# Preparation and Application of Mesoporous Nanotitania Photocatalysts Using Different Templates and pH Media

Authors: S. M. Abdel-Azim; A. K. Aboul-Gheit; S. M. Ahmed; D. S. El-Desouki; M. S. A. Abdel-Mottaleb
Journal: International Journal of Photoenergy
 (2014)

---

## Abstract

Mesoporous nanotitania photocatalysts were prepared by sol-gel method in acidic or basic media. Three types of surfactants, namely, cetyltrimethylammonium bromide, sodium dodecylbenzenesulfonate, and nonylphenol ethoxylate, were used as templating agents. The effects of surfactant type and pH on the morphology, particle size, surface area, pore-size distribution, UV-Vis absorbance, and TiO2 phase transformation were traced by SEM, TEM, BET, and XRD. In absence of surfactants, XRD revealed 54.5% anatase at pH 3-4 and 97.0% at pH 7–9. In presence of surfactant, phase transformation of anatase has been significantly inhibited such that anatase amounts to 82–100% in acidic media. In basic media, the brookite phase appeared in low concentrations (8–15%) while rutile totally disappeared. The photocatalytic performance of the synthesized catalysts was tested via naphthalene degradation, which exhibited high activity in visible irradiation (>400 nm). The data obtained indicate that the surface area and pore volume of the current catalysts are the most effective factors for photocatalytic performance. Nevertheless, at the low pH (acidic) range, the CTAB templated catalyst gave the highest surface area (86.7 cm3/g), which is mainly assigned to acquiring the highest photocatalytic degradation of naphthalene (97% after 4 h irradiation time).


---

## Body

## 1. Introduction

The properties of nanocrystals depend not only on their chemical compositions, but also on their structures, phases, shapes, sizes, and dimensionality [1]. Since the discovery of photocatalysis, titanium oxide (TiO2) has attracted signification research attention due to its broad applications in the fields of water and air purification [2–4]. Also, TiO2 has versatile potential applications besides catalysis, such as in solar-energy conversion, lithium storage, and optoelectronic devices. Many studies have described the shape and size control of inorganic nanoparticles by using conventional synthesis methods such as the sol-gel method and hydrothermal method. The sol-gel method has many advantages over other methods mainly because of the following: good homogeneity, ease of composition control, low processing temperature, large area coatings, low equipment cost, and good optical properties [5]. Mesoporous TiO2 has better properties in many respects than ordinary TiO2 because of its high specific surface area, uniform pore diameter, potential role in enhancing the light absorbance, and the accessibility of reactants to the active catalytic sites [6]. Mesoporous TiO2 has been prepared as bulk powders and films [6, 7]. An interesting method to fabricate highly porous materials with desired pore structure and size for target specific applications is the use of amphiphilic organic molecules such as surfactants and block copolymers as pore directing agents in sol-gel methods [8]. Our motivation is to explore an effective technique to construct the oriented organization of nanoparticles, which is based on creating an interfacial interaction by chemical modification on the surfaces of nanoparticles (or micelle formation, that is, form colloidal-size cluster in solution called micelles which depend on surfactant concentration and salt concentration). Park et al. [9] have reported the preparation of mesoporous titania through a modified sol-gel process in presence of CTAB surfactant. Shalan et al. [10] synthesized anatase TiO2 nanorods with controlled size for dye-sensitized solar cells (DSSCs) via hydrothermal route at low hydrothermal temperature of 100°C for 24 h. A number of formation mechanism models have been proposed to explain the growth process of nanostructured materials from the inorganic precursor in the presence of surfactants self-assembles [11]. Transition metal oxides have been prepared in mesoporous forms using the amphiphilic surfactant templates such as triblock copolymers and ionic surfactants such as CTAB and neutral amines [7].Naphthalene (NP C10H8) is a polycyclic aromatic hydrocarbon (PAH), which is a widespread environmental contaminant because of its generation as a combustion byproduct and use as a pesticide and pesticide synthesis intermediate and as component of fuels such as JP-8 [12]. Since it is the most water-soluble PAH (solubility 25–30 mg L−1 at ambient temperature), it is the dominant one in water. It has been considered as possibly carcinogenic to humans and it has both acute and chronic effects on humans and animal health. So, removing of naphthalene from water is urgently needed and possible via many techniques. Remediation and treatment of water, soil, or wastewater from PAH include conventional methods as homogeneous methods, bioremediation [13], hydrogenation [14], and ozonation, [15] and heterogeneous methods, photocatalytic degradation, fenton heterogeneous catalytic system [16], and metal oxides [17]. Advanced oxidation processes (AOPs) [18] present many advantages which are faster and can be achieved under direct sunlight making it cheaper to operate than other techniques. The total destruction of naphthalene using metal oxides with various supporting materials was carried out [19, 20]. Photocatalytic oxidation of naphthalene solution using various kinds of industrial titanium dioxide powders having anatase and rutile structure was tested as photocatalysts by Ohno et al. [21].Other authors investigated changing the conditions they applied in preparing the nanocatalysts for use as active photocatalysts. In our work, we categorized the different types of surfactants to be used at different pH values (acidic and basic media). This scheme of work makes us able to illustrate a wide understanding of surface-active templates in nanophotocatalysts.Therefore, in this work, we modified the sol-gel method through using three types of surfactants (cationic, anionic, or nonionic) in acidic or basic media for controlling the phase structure, size, crystallinity, mesoporosity, and hence the light absorptivity in the visible range. The photocatalytic activity of the nanostructured mesoporous TiO2 catalyst has been tested in photodegradation of naphthalene as a water pollutant model compound.


## 2.  Experiment

### 2.1. Materials

In the current experiments, all chemicals were used as received. Titanium (IV) isopropoxide (TTIP) (97% Aldrich), isopropanol (i-PrOH, Fisher), acetic acid (Fisher), ammonium hydroxide, cetyltrimetylammonium bromide (CTAB), sodium dodecylbenzenesulfonate (DBS), nonylphenol ethoxylate (NPE), and deionized water were used to prepare the solutions in our experiments. Naphthalene (Panreac, 98%) was used as a pollutant, acetonitrile and deionized water were used as HPLC eluent.


### 2.2. Synthesis of the Current Titania Catalysts

Mesoporous nanocrystalline titania was prepared under controllable sol-gel process using titanium alkoxide in absence or presence of micellar surfactants as templating agents [22]. The molar ratio of surfactant/TTIP/i-PrOH/acetic acid or ammonium hydroxide was  : 4 : 45 : 6, where R is the surfactant concentration was which 0 or 1 at pH 3-4 in acetic acid or 8-9 in ammonia solution. Hydrolysis and polymerization took place in this mixture producing a transparent, homogeneous, and stable TiO2 sol. After gelation for 24 h, the gel was dried overnight at 80°C. The recovered powder was intermittently washed with deionized water and isopropanol five times followed by separation in a centrifuge under 10000 rpm to remove the surfactant. The resulted filtered cake was dried overnight at 100°C and then calcined at 550°C for 4 h to remove the remaining surfactant and consequently produce the desired TiO2 nanoparticles photocatalyst (Scheme 1). The nomenclature was designed according to the pH range and the used surfactant. Preparation catalysts in acidic and basic medium were as follows: (1) without surfactant: A and B, (2) in presence of surfactants, CTAB-A, DBS-A, and NPE-A, in acidic medium, and (3) CTAB-B, DBS-B, and NPE-B in basic medium.Scheme 1
Preparation of TiO2 photocatalysts.


### 2.3. Photocatalytic Activity Testing

The photocatalytic activities of the synthesized catalysts were evaluated for naphthalene degradation in an aqueous solution using a tungsten lamp (300 W) under 300–800 nm irradiation for 4 hours. In each experiment, a suspension with a volume of 200 mL containing naphthalene concentration of 80μmol L−1 (10 ppm) and a TiO2 catalyst powder of 2.5 g L−1 was placed in the Pyrex photoreactor under continuous stirring with a magnetic stirrer. The temperature was maintained at 20°C using cooling thermostat because of naphthalene volatility. Prior to illumination, the current suspension was magnetically stirred in the dark for 30 min to reach an adsorption/desorption equilibrium between the photocatalyst and naphthalene. A fixed quantity of the solution was withdrawn at regular time intervals, centrifuging the retrieved samples at 10,000 rpm.


### 2.4. Physical Characterization of the TiO2 Catalysts

Identification of the prepared TiO2 powdered phases under the different preparation conditions at pH 3-4 or pH 8-9 with and without surfactants was examined by powder X-ray diffraction (XRD) analysis using Analytical {X′PERT PROMPD} X-ray diffractometer, CuKα radiation of wavelength λ = 1.5406 Å, rating of 40 KV, 40 mA, step size = 0.02, and scan step time of 0.4 sec in the 2θ range 10–80.The morphology of the samples was checked by using transmission electron microscopy (TEM). The microstructures of the synthesized PANIs were examined by TEM (Tokyo, Japan) on a JEOL JEM-2000EX (Tokyo, Japan) at an accelerating voltage of 100 kV and scanning electron microscopy (SEM). The emission SEM (Tokyo, Japan) was performed with a JEOL 5400 (Tokyo, Japan).The surface area was determined from nitrogen adsorption-desorption isotherms at liquid nitrogen temperature (77 K) using a Quantachrome AS1Win version 2.01 instrument. The TiO2 samples were outgassed for 3 hours at 150°C. The Brunauer-Emmett-Teller (BET) method was used for surface area calculation, while pore-size distribution (pore diameter and volume) was determined by the Barrett-Joyner-Halenda (BJH) method.Diffuse Reflectance Spectroscopy. Visible-ultraviolet spectra were obtained by diffuse reflectance spectroscopy by using a Shimadzu UV-2401 PC instrument. BaSO4 was the reference sample and the spectra were recorded in the range 200–800 nm.For photocatalytic activity measurement, high performance liquid chromatography (HPLC) using HPLC Waters 600 apparatus, equipped with an autosampler (Waters 717 plus) and a dual wavelength absorbance diode array detector (Waters 4487) set at 254 nm, was used with C18 5μm, 4.6 mm × 250 mm column (part no. 186004117) purchased from water USA. The mobile phase was HPLC grade water/acetonitrile (30/70) operating at a flow rate of 1 cm3min−1.


## 2.1. Materials

In the current experiments, all chemicals were used as received. Titanium (IV) isopropoxide (TTIP) (97% Aldrich), isopropanol (i-PrOH, Fisher), acetic acid (Fisher), ammonium hydroxide, cetyltrimetylammonium bromide (CTAB), sodium dodecylbenzenesulfonate (DBS), nonylphenol ethoxylate (NPE), and deionized water were used to prepare the solutions in our experiments. Naphthalene (Panreac, 98%) was used as a pollutant, acetonitrile and deionized water were used as HPLC eluent.


## 2.2. Synthesis of the Current Titania Catalysts

Mesoporous nanocrystalline titania was prepared under controllable sol-gel process using titanium alkoxide in absence or presence of micellar surfactants as templating agents [22]. The molar ratio of surfactant/TTIP/i-PrOH/acetic acid or ammonium hydroxide was  : 4 : 45 : 6, where R is the surfactant concentration was which 0 or 1 at pH 3-4 in acetic acid or 8-9 in ammonia solution. Hydrolysis and polymerization took place in this mixture producing a transparent, homogeneous, and stable TiO2 sol. After gelation for 24 h, the gel was dried overnight at 80°C. The recovered powder was intermittently washed with deionized water and isopropanol five times followed by separation in a centrifuge under 10000 rpm to remove the surfactant. The resulted filtered cake was dried overnight at 100°C and then calcined at 550°C for 4 h to remove the remaining surfactant and consequently produce the desired TiO2 nanoparticles photocatalyst (Scheme 1). The nomenclature was designed according to the pH range and the used surfactant. Preparation catalysts in acidic and basic medium were as follows: (1) without surfactant: A and B, (2) in presence of surfactants, CTAB-A, DBS-A, and NPE-A, in acidic medium, and (3) CTAB-B, DBS-B, and NPE-B in basic medium.Scheme 1
Preparation of TiO2 photocatalysts.


## 2.3. Photocatalytic Activity Testing

The photocatalytic activities of the synthesized catalysts were evaluated for naphthalene degradation in an aqueous solution using a tungsten lamp (300 W) under 300–800 nm irradiation for 4 hours. In each experiment, a suspension with a volume of 200 mL containing naphthalene concentration of 80μmol L−1 (10 ppm) and a TiO2 catalyst powder of 2.5 g L−1 was placed in the Pyrex photoreactor under continuous stirring with a magnetic stirrer. The temperature was maintained at 20°C using cooling thermostat because of naphthalene volatility. Prior to illumination, the current suspension was magnetically stirred in the dark for 30 min to reach an adsorption/desorption equilibrium between the photocatalyst and naphthalene. A fixed quantity of the solution was withdrawn at regular time intervals, centrifuging the retrieved samples at 10,000 rpm.


## 2.4. Physical Characterization of the TiO2 Catalysts

Identification of the prepared TiO2 powdered phases under the different preparation conditions at pH 3-4 or pH 8-9 with and without surfactants was examined by powder X-ray diffraction (XRD) analysis using Analytical {X′PERT PROMPD} X-ray diffractometer, CuKα radiation of wavelength λ = 1.5406 Å, rating of 40 KV, 40 mA, step size = 0.02, and scan step time of 0.4 sec in the 2θ range 10–80.The morphology of the samples was checked by using transmission electron microscopy (TEM). The microstructures of the synthesized PANIs were examined by TEM (Tokyo, Japan) on a JEOL JEM-2000EX (Tokyo, Japan) at an accelerating voltage of 100 kV and scanning electron microscopy (SEM). The emission SEM (Tokyo, Japan) was performed with a JEOL 5400 (Tokyo, Japan).The surface area was determined from nitrogen adsorption-desorption isotherms at liquid nitrogen temperature (77 K) using a Quantachrome AS1Win version 2.01 instrument. The TiO2 samples were outgassed for 3 hours at 150°C. The Brunauer-Emmett-Teller (BET) method was used for surface area calculation, while pore-size distribution (pore diameter and volume) was determined by the Barrett-Joyner-Halenda (BJH) method.Diffuse Reflectance Spectroscopy. Visible-ultraviolet spectra were obtained by diffuse reflectance spectroscopy by using a Shimadzu UV-2401 PC instrument. BaSO4 was the reference sample and the spectra were recorded in the range 200–800 nm.For photocatalytic activity measurement, high performance liquid chromatography (HPLC) using HPLC Waters 600 apparatus, equipped with an autosampler (Waters 717 plus) and a dual wavelength absorbance diode array detector (Waters 4487) set at 254 nm, was used with C18 5μm, 4.6 mm × 250 mm column (part no. 186004117) purchased from water USA. The mobile phase was HPLC grade water/acetonitrile (30/70) operating at a flow rate of 1 cm3min−1.


## 3. Results and Discussion

### 3.1. Effect of Surfactants Type and pH on Particle Size Distribution of TiO2

In order to prevent the growth of nano-TiO2, the influence of the surfactant types on the particle size distribution of TiO2, including anionic surfactant DBS, cationic surfactant CTAB, and nonionic surfactant NPE, is studied. These surfactants assist reducing the particle size of TiO2 during their sorption on the surface of nanoparticles. The reaction depends on the interfacial energy among particles which prevents the aggregation of powders from the static repulsion and special hindrance. To study the influence of reaction conditions on the morphology and phases of TiO2, controlled experiments have been designed with varied types of surfactants and pH. The pH of solution has a significant impact on the TiO2 morphology. The result obtained shows that TiO2 nanoparticles with different sizes can be formed under the conditions of hydrolysis of titanium isopropoxide at two different values, pH = 3-4 (acidic medium) and pH = 8-9 (alkaline medium). At different pH of the system, the diameter of nanoparticles becomes different, since, in acidic media, the concentration of H+ becomes higher. The oxygen atom in Ti–O which has a lone electron pair will easily form hydrogen bond with the H+. Thus the intensity of Ti–O bonds is weakened and the system becomes easier to hydrolyze with higher speed of TiO2 nucleation. The products are smaller while the amount of nucleus is larger [23].In presence of ammonia (alkaline medium), a complex can be formed with Ti4+ which will facilitate the growth of nuclei and increase the peptizing speed. However, the TiO2 crystal changes from anatase to brookite. So, the size of particles can be controlled by regulating the pH of solution [24].


### 3.2. XRD Pattern of TiO2 Nanoparticles

The XRD patterns in Figures1 and 2 and the data listed in Table 1 show the crystalline phase content in the synthesized catalysts. The XRD patterns illustrate the effect of pH modifiers (acetic acid and ammonia) in absence or presence of surfactants. The mass fractions of anatase, rutile, and brookite are calculated from the (101) reflection of anatase at 2θ = 25.48°, the (110) reflection of rutile at 2θ = 27.58°, and (121) reflection of brookite at 2θ = 30.8°. The mass fraction of each phase present in the powder was calculated using the equation x
=
1
+
0.8
(
I
A
/
I
R
)
-
1, where x is the weight fraction of rutile in the TiO2 and I
A and I
R are the X-ray intensities of the anatase and rutile peaks, respectively (see Table 1). Also, the crystallite size of these phases is calculated applying Scherrer’s equation D
=
0.9
λ
/
β
cos
θ, where D is the thickness of crystallite, λ is X-ray wavelength, β is FWHM (full width at half max), and θ is Bragg Angle. The crystallite sizes calculated are in agreement with the particle size measured by TEM.Table 1
Physical characterization of the current catalysts.
Catalyst
Surface area(m2/g)
Crystal phase %
Average TEM(nm)
Absorbance(nm)
Activity %
A
16
A
=
54.63
R
=
45.37
14
390
37
CTAB-A
86.71
A
=
100
8
400
97
DBS-A
57.49
A
=
82.99
R
=
17.01
9
395
85
NPE-A
43.01
A
=
94.73
R
=
5.27
9
390
24
B
12
A
=
96.45
R
=
3.54
11.5
380
20
CTAB-B
62.11
A
=
84.71
B
=
15.29
11
390
70.5
DBS-B
67.21
A
=
100
16
410
83.5
NPE-B
70.29
A
=
91.72
B
=
8.28
10
430
91.6Figure 1
X-ray diffraction spectra for TiO2 at different pH.Figure 2
X-ray diffraction spectra for TiO2 at different pH and surfactants.


#### 3.2.1. Effect of pH in Absence of Surfactants

In the XRD pattern (Figure1) obtained for the TiO2 catalyst prepared using acetic acid as a pH modifier (pH 3-4) (A) gives 54.6% anatase and 45.4% rutile forms. Parra et al. [25] have prepared pure anatase phase at pH 5-6 and reported that, in a stronger acidic medium, the rutile formation would be privileged. On the other hand, when ammonia has been used to adjust the pH at 8-9 (B), it is found to be 96.4% anatase and as low as 3.5% rutile phase. Lim et al. [26] reported that, when TiO2 was prepared using NH4OH at pH 7–9, the rutile phase was only observed at calcination temperatures above 500°C. Hence, it is concluded that the resistance of anatase transformation to rutile increases more in basic medium than in acidic medium at the same calcination temperature (550°C), as with Hu et al. [27].


#### 3.2.2. Effect of pH in Presence of Surfactants

During the preparation of TiO2 catalysts in presence of different types of surfactants, it is found that the produced TiO2 is completely anatase phase using the cationic surfactant (CTAB) at pH 3-4 (CTAB-A), whereas, at pH 9, in presence of the same surfactant (CTAB-B), TiO2 has been produced in two phases, anatase (84.7%) and brookite (15.3%). From XRD patterns (Figure 2 and Table 1), it is calculated from the broadening of the peaks that the crystallite size of the prepared TiO2 using the CTAB surfactant in ammonia solution or acetic acid is lower than that produced in absence of surfactant (in Figure 1). Also, the presence of surfactant suppresses the anatase-rutile transformation. In sample CTAB-A, there is no rutile phase while in sample CTAB-B there is a small amount of the brookite phase. Guohui et al. [28] prepared TiO2 powders using CTAB in the presence of ammonium hydroxide. The authors found that, at calcination temperatures below 600°C, TiO2 samples display dominantly anatase phase together with a small amount of brookite which is in agreement with our results. On using the anionic surfactant (DBS), anatase comprises 83.0% and rutile comprises 17.0% at pH 3-4 (DBS-A), whereas at pH 8-9 (DBS-B) anatase comprises 100%. Nevertheless, using the nonionic surfactant (NPE), the rutile phase comprises 5.3% in anatase/rutile mixture at pH 3-4 (NPE-A), which is less than in the absence of a surfactant. At pH 8-9, the brookite phase appears (8.28%) while the rutile phase is absent (NPE-B).


### 3.3. The Morphologies of TiO2 Nanoparticles

The TEM photographs obtained for the current TiO2 samples prepared at different conditions using various types of surfactants are given in Figures 3 and 4. In the acidic medium (at pH 3-4) while in absence of surfactant, the sample exhibits particles mainly in the form of hexagonal prisms and rhombohedrons (Figure 3). This may be attributed to the presence of sufficient precursor for the reaction to take place. This may help also in obtaining random shapes rather than regular spherical particles. The particle size is varied from 12 to 14 nm in both acidic and basic media. It is also observed that there is an agglomeration of TiO2 particles associated with low surface area and low pore volume. TEM images show many regions with shadow which have been reported to indicate the formation of curved channels between the packed particles [29]. These observations agree with our N2 adsorption/desorption results (Figure 5), where H3 hysteresis loops of TiO2 suggest that there are curved channels in the bulk.TEM images of the TiO2 at different pH.
(a)
(b)TEM images of the TiO2 at different pH and different surfactants. (a) CTAB-A, (b) DBS-A, (c) NPE-A, (d) CTAB-B, (e) DBS-B, and (f) NPE-B.
(a)
(b)
(c)
(d)
(e)
(f)SEM images of the TiO2 without and with different surfactants at pH 3-4.
(a)
(b)
(c)
(d)From the selected area electron diffraction patterns (SAED) of TiO2 with no surfactant in both basic and acidic media (inset of Figure 3), spotty sharp rings occur which are indicative of polycrystalline materials with high crystallinity. The first five SAED rings represent anatase phase indexed as (101), (004), (200), (105), and (211) (JCPDS no, 21-1272) and rutile phase indexed as (110). This result is in agreement with XRD patterns shown in Figure 1.The TEM morphology of TiO2 samples prepared using various types of surfactants in either acidic or basic medium is shown in Figure 4. It can be observed that all samples prepared with the aid of surfactant have more dispersed particles than those without surfactants, which could be attributed to the fact that surfactants prevent the aggregation of TiO2 powders [30]. Chen et al. [31] have reported that (1) the surfactants could adhere on the anatase face (101) of TiO2 and therefore it could modify the surface free energy of TiO2 during the titania catalyst preparation and (2) during the removal of a surfactant by successive washing and calcination processes more mesopores were left in TiO2. TEM images give hexagon, diamond, cohexagon, and bullet shapes.


### 3.4. SEM of TiO2 Nanoparticles

Figure5 shows the SEM images obtained for current samples. The TiO2 particles obtained during preparation in acidic medium in absence of a surfactant acquire heterogeneous sizes with their surface appearing rough. However, the images obtained for the samples CTAB-A, NPE-A, and DBS-A consist of large numbers of nanoparticles with relatively smooth external surfaces. The relatively smooth external surface of those nanoparticles suggests that they are composed of countless tiny primary nanoparticles. The aggregation of these tiny primary nanoparticles can produce large numbers of interaggregated pores, resulting in a highly mesoporous nanotitania as shown in Figure 5. The effect of applying surfactants on the morphology and microstructure of the mesoporous titania nanoparticles shows that there is shrinkage of the nanoparticles diameters caused by collapse of smaller pores. After washing and calcination for 5 times, the surfactants were completely removed and a porous structure was achieved in the microspheres [32, 33].


### 3.5. The BET Surface Characterization

Figure6 shows the isotherms obtained for the prepared TiO2 at different pH values in absence or presence of different templating surfactants. The isotherms are of classical type IV, characteristic for mesoporous materials according to the IUPAC classification [34]. The adsorbed volume at relative pressures below 0.3 is due to monolayer coverage of the surface, while the increase of the relative pressure to 0.4–0.8 with broad hysteresis loops is due to capillary condensation within mesopores [35].N2 adsorption/desorption isotherms for the catalysts.
(a)
(b)In presence of the three types of surfactants, the hysteresis loops of the photocatalysts prepared in basic medium at pH 8-9 appear at a high relative pressureP
/
P
0 range of 0.56–0.70 with H1 and H3 type loops, which correspond to slit shape pores [29]. However, using the same catalysts prepared in acidic medium at pH 3-4, the hysteresis loops appear at P
/
P
0 range of 0.4–0.6 with H2 type loops associated with ink-bottle pores [36]. The surface area, pore volume, and the average pore size of the catalysts are summarized in Table 1. In the presence of anionic and nonionic surfactants, the surface area and pore volume of the photocatalysts prepared at pH 3-4 are higher than those prepared at pH 8-9, indicating higher porosity [32]. In case of using the cationic surfactant (CTAB) at pH 3-4, higher surface area and pore volume have been obtained.Pore-size distribution was calculated according to the BJH method applying the desorption branch of the isotherm. Figure7 shows that the pore-size distribution values occupy a broader pore-size range on using the preparation in basic medium (40–180 Å) relative to that using the acidic medium (40–120 Å). It is observed that the catalyst with the widest pore-size distribution acquires higher surface area and pore volume, as in the case of using CTAB-A catalyst. This agrees with the results of Sasikala et al. [37]. The pore-size range of the synthesized TiO2 catalysts in acidic medium can be arranged in the surfactant order as follows: CTAB > NPE > DBS, whereas synthesis in the basic medium can be arranged in the surfactant order as follows: NPE > DBS > CTAB.Pore-size distribution of TiO2 in acidic and basic media.
(a)
(b)


### 3.6.  UV-Vis Diffuse Reflectance Spectra

Figure8 displays the UV-vis reflectance spectra obtained for TiO2 nanoparticles prepared under different conditions, namely, pH change and absence or presence of surfactants. All samples gave significant red shift towards the visible light region (385–430 nm) which indicates the suitability for applying solar irradiation since the absorbance is related to the sample morphology, surface area, particle size, and crystal phase composition of the particles. The catalysts prepared in absence of surfactants give absorbances at 390 and 385 at pH 3-4 and 8-9, respectively, which is due to the presence of the anatase and rutile of TiO2 phases [38]. However, the absorption edge is shifted to a longer wavelength with increasing the fraction of rutile phase that acquires a smaller band gap (3.0 eV) than that of the anatase phase (3.2 eV). From Figure 8, the largest red shift is caused by CTAB in acidic medium (400 nm) whereas NPE causes a higher shift in the basic medium (430 nm). This is attributed to high surface area, improved grain size [39], pore volume, and the coexistence of anatase and brookite in the TiO2 which cause a decrease of the band gap energy [40, 41]. Moreover, a trace residue of organic compounds or remaining surfactant [42] would have contributed to increasing the red shift. The band gap energy, E
g, of the photocatalysts is assigned to the intrinsic electron transition from the valence band (VB) to the conduction band (CB). E
g values were determined using the absorption UV-vis spectra (Table 1). The optical energy band gap was calculated using the relationship E
g
=
h
·
c
/
λ
=
1240
/
λ [43], where E
g is the band gap (eV) and λ is the wavelength of the absorption edges in the spectrum (nm).UV-vis absorption spectrum of the TiO2 catalysts.
(a)
(b)


### 3.7. Photodegradation of Naphthalene on the Catalysts

In this work, the decrease of naphthalene in the dark for the initial 30 min is taken as the primary adsorption on the catalyst surface. The adsorption capacity is found to increase as surface area increases (Table1). Naphthalene removal comprises as high as 35% on CTAB-A, whereas it is only 12% on NPE-A catalyst. It can be suggested that, as the number of Ti4+ active sites on the surface increases, the rate of electron transfer and adsorption of the pollutant molecules increases [44]. Hao and Zhang [45] reported that an increase of surface area and porosity of the catalyst can reduce the internal mass transfer limitation of the pollutant to the active sites.Figure9 shows that, in absence of any templating agent, the photoactivity of the current catalysts is relatively low (20.0% in basic medium and 37.1% in acidic medium). This can be attributed to acquiring very low surface area (12.0 m2g−1 and 16.3 m2g−1, resp.) and very low pore volume (0.0144 cm3g−1 and 0.0146 cm3g−1, resp.). Furthermore, the rutile formation is as appreciable being 45.4% in acidic medium and 3.5% in the basic medium. On the other hand, the catalyst prepared using CTAB as a templating agent in acidic medium exhibits the highest activity all over the present study for the photodegradation of naphthalene (97% after 180 min) which may be attributed to acquiring the highest surface area (86.7 m2g−1) and the highest pore volume (0.0569 cm3g−1) among all current catalysts. Moreover, this catalyst is composed of 100% anatase phase besides acquiring a particle size as low as 8.0 nm. Furthermore, Figure 8 shows that the largest red shift obtained using this catalyst appears at 400 nm indicating a shift towards reducing the band gab from 3.2 to 3.1 ev which is a great privilege for applying visible (solar) irradiation rather than applying UV irradiation. On the other hand, in the basic medium using the same templating agent (CTAB) while keeping the other variables unchanged, a lower photoactivity has been encountered (71.0%), most expectedly due to its lower surface area (60.1 m2g−1) and lower pore volume (0.0309 m2g−1) as well as acquiring a significant quantity of brookite.Figure 9
Photocatalytic activity of the current catalysts for naphthalene degradation.


## 3.1. Effect of Surfactants Type and pH on Particle Size Distribution of TiO2

In order to prevent the growth of nano-TiO2, the influence of the surfactant types on the particle size distribution of TiO2, including anionic surfactant DBS, cationic surfactant CTAB, and nonionic surfactant NPE, is studied. These surfactants assist reducing the particle size of TiO2 during their sorption on the surface of nanoparticles. The reaction depends on the interfacial energy among particles which prevents the aggregation of powders from the static repulsion and special hindrance. To study the influence of reaction conditions on the morphology and phases of TiO2, controlled experiments have been designed with varied types of surfactants and pH. The pH of solution has a significant impact on the TiO2 morphology. The result obtained shows that TiO2 nanoparticles with different sizes can be formed under the conditions of hydrolysis of titanium isopropoxide at two different values, pH = 3-4 (acidic medium) and pH = 8-9 (alkaline medium). At different pH of the system, the diameter of nanoparticles becomes different, since, in acidic media, the concentration of H+ becomes higher. The oxygen atom in Ti–O which has a lone electron pair will easily form hydrogen bond with the H+. Thus the intensity of Ti–O bonds is weakened and the system becomes easier to hydrolyze with higher speed of TiO2 nucleation. The products are smaller while the amount of nucleus is larger [23].In presence of ammonia (alkaline medium), a complex can be formed with Ti4+ which will facilitate the growth of nuclei and increase the peptizing speed. However, the TiO2 crystal changes from anatase to brookite. So, the size of particles can be controlled by regulating the pH of solution [24].


## 3.2. XRD Pattern of TiO2 Nanoparticles

The XRD patterns in Figures1 and 2 and the data listed in Table 1 show the crystalline phase content in the synthesized catalysts. The XRD patterns illustrate the effect of pH modifiers (acetic acid and ammonia) in absence or presence of surfactants. The mass fractions of anatase, rutile, and brookite are calculated from the (101) reflection of anatase at 2θ = 25.48°, the (110) reflection of rutile at 2θ = 27.58°, and (121) reflection of brookite at 2θ = 30.8°. The mass fraction of each phase present in the powder was calculated using the equation x
=
1
+
0.8
(
I
A
/
I
R
)
-
1, where x is the weight fraction of rutile in the TiO2 and I
A and I
R are the X-ray intensities of the anatase and rutile peaks, respectively (see Table 1). Also, the crystallite size of these phases is calculated applying Scherrer’s equation D
=
0.9
λ
/
β
cos
θ, where D is the thickness of crystallite, λ is X-ray wavelength, β is FWHM (full width at half max), and θ is Bragg Angle. The crystallite sizes calculated are in agreement with the particle size measured by TEM.Table 1
Physical characterization of the current catalysts.
Catalyst
Surface area(m2/g)
Crystal phase %
Average TEM(nm)
Absorbance(nm)
Activity %
A
16
A
=
54.63
R
=
45.37
14
390
37
CTAB-A
86.71
A
=
100
8
400
97
DBS-A
57.49
A
=
82.99
R
=
17.01
9
395
85
NPE-A
43.01
A
=
94.73
R
=
5.27
9
390
24
B
12
A
=
96.45
R
=
3.54
11.5
380
20
CTAB-B
62.11
A
=
84.71
B
=
15.29
11
390
70.5
DBS-B
67.21
A
=
100
16
410
83.5
NPE-B
70.29
A
=
91.72
B
=
8.28
10
430
91.6Figure 1
X-ray diffraction spectra for TiO2 at different pH.Figure 2
X-ray diffraction spectra for TiO2 at different pH and surfactants.


### 3.2.1. Effect of pH in Absence of Surfactants

In the XRD pattern (Figure1) obtained for the TiO2 catalyst prepared using acetic acid as a pH modifier (pH 3-4) (A) gives 54.6% anatase and 45.4% rutile forms. Parra et al. [25] have prepared pure anatase phase at pH 5-6 and reported that, in a stronger acidic medium, the rutile formation would be privileged. On the other hand, when ammonia has been used to adjust the pH at 8-9 (B), it is found to be 96.4% anatase and as low as 3.5% rutile phase. Lim et al. [26] reported that, when TiO2 was prepared using NH4OH at pH 7–9, the rutile phase was only observed at calcination temperatures above 500°C. Hence, it is concluded that the resistance of anatase transformation to rutile increases more in basic medium than in acidic medium at the same calcination temperature (550°C), as with Hu et al. [27].


### 3.2.2. Effect of pH in Presence of Surfactants

During the preparation of TiO2 catalysts in presence of different types of surfactants, it is found that the produced TiO2 is completely anatase phase using the cationic surfactant (CTAB) at pH 3-4 (CTAB-A), whereas, at pH 9, in presence of the same surfactant (CTAB-B), TiO2 has been produced in two phases, anatase (84.7%) and brookite (15.3%). From XRD patterns (Figure 2 and Table 1), it is calculated from the broadening of the peaks that the crystallite size of the prepared TiO2 using the CTAB surfactant in ammonia solution or acetic acid is lower than that produced in absence of surfactant (in Figure 1). Also, the presence of surfactant suppresses the anatase-rutile transformation. In sample CTAB-A, there is no rutile phase while in sample CTAB-B there is a small amount of the brookite phase. Guohui et al. [28] prepared TiO2 powders using CTAB in the presence of ammonium hydroxide. The authors found that, at calcination temperatures below 600°C, TiO2 samples display dominantly anatase phase together with a small amount of brookite which is in agreement with our results. On using the anionic surfactant (DBS), anatase comprises 83.0% and rutile comprises 17.0% at pH 3-4 (DBS-A), whereas at pH 8-9 (DBS-B) anatase comprises 100%. Nevertheless, using the nonionic surfactant (NPE), the rutile phase comprises 5.3% in anatase/rutile mixture at pH 3-4 (NPE-A), which is less than in the absence of a surfactant. At pH 8-9, the brookite phase appears (8.28%) while the rutile phase is absent (NPE-B).


## 3.2.1. Effect of pH in Absence of Surfactants

In the XRD pattern (Figure1) obtained for the TiO2 catalyst prepared using acetic acid as a pH modifier (pH 3-4) (A) gives 54.6% anatase and 45.4% rutile forms. Parra et al. [25] have prepared pure anatase phase at pH 5-6 and reported that, in a stronger acidic medium, the rutile formation would be privileged. On the other hand, when ammonia has been used to adjust the pH at 8-9 (B), it is found to be 96.4% anatase and as low as 3.5% rutile phase. Lim et al. [26] reported that, when TiO2 was prepared using NH4OH at pH 7–9, the rutile phase was only observed at calcination temperatures above 500°C. Hence, it is concluded that the resistance of anatase transformation to rutile increases more in basic medium than in acidic medium at the same calcination temperature (550°C), as with Hu et al. [27].


## 3.2.2. Effect of pH in Presence of Surfactants

During the preparation of TiO2 catalysts in presence of different types of surfactants, it is found that the produced TiO2 is completely anatase phase using the cationic surfactant (CTAB) at pH 3-4 (CTAB-A), whereas, at pH 9, in presence of the same surfactant (CTAB-B), TiO2 has been produced in two phases, anatase (84.7%) and brookite (15.3%). From XRD patterns (Figure 2 and Table 1), it is calculated from the broadening of the peaks that the crystallite size of the prepared TiO2 using the CTAB surfactant in ammonia solution or acetic acid is lower than that produced in absence of surfactant (in Figure 1). Also, the presence of surfactant suppresses the anatase-rutile transformation. In sample CTAB-A, there is no rutile phase while in sample CTAB-B there is a small amount of the brookite phase. Guohui et al. [28] prepared TiO2 powders using CTAB in the presence of ammonium hydroxide. The authors found that, at calcination temperatures below 600°C, TiO2 samples display dominantly anatase phase together with a small amount of brookite which is in agreement with our results. On using the anionic surfactant (DBS), anatase comprises 83.0% and rutile comprises 17.0% at pH 3-4 (DBS-A), whereas at pH 8-9 (DBS-B) anatase comprises 100%. Nevertheless, using the nonionic surfactant (NPE), the rutile phase comprises 5.3% in anatase/rutile mixture at pH 3-4 (NPE-A), which is less than in the absence of a surfactant. At pH 8-9, the brookite phase appears (8.28%) while the rutile phase is absent (NPE-B).


## 3.3. The Morphologies of TiO2 Nanoparticles

The TEM photographs obtained for the current TiO2 samples prepared at different conditions using various types of surfactants are given in Figures 3 and 4. In the acidic medium (at pH 3-4) while in absence of surfactant, the sample exhibits particles mainly in the form of hexagonal prisms and rhombohedrons (Figure 3). This may be attributed to the presence of sufficient precursor for the reaction to take place. This may help also in obtaining random shapes rather than regular spherical particles. The particle size is varied from 12 to 14 nm in both acidic and basic media. It is also observed that there is an agglomeration of TiO2 particles associated with low surface area and low pore volume. TEM images show many regions with shadow which have been reported to indicate the formation of curved channels between the packed particles [29]. These observations agree with our N2 adsorption/desorption results (Figure 5), where H3 hysteresis loops of TiO2 suggest that there are curved channels in the bulk.TEM images of the TiO2 at different pH.
(a)
(b)TEM images of the TiO2 at different pH and different surfactants. (a) CTAB-A, (b) DBS-A, (c) NPE-A, (d) CTAB-B, (e) DBS-B, and (f) NPE-B.
(a)
(b)
(c)
(d)
(e)
(f)SEM images of the TiO2 without and with different surfactants at pH 3-4.
(a)
(b)
(c)
(d)From the selected area electron diffraction patterns (SAED) of TiO2 with no surfactant in both basic and acidic media (inset of Figure 3), spotty sharp rings occur which are indicative of polycrystalline materials with high crystallinity. The first five SAED rings represent anatase phase indexed as (101), (004), (200), (105), and (211) (JCPDS no, 21-1272) and rutile phase indexed as (110). This result is in agreement with XRD patterns shown in Figure 1.The TEM morphology of TiO2 samples prepared using various types of surfactants in either acidic or basic medium is shown in Figure 4. It can be observed that all samples prepared with the aid of surfactant have more dispersed particles than those without surfactants, which could be attributed to the fact that surfactants prevent the aggregation of TiO2 powders [30]. Chen et al. [31] have reported that (1) the surfactants could adhere on the anatase face (101) of TiO2 and therefore it could modify the surface free energy of TiO2 during the titania catalyst preparation and (2) during the removal of a surfactant by successive washing and calcination processes more mesopores were left in TiO2. TEM images give hexagon, diamond, cohexagon, and bullet shapes.


## 3.4. SEM of TiO2 Nanoparticles

Figure5 shows the SEM images obtained for current samples. The TiO2 particles obtained during preparation in acidic medium in absence of a surfactant acquire heterogeneous sizes with their surface appearing rough. However, the images obtained for the samples CTAB-A, NPE-A, and DBS-A consist of large numbers of nanoparticles with relatively smooth external surfaces. The relatively smooth external surface of those nanoparticles suggests that they are composed of countless tiny primary nanoparticles. The aggregation of these tiny primary nanoparticles can produce large numbers of interaggregated pores, resulting in a highly mesoporous nanotitania as shown in Figure 5. The effect of applying surfactants on the morphology and microstructure of the mesoporous titania nanoparticles shows that there is shrinkage of the nanoparticles diameters caused by collapse of smaller pores. After washing and calcination for 5 times, the surfactants were completely removed and a porous structure was achieved in the microspheres [32, 33].


## 3.5. The BET Surface Characterization

Figure6 shows the isotherms obtained for the prepared TiO2 at different pH values in absence or presence of different templating surfactants. The isotherms are of classical type IV, characteristic for mesoporous materials according to the IUPAC classification [34]. The adsorbed volume at relative pressures below 0.3 is due to monolayer coverage of the surface, while the increase of the relative pressure to 0.4–0.8 with broad hysteresis loops is due to capillary condensation within mesopores [35].N2 adsorption/desorption isotherms for the catalysts.
(a)
(b)In presence of the three types of surfactants, the hysteresis loops of the photocatalysts prepared in basic medium at pH 8-9 appear at a high relative pressureP
/
P
0 range of 0.56–0.70 with H1 and H3 type loops, which correspond to slit shape pores [29]. However, using the same catalysts prepared in acidic medium at pH 3-4, the hysteresis loops appear at P
/
P
0 range of 0.4–0.6 with H2 type loops associated with ink-bottle pores [36]. The surface area, pore volume, and the average pore size of the catalysts are summarized in Table 1. In the presence of anionic and nonionic surfactants, the surface area and pore volume of the photocatalysts prepared at pH 3-4 are higher than those prepared at pH 8-9, indicating higher porosity [32]. In case of using the cationic surfactant (CTAB) at pH 3-4, higher surface area and pore volume have been obtained.Pore-size distribution was calculated according to the BJH method applying the desorption branch of the isotherm. Figure7 shows that the pore-size distribution values occupy a broader pore-size range on using the preparation in basic medium (40–180 Å) relative to that using the acidic medium (40–120 Å). It is observed that the catalyst with the widest pore-size distribution acquires higher surface area and pore volume, as in the case of using CTAB-A catalyst. This agrees with the results of Sasikala et al. [37]. The pore-size range of the synthesized TiO2 catalysts in acidic medium can be arranged in the surfactant order as follows: CTAB > NPE > DBS, whereas synthesis in the basic medium can be arranged in the surfactant order as follows: NPE > DBS > CTAB.Pore-size distribution of TiO2 in acidic and basic media.
(a)
(b)


## 3.6.  UV-Vis Diffuse Reflectance Spectra

Figure8 displays the UV-vis reflectance spectra obtained for TiO2 nanoparticles prepared under different conditions, namely, pH change and absence or presence of surfactants. All samples gave significant red shift towards the visible light region (385–430 nm) which indicates the suitability for applying solar irradiation since the absorbance is related to the sample morphology, surface area, particle size, and crystal phase composition of the particles. The catalysts prepared in absence of surfactants give absorbances at 390 and 385 at pH 3-4 and 8-9, respectively, which is due to the presence of the anatase and rutile of TiO2 phases [38]. However, the absorption edge is shifted to a longer wavelength with increasing the fraction of rutile phase that acquires a smaller band gap (3.0 eV) than that of the anatase phase (3.2 eV). From Figure 8, the largest red shift is caused by CTAB in acidic medium (400 nm) whereas NPE causes a higher shift in the basic medium (430 nm). This is attributed to high surface area, improved grain size [39], pore volume, and the coexistence of anatase and brookite in the TiO2 which cause a decrease of the band gap energy [40, 41]. Moreover, a trace residue of organic compounds or remaining surfactant [42] would have contributed to increasing the red shift. The band gap energy, E
g, of the photocatalysts is assigned to the intrinsic electron transition from the valence band (VB) to the conduction band (CB). E
g values were determined using the absorption UV-vis spectra (Table 1). The optical energy band gap was calculated using the relationship E
g
=
h
·
c
/
λ
=
1240
/
λ [43], where E
g is the band gap (eV) and λ is the wavelength of the absorption edges in the spectrum (nm).UV-vis absorption spectrum of the TiO2 catalysts.
(a)
(b)


## 3.7. Photodegradation of Naphthalene on the Catalysts

In this work, the decrease of naphthalene in the dark for the initial 30 min is taken as the primary adsorption on the catalyst surface. The adsorption capacity is found to increase as surface area increases (Table1). Naphthalene removal comprises as high as 35% on CTAB-A, whereas it is only 12% on NPE-A catalyst. It can be suggested that, as the number of Ti4+ active sites on the surface increases, the rate of electron transfer and adsorption of the pollutant molecules increases [44]. Hao and Zhang [45] reported that an increase of surface area and porosity of the catalyst can reduce the internal mass transfer limitation of the pollutant to the active sites.Figure9 shows that, in absence of any templating agent, the photoactivity of the current catalysts is relatively low (20.0% in basic medium and 37.1% in acidic medium). This can be attributed to acquiring very low surface area (12.0 m2g−1 and 16.3 m2g−1, resp.) and very low pore volume (0.0144 cm3g−1 and 0.0146 cm3g−1, resp.). Furthermore, the rutile formation is as appreciable being 45.4% in acidic medium and 3.5% in the basic medium. On the other hand, the catalyst prepared using CTAB as a templating agent in acidic medium exhibits the highest activity all over the present study for the photodegradation of naphthalene (97% after 180 min) which may be attributed to acquiring the highest surface area (86.7 m2g−1) and the highest pore volume (0.0569 cm3g−1) among all current catalysts. Moreover, this catalyst is composed of 100% anatase phase besides acquiring a particle size as low as 8.0 nm. Furthermore, Figure 8 shows that the largest red shift obtained using this catalyst appears at 400 nm indicating a shift towards reducing the band gab from 3.2 to 3.1 ev which is a great privilege for applying visible (solar) irradiation rather than applying UV irradiation. On the other hand, in the basic medium using the same templating agent (CTAB) while keeping the other variables unchanged, a lower photoactivity has been encountered (71.0%), most expectedly due to its lower surface area (60.1 m2g−1) and lower pore volume (0.0309 m2g−1) as well as acquiring a significant quantity of brookite.Figure 9
Photocatalytic activity of the current catalysts for naphthalene degradation.


## 4. Conclusion

The current TiO2 photocatalysts have been prepared by sol-gel method using Ti-alkoxide as precursor, in acidic or basic media in absence or presence of different surfactants (templates). XRD analysis showed that addition of surfactants suppressed the transformation of anatase to rutile phase. All catalysts exhibited activities in the visible range at various levels. In both acidic and basic media, in absence of surfactants, the photoactivities for the pollutant degradation were 37% (A: acid medium) and 20% (B: basic medium), respectively, whereas these values jumped by adding the surfactants to ~97% using CTAB-A catalyst and to ~91% using NPE-B sample. The most effective factors for photodegradation improvement were the surface area and total pore volume (mainly described by pore-size distribution). The pore-size distribution behaviour is found to exhibit the most pronounced relevance to the catalytic activity of the current photocatalytic degradation of naphthalene. The widest mesopores are acquired by the CTAB templated acidic sample but they acquire the narrowest sizes in the pore-size distribution of the basic medium. CTAB-A catalyst gave the highest red shift in the visible range.



---

*Source: 687597-2014-02-04.xml*