Adsorption of methyl orange on nanoparticles of a synthetic zeolite NaA/CuO

El Hadj Mekatel; Samira Amokrane; Asma Aid; Djamel Nibou; Mohamed Trari

doi:10.1016/j.crci.2014.09.009

GeCat 2014: Advances and prospects in heterogeneous catalysis

Adsorption of methyl orange on nanoparticles of a synthetic zeolite NaA/CuO

El Hadj Mekatel ¹ ; Samira Amokrane ¹ ; Asma Aid ¹ ; Djamel Nibou ¹ ; Mohamed Trari ²

¹ Laboratoire de technologie des matériaux, USTHB, BP 32, El-Alia, Bab-Ezzouar, 16111 Alger, Algeria
² Laboratory of Storage and Valorization of Renewable Energies, USTHB, BP 32, El-Alia, 16111 Alger, Algeria

Comptes Rendus. Chimie, Volume 18 (2015) no. 3, pp. 336-344.

Résumés

Anglais
Français

CuO supported on an NaA zeolite (CuO/NaA) was prepared with an NaA zeolite through the ion-exchange (CuO/NaA) method. The morphology and the physicochemical properties of the prepared samples were investigated by XRD, MEB, and EDS. The various parameters, such as contact time, catalyst dose, initial dye concentration, initial pH, and temperature, influencing the adsorption of methyl orange (MO) were optimized. The MO adsorption equilibrium was reached after 240 min of contact time. Removal of MO is better at neutral pH than in acidic and alkaline solutions. Among the tested models, the equilibrium adsorption data are well fitted by the Langmuir isotherm. The adsorption kinetics is best described by the pseudo-second-order model. The evaluation of the thermodynamic parameters, i.e. ΔG^o, ΔH^o, and ΔS^o, revealed that MO adsorption was spontaneous, while the activation energy (20.98 kJ/mol) indicates a physical adsorption. The photodegradation of MO decreased from 100 mg/L down to 2 mg/L when the solution is exposed to visible light.

L’oxyde de cuivre CuO supporté sur une zéolithe NaA (CuO/NaA) a été préparé par la méthode d’échange d’ions. Les propriétés morphologiques et physico-chimiques des échantillons préparés ont été étudiées par diffraction des rayons X, MEB et SED. Les différents paramètres, tels que le temps de contact, le dosage de l’agent adsorbant, la concentration initiale en colorant, le pH initial et la température, influençant l’adsorption de l’orange de méthyle (MO) ont été optimisés. L’équilibre d’adsorption de MO a été atteint après 240 minutes de réaction. L’élimination du MO est meilleure à un pH neutre par rapport aux solutions acides et alcalines. Parmi les modèles testés, les données de l’équilibre d’adsorption ont été bien décrites par l’isotherme de Langmuir. Les cinétiques d’adsorption ont été mieux décrites par un modèle du pseudo-deuxième ordre. L’évaluation des paramètres thermodynamiques ΔG^o, ΔH^o and ΔS^o a révélé que l’adsorption du MO était spontanée. L’énergie d’activation a été trouvée égale à 20,98 kJ/mol, indiquant une adsorption physique. La photodégradation du MO a diminué de 100 mg/L jusqu’à 2 mg/L lorsque la solution était exposée à la lumière visible.

Métadonnées

Reçu le : 2014-04-29
Accepté le : 2014-09-25
Publié le : 2015-02-01

DOI : 10.1016/j.crci.2014.09.009

Keywords: CuO, NaA zeolite, Adsorption, Methyl orange (MO), Photodegradation
Mots clés : CuO, Zéolithe NaA, Adsorption, Méthyle orange (MO), Photodégradation

Affiliations des auteurs :

El Hadj Mekatel ¹ ; Samira Amokrane ¹ ; Asma Aid ¹ ; Djamel Nibou ¹ ; Mohamed Trari ²

@article{CRCHIM_2015__18_3_336_0,
     author = {El Hadj Mekatel and Samira Amokrane and Asma Aid and Djamel Nibou and Mohamed Trari},
     title = {Adsorption of methyl orange on nanoparticles of a synthetic zeolite {NaA/CuO}},
     journal = {Comptes Rendus. Chimie},
     pages = {336--344},
     publisher = {Elsevier},
     volume = {18},
     number = {3},
     year = {2015},
     doi = {10.1016/j.crci.2014.09.009},
     language = {en},
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El Hadj Mekatel; Samira Amokrane; Asma Aid; Djamel Nibou; Mohamed Trari. Adsorption of methyl orange on nanoparticles of a synthetic zeolite NaA/CuO. Comptes Rendus. Chimie, Volume 18 (2015) no. 3, pp. 336-344. doi : 10.1016/j.crci.2014.09.009. https://comptes-rendus.academie-sciences.fr/chimie/articles/10.1016/j.crci.2014.09.009/

Version originale du texte intégral

1 Introduction

Over the last decades, considerable amounts of colored wastewaters have been generated from many industries, including textile, leather, paper, printing, dyestuff, plastic, and so on [1,2]. Dye removal from contaminated water is very important because the water quality is strongly influenced by color. Even a small amount of dye is undesirable and affects dramatically the ecosystem. Moreover, many dyes employed nowadays are considered to be toxic and even carcinogenic [1,3].

Dye effluents normally contain about 10 to 50 mg/L; however, for concentrations as small as 1 mg/L, the dyes are easily noticeable and may be perceived as contaminators and consequently unacceptable. As a result, the treatments of dye effluents have been extensively investigated. Currently, the adsorption is found to be efficient because of its easy operation and the flexibility and simplicity of the design [4,5]. In this respect, activated carbon is extensively used due to its moderate price, single adsorption ability and regeneration process [6]; this explains why its use is limited. For this reason, the exploration of new and more efficient adsorption materials has important practical significance and wide application prospects for environmental protection. Cupric oxide (CuO) is a p-type semiconductor with an energy band gap of 1.21 eV, which can be excited under sunlight radiation [7]. CuO has various applications: glucose sensors [8], field emission emitters [9], gas sensors [10], and heterogeneous catalysts [11]. More recently, many studies have been focused on its application in photocatalysis. However, in most reports, CuO was used only as a sensitizer in photocatalytic heterosystems, like CuO/TiO₂ [12,13], CuO/SnO₂ [14], CuO/ZnO [15], and CuO/clay [16,17]. Therefore, the objective of the present work is to prepare heterogeneous a CuO catalyst supported on an NaA zeolite by exchange process and to assess its adsorption and photocatalytic activity for the degradation of methyl orange (MO) under artificial light.

2 Materials and methods

2.1 Catalyst preparation

The exchange technique was used to prepare CuO/NaA according to the following protocol: 1 g of the NaA synthesized zeolite was added to 200 mL of Cu (NO₃)₂·3H₂O (0.1 M) (Assay, 98%) and shaken for 8 h in a polyethylene bottle at room temperature. The NaA zeolite was synthesized by hydrothermal process, as reported in our previous work [18]. The solid product was filtered and washed with doubly distilled water until Cu²⁺ becomes undetectable in solution. Then, the sample was dried at room temperature and referred to as CuO/NaA zeolite. Finally, CuO/NaA was calcined at 450 °C for 4 h.

2.2 Characterization

The NaA, CuO and CuO/NaA samples were characterized by X-ray diffraction (Philips PW 1800, using Cu Kα radiation), over the 2θ range between 5 and 35°. The surface morphology was observed with a scanning electronic microscope (SEM, Philips XL 30) equipped with an energy dispersive spectrometry (EDS) unit for chemical analysis.

2.3 Batch adsorption

Batch adsorption experiments of MO were carried out in a double-walled Pyrex reactor of capacity 200 cm³, whose temperature was regulated by a thermostated bath. The MO solutions (50–200 mg/L) were prepared by dilution from a stock solution (1000 mg/L) of MO (Merck, 99.5%). The effect of pH on the adsorption of MO was examined by mixing 0.2 g of CuO/NaA with 100 mL of a MO (50 mg/L) solution whose pH ranged from 3.0 to 11.0; the pH was adjusted with NaOH (0.1 N) or HCl (0.1 N). The adsorption kinetics and isotherms of the dye solutions (50–250 mg/L) were performed at different temperatures (25, 30, 40, and 55 °C). The final MO concentration was determined using a UV–Vis spectrophotometer (Optizen 2120 UV–Visible, λ_max = 465 nm). The percentage of MO removal was calculated using the relationship:

Removal of MO (%) = \frac{(C_{o} - C_{e})}{C_{o}} \times 100

(1)

where C_o and C_e are the initial and equilibrium MO concentrations (mg/L), respectively. The adsorption capacity of the adsorbent material, q_t (mg/g), was determined using the relationship:

q_{t} = \frac{(C_{o} - C_{e}) V}{m}

(2)

q_t is the adsorbed quantity per unit mass at any time (mg/g), V is the volume of the MO solution and m is the weight of CuO/NaA. The uptake distribution coefficient (K_d) is given by [19]:

K_{d} = \frac{(C_{o} - C_{e}) m}{C_{e} V}

(3)

2.4 Photoactivity experiments

The photocatalytic degradation is undertaken with a volume of 100 mL (MO: 100 mg/L, pH ∼ 7) and 200 mg of CuO/NaA in the same reactor as above. The light source is a tungsten lamp (200 W, Philips) emitting over the range from 400 to 750 nm and located 14 cm above the reactor, thus providing a light flux of 10.3 mW·cm⁻².

3 Results and discussion

3.1 Characterization

Fig. 1 shows the XRD patterns of three samples. Fig. 1a corresponds to the sodalite NaA structure with strong peaks in the 2θ range from 5 to 35°, which indicates that the zeolite was well prepared, while Fig. 1b corresponds to the CuO structure. The two phases are in good agreement with those already reported in the literature [13,18]. As expected, the XRD pattern (Fig. 1c) shows the peaks of the zeolite NaA, which coexist with those of CuO.

Fig. 1
XRD patterns of NaA (a), CuO (b) and CuO/NaA (c).

Scanning electronic micrographs (Fig. 2a) show that the crystallites of an NaA zeolite form fine cubic particles with an average size of 2–5 μm. Fig. 2b shows that CuO particles crystallize as needles, with an average size of about 0.1–0.5 μm, and form spherical aggregates. It seems that the preparation method of this oxide has a positive influence on crystal morphology. Fig. 2c shows that CuO particles are well dispersed in the structure surface of the NaA zeolite. The chemical analysis by EDS confirmed the presence of copper on the surface of the NaA zeolite.

Fig. 2
SEM images of the zeolite NaA (a), CuO (b) and CuO/NaA (c).

3.2 Adsorption

3.2.1 Effect of pH

The pH of the solution is a controlling parameter that strongly affects the adsorption of dyes on the CuO/NaA surface. The influence of pH on MO adsorption was investigated over the range from 3 to 11 and the results are displayed in Fig. 3, which shows a maximum removal of MO (99%) at pH ∼ 7. At lower pH_s values, the adsorbants have a net positive charge. Hence, the minimum MO removal obtained at low pH may be due to the electrostatic attractions between negatively charged functional groups located on MO and the positively charged adsorbent surface. Hydrogen ion also acts as a bridging ligand between the adsorbent and dye molecules [20]. As pH increases, the number of hydroxide ions increases and competes with anionic ion MO on the adsorption. A similar type of behavior was reported for the adsorption of the dye onto different adsorbents [20]. Therefore, a pH value ∼ 7 was selected for further studies.

Fig. 3
Effect of pH on the removal of MO onto CuO/NaA (MO = 50 mg/L, catalyst dose = 2 g/L, T = 298 K and time of agitation = 5 h).

3.2.2 Effect of contact time

The effect of the contact time on the removal percentage of MO was investigated for a concentration of 50 mg/L (Fig. 4). The uptake of MO by CuO/NaA was rapid at the beginning, due to a larger surface area of adsorbent, and gradually decreases with time until it reaches saturation. The plots reveal that the maximum removal is achieved after 240 min of shaking. After adsorption, MO uptake is controlled by the rate of dye transported from the exterior to the internal pores of the adsorbent.

Fig. 4
Time of contact on the removal of MO onto CuO/NaA (MO = 50 mg/L, pH ∼ 7, catalyst dose = 2 g/L and T = 298 K).

3.2.3 Effect of the catalyst dose

The adsorbent dose is an important parameter since it determines the uptake capacity of an adsorbent for a given initial MO concentration under the operating conditions. The influence of the dose on MO adsorption (Fig. 5) increases with increasing the dose of CuO/NaA, and the adsorption is almost constant at doses higher than 2 g/L. This may be due to the increased availability of surface active sites resulting from the increased dose and conglomeration of the adsorbent.

Fig. 5
Effect of the dose of catalyst on the removal of MO onto CuO/NaA (MO = 50 mg/L, pH ∼ 7, T = 298 K).

3.2.4 Effect of initial concentration of MO

The effect of MO concentration over the range (50–250 mg/L) was investigated with a dose of 2 g/L, pH ∼ 7, a temperature of 25 °C and a duration of 6 h. The results show that the percentage removal of MO was found to decrease with increasing the initial MO concentration, achieving a maximum removal of 97% at 50 mg/L and of 60% for 250 mg/L (Fig. 6). This strong adsorption for low initial MO concentrations might be explained by the active sites available on the adsorbent. Similar results have been reported in the literature [21–23].

Fig. 6
Effect of initial concentration and contact time on the removal of MO onto CuO/NaA. (pH ∼ 7, catalyst dose = 2 g/L and T = 298 K).

3.2.5 Effect of temperature

The adsorption of MO onto CuO/NaA was studied for a concentration of 50 mg/L by varying the temperature from 25 to 55 °C (Fig. 7). The percentage of MO removal increased with increasing the temperature from 25 to 55 °C; it can be seen that higher temperatures were favorable for adsorption. The equilibrium adsorption capacity was affected by the temperature and the amount of MO adsorbed increased from 67.55 to 94% when the temperature was raised from 25 to 55 °C. It has been well documented that the temperature has two major effects on the adsorption process. An increase in temperature is known to increase the diffusion rate of the adsorbate molecules across the external boundary layer and in the internal pores of the adsorbent particles as a result of the decreased viscosity of the solution.

Fig. 7
Effect of temperature and contact time on the removal of MO by CuO/NaA (MO = 50 mg/L, pH ∼ 7 and catalyst dose = 1 g/L).

3.3 Adsorption isotherms

In order to describe the removal mechanism of MO from water onto CuO/NaA, three isotherm models (Freundlich, Langmuir and Temkin isotherm models) were applied. The Langmuir, Freundlich and Temkin isotherm models were applied to establish the relationship between the amount of MO adsorbed by CuO/NaA and their equilibrium concentration in aqueous solution. The experimental data are fitted by the Langmuir model [24]:

\frac{C_{e}}{q_{e}} = \frac{1}{q_{m} b} + \frac{C_{e}}{q_{m}}

(4)

where C_e is equilibrium concentration of MO (mg/L) and q_e is the amount of adsorbed MO (mg/g). The monolayer adsorption capacity (q_m, mg/g) and the Langmuir constant related to the free adsorption energy (b, L/mg) were evaluated from the slope and intercept of the linear plots of C_e/q_e versus C_e, respectively (Fig. 8a); the results are presented in Table 1.

Fig. 8
(a) Langmuir, (b) Freudlich, (c) Temkin isotherms for the MO adsorption and experimental data that do not arrange linearly.

Langmuir
q_m (mg/g)	79.49
b (L/mg)	0.108
R²	0.995
Freundlich
K_F (mg/g)	19.636
n	3.28
R²	0.979
Temkin
b_T (J/mol)	182.317
A_T (L/g)	2.492
R²	0.955

The adsorption equilibrium data were also applied to the Freundlich model in logarithmic form [25]:

\ln q_{e} = \ln K_{F} + \frac{1}{n} \ln C_{e}

(5)

where K_F (mg/g) and n are the Freundlich constants related to adsorption capacity and adsorption intensity, respectively; Fig. 8b illustrates the analysis data. The values of K_F and n were determined from the intercept and slope of the linear plot of ln q_e versus ln C_e, respectively, and the results are presented in Table 1.

The Temkin isotherm contains a factor that explicitly takes into account adsorbent–adsorbate interactions. By ignoring the extremely low and large concentrations, the model assumes that the heat of adsorption (function of temperature) of all molecules in the layer would decrease linearly rather than logarithmically with coverage. The derivation is characterized by a uniform distribution of binding energies (up to some maximum binding energy) that was evidenced by plotting q_e against ln C_e [Eq. (6)]:

q_{e} = B \ln A_{T} + B \ln C_{e}

(6)

where A_T (L/g) and B (J/mol) are the Temkin constants related to the binding equilibrium isotherm and to the heat of adsorption, respectively. The constants were determined from the slope and the intercept.

The adsorption of MO onto CuO/NaA was well fitted with the Langmuir, Freundlich and Temkin models because of the high correlation coefficients (R²). The Langmuir model (R² = 0.995) was more applicable than those of Freundlich (R² = 0.979) and Temkin (R² = 0.955). The Langmuir adsorption maximum, q_m, is quite high (79.49 mg/g), with a constant b of 0.108 L/mg. The Freundlich coefficient (n = 3.28) was smaller than 10, indicating that the adsorption of MO on CuO/NaA under the studied conditions was favored. By contrast, Fig. 8 shows experimental data that do not arrange linearly. It seems that the data are well fitted by using the models of Langmuir and Temkin.

3.4 Adsorption kinetics

The adsorption kinetics is important because it controls the efficiency of the process and the equilibrium time. It also describes the rate of adsorbate uptake on CuO/NaA. In order to identify the potential rate-controlling steps involved in the adsorption process, two kinetic models were used to fit the experimental data, namely the pseudo-first-order and pseudo-second-order models.

3.4.1 Lagergren pseudo-first-order model

The Lagergren equation is the earliest known example describing the rate of adsorption in the liquid–phase systems; it involves a pseudo-first-order kinetics [26,28]:

\frac{d q}{d t} = k_{1} (q_{e} - q_{t})

(7)

where k₁ is the pseudo-first-order adsorption rate coefficient (min⁻¹). The integrated form of Eq. (7) for the boundary conditions (t = 0 to t and q_t = 0 to q_t) becomes:

ln (q_{e} - q_{t}) = ln q_{e} - k_{1} t

(8)

The values of k₁ can be obtained from the slope of the linear plot of $ln (q_{e} - q_{t})$ versus t.

3.4.2 Pseudo-second-order model

The second-order kinetics may be tested on the basis of the following equation [29]:

\frac{d q}{d t} = k_{2} {(q_{e} - q_{t})}^{2}

(9)

where k₂ is the pseudo-second-order adsorption rate coefficient (g/mg/min). For the boundary conditions (t = 0 to t and q_t = 0 to q_t), Eq. (9) becomes:

\frac{t}{q_{t}} = \frac{1}{(k_{2} {q_{e}}^{2})} + \frac{1}{q_{e}} t

(10)

The plots of t/q_t versus time (t) for different concentrations (C_o) and various temperatures fit well with the experimental data and provide the rate constants k₂ and q_e. Plots of Lagergren first-order and pseudo-second-order kinetic models are shown in Figs. 9 and 10 for different MO concentrations and temperatures (Table 2). The R² coefficients of the pseudo-second-order kinetics were higher than 0.994 for both solutions. Moreover, the calculated q_e value agrees well with the experimental one, indicating that the model fits better the adsorption data.

Fig. 9
Pseudo-first-order kinetic model for the removal of MO onto CuO/NaA under: (a) different initial concentrations (C_o); (b) different temperatures.

Fig. 10
Pseudo-second-order kinetic model for the removal of MO onto CuO/NaA under: (a) different initial concentrations (C_o); (b) different temperatures.

	Pseudo-first-order	Pseudo-second-order
	q_e^cal (mg/g)	k₁ × 10² (min⁻¹)	R²	q_e^cal (mg/g)	k₂ × 10⁴ (g·mg⁻¹·min⁻¹)	R²
MO (mg/L)
50	31.74	1.48	0.941	31.84	3.22	0.994
100	44.53	1.19	0.990	54.05	2.21	0.997
150	55.49	1.51	0.899	76.92	1.57	0.996
200	75.07	1.40	0.992	86.20	1.62	0.995
250	66.63	1.14	0.975	90.09	1.69	0.997
T (K)
298	31.76	1.08	0.9458	72.67	5.18	0.9989
308	61.72	1.07	0.9988	98.91	1.94	0.9965
318	63.25	1.28	0.9006	101.01	2.81	0.9961
328	48.58	1.03	0.9879	102.46	3.19	0.9962

The rate constants k₂ at different temperatures (Table 2) were used to estimate the activation energy of MO adsorption onto CuO/NaA. The relationship among the rate constant k₂, temperature (T) and activation energy (E_a) follows the Arrhenius equation [30]:

k_{2} = A_{o} \exp (- E_{a} / R T)

(11)

the linearization gives:

ln k_{2} = - E_{a} / R (1/ T) + ln A_{o}

(12)

where R (8.314 J/mol·K) is the universal gas constant and A_o is a pre-exponential factor. The slope of plot ln k₂ versus 1/T (Fig. 11) gives an activation energy E_a (20.98 kJ/mol) that indicates physical adsorption [18,30].

Fig. 11
Determination of the adsorption activation energy (E_a).

3.5 Thermodynamic study

The thermodynamic parameters were evaluated to confirm the nature of the adsorption and the inherent energetic changes involved during MO adsorption. Standard enthalpy (ΔH°), free energy (ΔG°) and entropy change (ΔS°) were calculated to determine the thermodynamic feasibility and the spontaneous nature of the process. Therefore, the values of ΔH° and ΔS° were obtained from the slope and intercept of the ln K_d versus 1/T curve according to Eq. (12) (Fig. 12) [18]:

ln K_{d} = (\frac{Δ S^{\circ}}{R}) - (\frac{Δ H^{\circ}}{R T})

(12)

while the ΔG° value of can be determined from:

ΔG° = ΔH° – TΔS°

(13)

Fig. 12
Graphical determination of ΔH° and ΔS°.

As can be seen in Table 3, the ΔG° values are negative for all temperatures, indicating that MO adsorbed spontaneously onto CuO/NaA and that the system does not gain energy from an external source. The positive value of ΔH° further confirms the endothermic nature of MO adsorption, while positive entropy (ΔS°) indicates the increased randomness with MO adsorption, probably because the number of desorbed water molecules is larger than that of adsorbed MO molecules.

T (K)	Thermodynamic parameters
	ΔG° (kJ/mol)	ΔH° (kJ/mol)	ΔS° (J/mol K)
298	–16.265
308	–17.103	8.705	83.797
318	–17.941
328	–18.779

3.6 Photocatalysis

It is worthwhile to outline that MO (with a concentration of 100 mg/L) was partially adsorbed (88%). So, the remaining concentration was subjected to visible illumination. The kinetic was studied by withdrawing aliquots at regular time intervals. Fig. 13 clearly shows that MO photodegradation obeys a first-order kinetic with a rate constant of 7.47 ×10⁻³ min⁻¹ and a removal percentage of 76%.

Fig. 13
a: MO photodegradation by CuO/NaA; b: photocatalytic degradation kinetic of MO (MO = 12 mg/L, pH ∼ 7, catalyst dose = 2 g/L and T = 298 K).

From Table 4, comparing the maximum adsorption capacities q_m (mg/g) of MO on different adsorbents, shows that the CuO supported on NaA zeolite performs considerably better than the other ones.

Adsorbent	q_m (mg/g)	Reference
γ-Fe₂O₃/SiO₂/CS composite	34.29	[1]
CuO/NaA zeolite	79.49	This study
Carbon coated monolith	27.2	[5]
Hypercrosslinked polymeric	76.92	[25]
Multiwalled carbon nanotubes	52.86	[27]
Natural zeolite modified with hexamethylenediamine	33.0	[28]
Surfactant modified silkworm exuviae	87.03	[31]
De-oiled soya	13.46	[32]

4 Conclusion

CuO supported on a NaA zeolite was elaborated by an exchange method and characterized by X-ray diffraction and scanning electron microscopy. The physical parameters of the adsorption of methyl orange, like the solution pH, the dose of catalyst, the MO concentration and temperature were optimized. The data were well fitted by the Langmuir model. The disappearance of MO follows a second-order kinetic, and the thermodynamic parameters indicate a spontaneous and endothermic process. The catalyst CuO/NaA has been successfully tested for the photodegradation of methyl orange under visible light.

Bibliographie

[1] H.Y. Zhu; R. Jiang; L. Xiao Appl. Clay Sci., 48 (2010), p. 522

[2] A. Ansafi; M. Khemis; M.N. Pons; J.-P. Leclerc; A. Yaacoubi; A. Ben hammou; A. Nejmeddine Chem. Eng. Proc., 44 (2005), p. 461

[3] J. Guo; D. Jiang; Y. Wu; P. Zhou; Y. Lan J. Hazard. Mater., 194 (2011), p. 290

[4] Y.S. Jeon; J. Lei; J.H. Kim J. Ind. Eng. Chem., 14 (2008), p. 726

[5] S. Hosseini; M.A. Khan; M.R. Malekbala; W. Cheah; T.S.Y. Choong Chem. Eng. J., 171 (2011), p. 1124

[6] W.L. Sun; Y.Z. Qu; Q. Yu; J.R. Ni J. Hazard. Mater., 154 (2008), p. 595

[7] Q. Zhang; K. Zhang; D. Xu; G. Yang; H. Huang; F. Nie; Ch. Liu; S. Yang Progress. Mater. Sci., 60 (2014), p. 208

[8] S.C. Yeon; W.Y. Sung; W.J. Kim; S.M. Lee; H.Y. Lee; Y.H. Kim J. Vac. Sci. Technol. B, 24 (2006), p. 940

[9] C.T. Hsieh; J.M. Chen; H.H. Lin; H.C. Shih Appl. Phys. Lett., 83 (2003), p. 3383

[10] Y.J. Mu; J. Yang; S. Han; H.W. Hou; Y.T. Fan Mater. Lett., 64 (2010), p. 1287

[11] P. Sathishkumar; R. Sweena; J.J. Wu; S. Anandan Chem. Eng. J., 171 (2011), p. 136

[12] W. Xu; H. Wang; X. Zhou; T. Zhu Chem. Eng. J., 243 (2014), p. 380

[13] P. Khemthong; P. Photai; N. Grisdanurak Int. J. Hydrogen Energy, 38 (2013), p. 15992

[14] J.H. Jeun; S.H. Hong Sens. Actuators, B: Chem., 151 (2010), p. 1

[15] R. Saravanan; S. Karthikeyan; V.K. Gupta; G. Sekaran; V. Narayanan; A. Stephen Mat. Sci. Eng. C, 33 (2013), p. 91

[16] J.L. Cao; G.S. Shao; Y. Wang; Y. Liu; Z.Y. Yuan Catal. Commun., 9 (2008), p. 2555

[17] Sh. Sohrabnezhad; M.J.M. Moghaddam; T. Salavatiyan Spectrochim. Acta Part A: Mol. Biomol. Spectrosc., 125 (2014), p. 73

[18] D. Nibou; H. Mekatel; S. Amokrane; M. Barakat; M. Trari J. Hazard. Mater., 173 (2010), p. 637

[19] H. Mekatel; S. Amokrane; B. Bellal; M. Trari; D. Nibou Chem. Eng. J., 200–202 (2012), p. 611

[20] S. Asuha; X.G. Zhou; S. Zhao J. Hazard. Mater., 181 (2010), p. 204

[21] S. Chen; J. Zhang; C. Zhang; Q. Yue; Y. Li; C. Li Desalination, 252 (2010), p. 149

[22] A. Mittal; A. Malviya; D. Kaur; J. Mittal; L. Kurup J. Hazard. Mater., 148 (2007), p. 229

[23] H.Y. Zhu; R. Jiang; Y.Q. Fu; J.H. Jiang; L. Xiao; G.M. Zeng Appl. Surf. Sci., 258 (2011), p. 1337

[24] N. Mohammadi; H. Khani; V.K. Gupta; E. Amereh; S. Agarwal J. Colloid Interf. Sci., 362 (2011), p. 457

[25] J.H. Huang; K.L. Huang; S.Q. Liu; A. Ting Wang; C. Yan Colloids Surf. A: Physicochem. Eng. Aspects, Volume 330 (2008), p. 55

[26] D. Chen; J. Chen; X. Luan; H. Ji; Z. Xia Chem. Eng. J., 171 (2011), p. 1150

[27] Y. Yao; B. He; F. Xu; X. Chen Chem. Eng. J., 170 (2011), p. 82

[28] E. Alver; A.U. Metin Chem. Eng. J., 200–202 (2012), p. 59

[29] E. Haque; J.W. Jun; S.H. Jhung J. Hazard. Mater., 185 (2011), p. 507

[30] M. Barkat; D. Nibou; S. Chegrouche; A. Mellah Chem. Eng. Proc., 48 (2009), p. 38

[31] A. Mittal; A. Malviya; D. Kaur; J. Mittal; L. Kurup J. Hazard. Mater., 148 (2007), pp. 229-240

[32] H. Chen; J. Zhao; J. Wu; G. Dai J. Hazard. Mater., 192 (2011), p. 246

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