analysis of Samples

Figures7–11 show SEM images of different loaded samples on top of Al2O3 support. The shape of Al2O3 support was clearly observed in all samples. No aggregations of TiO2 were observed, as expected from XRD, which leads to the conclusion that TiO2 is well dispersed over Al2O3 support and indicates its presence in nanoscale [13].Figure 7
SEM image of 0.05 mole ratio La-loaded on TiO2/Al2O3.Figure 8
SEM image of 0.3 mole ratio La-loaded on TiO2/Al2O3.Figure 9
SEM image of 0.05 mole ratio Ce-loaded on TiO2/Al2O3.Figure 10
SEM image of 0.3 mole ratio Ce-loaded on TiO2/Al2O3.Figure 11
SEM image of 5 wt.% TiO2/Al2O3 (using TIP as a source of TiO2).


### 3.1.4. EDX Analysis of Samples

Table5 provides the experimental EDX analysis of some selected samples compared to the theoretical wt.% of same samples.Table 5
EDX analysis of selected samples.
wt.%
Al2O3%
TiO2%
La2O3%
CeO2%
La/TIP (0.05)
99.21061
0.789391
0
0
La/TIP (0.3)
98.41669
1.583311
0
0
Ce/TIP (0.05)
98.98106
1.018944
0
0
Ce/TIP (0.3)
98.18298
0
0
1.817018
Ce/TIP (0.3)
97.56178
0
0
2.438221
Ce/TIP (0.3)
99.25471
0.745288
0
0
Ce/TIP (0.3)
87.76509
0
0
12.23491
TIP/Al2O3 (5%)
97.57552
2.424481
0
0Tables5–7 present the data analysis for all investigated samples obtained by calculating the theoretical and the actual wt.% loading, in addition to determining the excess surface concentration of each component. The excess surface concentration is defined as follows:(1)
Excess surface concentration
=
wt
.
%
2
-
wt
.
%
1
wt
.
%
1
×
100
,where wt
.
%
1 is the theoretical weight percentage of loading and wt
.
%
2 is the surface weight percentage of the metal oxide measured by EDX analysis [13].Table 6
Theoretical wt.% of loading of different samples.
Theoretical (wt.%)
Al2O3%
TiO2%
La2O3%
CeO2%
La/TIP (0.05)
95
4.537242
0.462758
0
La/TIP (0.3)
95
3.101841
1.898159
0
Ce/TIP (0.05)
95
4.513598
0
0.486402
Ce/TIP (0.3)
95
4.513598
0
0.486402
Ce/TIP (0.3)
95
4.513598
0
0.486402
Ce/TIP (0.3)
95
4.513598
0
0.486402
Ce/TIP (0.3)
95
4.513598
0
0.486402
TIP/Al2O3 (5%)
95
5
0
0Table 7
Excess surface concentrations of investigated samples.
wt.%
Surface excess concentration
Al2O3%
TiO2%
La2O3%
CeO2%
La/TIP (0.05)
4.43222
−82.602
−100
0
La/TIP (0.3)
3.596515
−48.9558
−100
0
Ce/TIP (0.05)
4.190585
−77.425
−100
−100
Ce/TIP (0.3)
3.350508
−100
−100
273.5633
Ce/TIP (0.3)
2.696609
−100
−100
401.2774
Ce/TIP (0.3)
4.478644
−83.4879
−100
−100
Ce/TIP (0.3)
−7.61569
−100
−100
2415.392
TIP/Al2O3 (5%)
2.711073
−51.5104
0
0From these tables it could be observed that the presence of La2O3, as a dopant, facilitated the diffusion of TiO2 into the alumina support, as reflected by the remarkably small amount of TiO2 when compared to values for the theoretical load and those observed for undoped samples. The facile diffusion of TiO2 into alumina appeared to exist even in undoped samples. It is suggested that approximately half of TiO2 diffused into undoped samples when compared to the theoretical loading values. The introduction of La2O3 as a dopant with a 0.05 Ti : La mole ratio resulted in a dramatic increase (30%) of TiO2 diffusion. From the data below, we can conclude that there are two types of active sites: one is predominantly a surface site associated with TiO2, and the other is bulk or diffused TiO2. From Figure 16, which indicates the catalytic activity of La-doped and undoped samples, we can observe that the sample with a 0.05 Ti : La mole ratio showed the highest catalytic activity of all samples. Increasing the amount of the dopant, however, did not increase the catalytic activity but decreased it when compared to the undoped samples. This behavior could be explained when we examined the EDX data. This analysis showed that the 0.3 Ti : La mole ratio sample reduced the amount of diffused TiO2 by approximately 30% when compared to the 0.05 sample. The direct conclusion based on the above behavior is that the diffused TiO2 catalytic active site is much higher than that of surface one. The decrease in diffusion of TiO2 observed upon increasing the amount of dopant may be understood as a competition between the affinity of TiO2 for La2O3 and that for alumina. This competition could be further influenced by the intermolecular interactions between molecules of La2O3, which could be favored at high levels of dopant (0.3 mole ratio).This possible interaction was not observed with XRD, due to the detection limit; however, it is well observed from FT-IR spectra in Figure6.In addition, we can discuss the observation of M–O bands in the FT-IR spectra of doped samples (Figure6), which could also result from the dopant facilitating the diffusion of TiO2 into alumina. Hence, the presence of multiple metal-oxygen vibrational bands in the same vicinity could be evidence of a possible interaction between them.Returning to the CeO2-doped samples, the EDX analysis showed nearly the same enhancement of TiO2 diffusion at the low doping concentration (0.05 mole ratio), which was not reflected in its catalytic activity. Moreover, by increasing the dopant level (0.3 mole ratio) and through a different spot analysis, CeO2 seemed to aggregate on the surface. This could be explained as the affinity of CeO2 towards alumina being higher than its affinity for TiO2, which is in contrast to La2O3, which first interacts with TiO2.


## 3.1.1. XRD Analysis

The XRD patterns of 5 wt.% loaded samples on Al2O3 only showed the crystalline of corundum phase of the support; there was no indication of any crystalline phase of TiO2. This could be explained by the low detection limit of XRD towards TiO2 or by TiO2 being well dispersed over Al2O3 support (Figure 2) [7, 8]. For high loading percent of TiO2 a small fraction of anatase form was detected (figures not given).Figure 2
XRD pattern of 5 wt.% TiO2/Al2O3 (using TIP as a source of TiO2) nominated with h
k
l values of planes.


## 3.1.2. FT-IR Analysis

The FT-IR spectra of different doped and undoped samples are shown in Figures3–6. The FT-IR spectra of solids were recorded before and after the reaction. The vibrational mode of Ti–O and Al–O was clearly observed in all samples.Figure 3
FT-IR spectra of 5 wt.% TiO2/Al2O3 (a) before reaction and (b) after reaction (using TIP as a source of TiO2).Figure 4
FT-IR spectra of 0.05, 0.1, 0.2, and 0.3 mole ratio La-TiO2/Al2O3 (a) before reaction and (b) after reaction.Figure 5
FT-IR spectra of 0.05, 0.1, 0.2, and 0.3 mole ratio Ce-TiO2/Al2O3 (a) before reaction and (b) after reaction.Figure 6
FT-IR spectra of La-doped and undoped samples.Doping with La or Ce did not change the Ti–O and Al–O bands; however, after the reaction of most samples, a slight change in the positions and the shapes of these peaks was observed. This could be explained by a physical change of the support after reacting.In Figure6, it can be observed that the lower absorption bands (326 and 418 cm−1), which are assigned to the M–O vibration (M = Ti, La, or Al) [9–12], are well separated in undoped samples; however, even with a doping level of 0.05 wt.%, only unresolved bands are observed.


## 3.1.3. SEM Analysis of Samples

Figures7–11 show SEM images of different loaded samples on top of Al2O3 support. The shape of Al2O3 support was clearly observed in all samples. No aggregations of TiO2 were observed, as expected from XRD, which leads to the conclusion that TiO2 is well dispersed over Al2O3 support and indicates its presence in nanoscale [13].Figure 7
SEM image of 0.05 mole ratio La-loaded on TiO2/Al2O3.Figure 8
SEM image of 0.3 mole ratio La-loaded on TiO2/Al2O3.Figure 9
SEM image of 0.05 mole ratio Ce-loaded on TiO2/Al2O3.Figure 10
SEM image of 0.3 mole ratio Ce-loaded on TiO2/Al2O3.Figure 11
SEM image of 5 wt.% TiO2/Al2O3 (using TIP as a source of TiO2).


## 3.1.4. EDX Analysis of Samples

Table5 provides the experimental EDX analysis of some selected samples compared to the theoretical wt.% of same samples.Table 5
EDX analysis of selected samples.
wt.%
Al2O3%
TiO2%
La2O3%
CeO2%
La/TIP (0.05)
99.21061
0.789391
0
0
La/TIP (0.3)
98.41669
1.583311
0
0
Ce/TIP (0.05)
98.98106
1.018944
0
0
Ce/TIP (0.3)
98.18298
0
0
1.817018
Ce/TIP (0.3)
97.56178
0
0
2.438221
Ce/TIP (0.3)
99.25471
0.745288
0
0
Ce/TIP (0.3)
87.76509
0
0
12.23491
TIP/Al2O3 (5%)
97.57552
2.424481
0
0Tables5–7 present the data analysis for all investigated samples obtained by calculating the theoretical and the actual wt.% loading, in addition to determining the excess surface concentration of each component. The excess surface concentration is defined as follows:(1)
Excess surface concentration
=
wt
.
%
2
-
wt
.
%
1
wt
.
%
1
×
100
,where wt
.
%
1 is the theoretical weight percentage of loading and wt
.
%
2 is the surface weight percentage of the metal oxide measured by EDX analysis [13].Table 6
Theoretical wt.% of loading of different samples.
Theoretical (wt.%)
Al2O3%
TiO2%
La2O3%
CeO2%
La/TIP (0.05)
95
4.537242
0.462758
0
La/TIP (0.3)
95
3.101841
1.898159
0
Ce/TIP (0.05)
95
4.513598
0
0.486402
Ce/TIP (0.3)
95
4.513598
0
0.486402
Ce/TIP (0.3)
95
4.513598
0
0.486402
Ce/TIP (0.3)
95
4.513598
0
0.486402
Ce/TIP (0.3)
95
4.513598
0
0.486402
TIP/Al2O3 (5%)
95
5
0
0Table 7
Excess surface concentrations of investigated samples.
wt.%
Surface excess concentration
Al2O3%
TiO2%
La2O3%
CeO2%
La/TIP (0.05)
4.43222
−82.602
−100
0
La/TIP (0.3)
3.596515
−48.9558
−100
0
Ce/TIP (0.05)
4.190585
−77.425
−100
−100
Ce/TIP (0.3)
3.350508
−100
−100
273.5633
Ce/TIP (0.3)
2.696609
−100
−100
401.2774
Ce/TIP (0.3)
4.478644
−83.4879
−100
−100
Ce/TIP (0.3)
−7.61569
−100
−100
2415.392
TIP/Al2O3 (5%)
2.711073
−51.5104
0
0From these tables it could be observed that the presence of La2O3, as a dopant, facilitated the diffusion of TiO2 into the alumina support, as reflected by the remarkably small amount of TiO2 when compared to values for the theoretical load and those observed for undoped samples. The facile diffusion of TiO2 into alumina appeared to exist even in undoped samples. It is suggested that approximately half of TiO2 diffused into undoped samples when compared to the theoretical loading values. The introduction of La2O3 as a dopant with a 0.05 Ti : La mole ratio resulted in a dramatic increase (30%) of TiO2 diffusion. From the data below, we can conclude that there are two types of active sites: one is predominantly a surface site associated with TiO2, and the other is bulk or diffused TiO2. From Figure 16, which indicates the catalytic activity of La-doped and undoped samples, we can observe that the sample with a 0.05 Ti : La mole ratio showed the highest catalytic activity of all samples. Increasing the amount of the dopant, however, did not increase the catalytic activity but decreased it when compared to the undoped samples. This behavior could be explained when we examined the EDX data. This analysis showed that the 0.3 Ti : La mole ratio sample reduced the amount of diffused TiO2 by approximately 30% when compared to the 0.05 sample. The direct conclusion based on the above behavior is that the diffused TiO2 catalytic active site is much higher than that of surface one. The decrease in diffusion of TiO2 observed upon increasing the amount of dopant may be understood as a competition between the affinity of TiO2 for La2O3 and that for alumina. This competition could be further influenced by the intermolecular interactions between molecules of La2O3, which could be favored at high levels of dopant (0.3 mole ratio).This possible interaction was not observed with XRD, due to the detection limit; however, it is well observed from FT-IR spectra in Figure6.In addition, we can discuss the observation of M–O bands in the FT-IR spectra of doped samples (Figure6), which could also result from the dopant facilitating the diffusion of TiO2 into alumina. Hence, the presence of multiple metal-oxygen vibrational bands in the same vicinity could be evidence of a possible interaction between them.Returning to the CeO2-doped samples, the EDX analysis showed nearly the same enhancement of TiO2 diffusion at the low doping concentration (0.05 mole ratio), which was not reflected in its catalytic activity. Moreover, by increasing the dopant level (0.3 mole ratio) and through a different spot analysis, CeO2 seemed to aggregate on the surface. This could be explained as the affinity of CeO2 towards alumina being higher than its affinity for TiO2, which is in contrast to La2O3, which first interacts with TiO2.


## 3.2. Effect of Precursors and Support Type on Catalytic Activity

Figures12–15 showed the photocatalytic activity for differently loaded samples of TiO2/Al2O3 and TiO2/SiO2. From these curves, we could see that the titanium isopropoxide precursor produced TiO2 evenly dispersed across the surfaces of either Al2O3 or SiO2 and yielded samples with high photocatalytic activity. It was also observed that the photocatalytic activity of Al2O3 support was much higher than that of SiO2.Figure 12
Curve of dye concentration (MO) divided by % TiO2/Al2O3 (using TIP as a source of TiO2) versus time during the photocatalytic degradation experiment.Figure 13
Curve of dye concentration (MO) divided by % TiO2/SiO2 (using TIP as a source of TiO2) versus time during the photocatalytic degradation experiment.Figure 14
Curve of dye concentration (MO) divided by % TiO2/Al2O3 (using TiCl4 as a source of TiO2) versus time during the photocatalytic degradation experiment.Figure 15
Curve of dye concentration (MO) divided by % TiO2/SiO2 (using TiCl4 as a source of TiO2) versus time during the photocatalytic degradation experiment.Figure 16
The effect of different doping levels with La 0.05, 0.1, 0.2, and 0.3 mole ratio compared to 5 wt.% TiO2/Al2O3 (using TIP as a source of TiO2).For Al2O3 support it could be concluded that the 5 wt.% loading was the optimum loading with respect to catalytic activity and the decomposition rate of the organic dye.


## 3.3. Effect of Doping with La and Ce

Figure16 showed the effect of different samples doped with La (0.05, 0.1, 0.2, and 0.3 mole ratio), compared to undoped samples. From this figure, it could be observed that as doping decreases, the catalytic activity increases. Photocatalysis reaches a maximum at a doping of 0.05 mole ratio La, which is greater than the activity of the undoped sample.Moreover, Figure17 showed the effect of different doping levels using Ce at the same concentrations. The same trend could be observed for Ce-doped samples as was noted for La-doped samples; however, the doping with Ce leads to a remarkable decrease in catalytic activity compared with the undoped samples.Figure 17
The effect of different doping levels with Ce 0.05, 0.1, 0.2, and 0.3 mole ratio compared to 5 wt.% TiO2/Al2O3 (using TIP as a source of TiO2).


## 4. Conclusions

From the above research, the following conclusions were drawn:(1)
Titania supported on silica or alumina could be used as a good photocatalyst for the degradation of organic dyes.
(2)
Titanium isopropoxide (TIP) was found to be more effective than titanium tetrachloride (TiCl4).
(3)
The optimum loading value was found to be 5 wt.% TiO2 which insures its presence in nanoscale.
(4)
The alumina support (corundum phase) was found to be more effective than that of amorphous silica.
(5)
In trying to increase catalytic activity by dopant inclusion of either La2O3 or CeO2, we determined that La2O3 enhances the catalytic activity more than CeO2.
(6)
The interactions between La2O3, TiO2, and alumina were correlated with catalytic activity.
(7)
The 0.05 mole ratio for the dopant was found to be the optimum value, above which the catalytic activity decreased.



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*Source: 1035402-2016-04-20.xml*