Plan
Comptes Rendus

GeCat 2014: Advances and prospects in heterogeneous catalysis
Adsorption of methyl orange on nanoparticles of a synthetic zeolite NaA/CuO
Comptes Rendus. Chimie, GECat 2014 – Advances and prospects in heterogeneous catalysis, Volume 18 (2015) no. 3, pp. 336-344.

Résumés

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. ΔGo, ΔHo, and ΔSo, 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 ΔGo, ΔHo and ΔSo 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 :
Accepté le :
Publié le :
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

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
@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},
}
TY  - JOUR
AU  - El Hadj Mekatel
AU  - Samira Amokrane
AU  - Asma Aid
AU  - Djamel Nibou
AU  - Mohamed Trari
TI  - Adsorption of methyl orange on nanoparticles of a synthetic zeolite NaA/CuO
JO  - Comptes Rendus. Chimie
PY  - 2015
SP  - 336
EP  - 344
VL  - 18
IS  - 3
PB  - Elsevier
DO  - 10.1016/j.crci.2014.09.009
LA  - en
ID  - CRCHIM_2015__18_3_336_0
ER  - 
%0 Journal Article
%A El Hadj Mekatel
%A Samira Amokrane
%A Asma Aid
%A Djamel Nibou
%A Mohamed Trari
%T Adsorption of methyl orange on nanoparticles of a synthetic zeolite NaA/CuO
%J Comptes Rendus. Chimie
%D 2015
%P 336-344
%V 18
%N 3
%I Elsevier
%R 10.1016/j.crci.2014.09.009
%G en
%F CRCHIM_2015__18_3_336_0
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, GECat 2014 – Advances and prospects in heterogeneous catalysis, 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

Le texte intégral ci-dessous peut contenir quelques erreurs de conversion par rapport à la version officielle de l'article publié.

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, λmax = 465 nm). The percentage of MO removal was calculated using the relationship:

RemovalofMO(%)=CoCeCo×100(1)
where Co and Ce are the initial and equilibrium MO concentrations (mg/L), respectively. The adsorption capacity of the adsorbent material, qt (mg/g), was determined using the relationship:
qt=CoCeVm(2)
qt 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 (Kd) is given by [19]:
Kd=CoCemCeV(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 pHs 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]:

Ceqe=1qmb+Ceqm(4)
where Ce is equilibrium concentration of MO (mg/L) and qe is the amount of adsorbed MO (mg/g). The monolayer adsorption capacity (qm, 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 Ce/qe versus Ce, 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.

Table 1

Comparison of the equilibrium isotherm models.

Langmuir
qm (mg/g)79.49
b (L/mg)0.108
R20.995
Freundlich
KF (mg/g)19.636
n3.28
R20.979
Temkin
bT (J/mol)182.317
AT (L/g)2.492
R20.955

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

lnqe=lnKF+1nlnCe(5)
where KF (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 KF and n were determined from the intercept and slope of the linear plot of ln qe versus ln Ce, 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 qe against ln Ce [Eq. (6)]:

qe=B   ln   AT+B   ln   Ce(6)

where AT (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, qm, 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]:

dqdt=k1qeqt(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 qt = 0 to qt) becomes:
lnqeqt=ln   qek1t(8)

The values of k1 can be obtained from the slope of the linear plot of lnqeqt versus t.

3.4.2 Pseudo-second-order model

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

dqdt=k2qeqt2(9)
where k2 is the pseudo-second-order adsorption rate coefficient (g/mg/min). For the boundary conditions (t = 0 to t and qt = 0 to qt), Eq. (9) becomes:
tqt=1(k2qe2)+1qet(10)

The plots of t/qt versus time (t) for different concentrations (Co) and various temperatures fit well with the experimental data and provide the rate constants k2 and qe. 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 qe 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 (Co); (b) different temperatures.

Fig. 10

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

Table 2

Pseudo-first-order and pseudo-second-order models constants for the adsorption of MO on CuO/NaA under different initial concentrations and different temperatures.

Pseudo-first-orderPseudo-second-order
qecal
(mg/g)
k1 × 102
(min−1)
R2qecal
(mg/g)
k2 × 104
(g·mg−1·min−1)
R2
MO (mg/L)
 5031.741.480.94131.843.220.994
 10044.531.190.99054.052.210.997
 15055.491.510.89976.921.570.996
 20075.071.400.99286.201.620.995
 25066.631.140.97590.091.690.997
T (K)
 29831.761.080.945872.675.180.9989
 30861.721.070.998898.911.940.9965
 31863.251.280.9006101.012.810.9961
 32848.581.030.9879102.463.190.9962

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 (Ea) follows the Arrhenius equation [30]:

k2=Aoexp(Ea/RT)(11)

the linearization gives:

ln   k2=Ea/R   1/T+ln   Ao(12)
where R (8.314 J/mol·K) is the universal gas constant and Ao is a pre-exponential factor. The slope of plot ln k2 versus 1/T (Fig. 11) gives an activation energy Ea (20.98 kJ/mol) that indicates physical adsorption [18,30].

Fig. 11

Determination of the adsorption activation energy (Ea).

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 Kd versus 1/T curve according to Eq. (12) (Fig. 12) [18]:

ln   Kd=ΔSRΔHRT(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.

Table 3

Thermodynamic parameters for the adsorption of MO onto CuO/NaA at different temperatures (MO = 50 mg/L, pH ∼ 7, dose of catalyst = 1 g/L).

T (K)Thermodynamic parameters
ΔG° (kJ/mol)ΔH° (kJ/mol)ΔS° (J/mol K)
298–16.265
308–17.1038.70583.797
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 qm (mg/g) of MO on different adsorbents, shows that the CuO supported on NaA zeolite performs considerably better than the other ones.

Table 4

Comparison of maximum adsorption capacities qm (mg/g) of MO onto different adsorbents.

Adsorbentqm (mg/g)Reference
γ-Fe2O3/SiO2/CS composite34.29[1]
CuO/NaA zeolite79.49This study
Carbon coated monolith27.2[5]
Hypercrosslinked polymeric76.92[25]
Multiwalled carbon nanotubes52.86[27]
Natural zeolite modified with hexamethylenediamine33.0[28]
Surfactant modified silkworm exuviae87.03[31]
De-oiled soya13.46[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


Cité par

  • Lynda Jmai; Sami Guiza; Salah Jellali; Mohamed Bagane; Mejdi Jeguirim Synthesis of a novel biocomposite from orange peels and its application for the removal of diclofenac from aqueous solutions: assessment of adsorption characteristics, Comptes Rendus. Chimie, Volume 28 (2025) no. G1, p. 225 | DOI:10.5802/crchim.381
  • Younes Dehmani; Dison S.P. Franco; Jordana Georgin; Redouane Mghaiouini; Bouchra Ba Mohammed; Rachid Kacimi; Taibi Lamhasni; Eder C. Lima; Noureddine El Messaoudi; Abouarnadasse Sadik Towards a deeper understanding of the adsorption of methyl orange on a commercial activated carbon: Study of impact factors, isotherm and mechanism, Environmental Surfaces and Interfaces, Volume 3 (2025), p. 103 | DOI:10.1016/j.esi.2025.02.002
  • Shuyu Wang; Xiaohui Wu; Lijuan Ren; Xian Pei; Hui Fang; Ping Lv; Ning Nan; Xianwei Lv; Xianming Zheng; Feihe Ma; Yun Wu; Yuping Liu; Linqi Shi Clew-like Cu2O/CuO Microsphere Adsorbents for Highly Efficient Anionic Dye Removal, Langmuir, Volume 41 (2025) no. 4, p. 2364 | DOI:10.1021/acs.langmuir.4c04019
  • Mohamed Zayed; Mervat Nasr; Mamduh J. Aljaafreh; Mohammad Marashdeh; M. Al-Hmoud; Mohamed Shaban; Mohamed Rabia; Amna Tarek; Ashour M. Ahmed Sodium titanium oxide/zinc oxide (STO/ZnO) photocomposites for efficient dye degradation applications, Green Processing and Synthesis, Volume 13 (2024) no. 1 | DOI:10.1515/gps-2023-0272
  • Djamaa Zoulikha; Bouras Brahim; Labied Radia; Bachari Khaldoun; Lerari Djahida Modeling the Kinetics, Equilibrium and Thermodynamics of Poly(acrylamide)/Sodium-Bentonite for Enhanced Phenol Removal from Aqueous Media, Journal of Macromolecular Science, Part B (2024), p. 1 | DOI:10.1080/00222348.2024.2366744
  • Najib Meftah Almukhtar Omar; Mohd Hafiz Dzarfan Othman; Zhong Sheng Tai; Jerry Y. Y. Heng; Tonni Agustiono Kurniawan; Mohd Hafiz Puteh; Suriani Abu Bakar; Juhana Jaafar; Mukhlis A. Rahman A review of the latest progress in superhydrophobic surface technology using copper oxide nanoparticles, Journal of Materials Science, Volume 59 (2024) no. 41, p. 19450 | DOI:10.1007/s10853-024-10352-w
  • Mobinul Islam; Md. Shahriar Ahmed; Sua Yun; Hae-Yong Kim; Kyung-Wan Nam Harnessing Radiation for Nanotechnology: A Comprehensive Review of Techniques, Innovations, and Application, Nanomaterials, Volume 14 (2024) no. 24, p. 2051 | DOI:10.3390/nano14242051
  • Hammoudi Hadda Aya; Nibou Djamel; Amokrane Samira; Marta Otero; Moonis Ali Khan Optimizing methylene blue adsorption conditions on hydrothermally synthesized NaX zeolite through a full two-level factorial design, RSC Advances, Volume 14 (2024) no. 33, p. 23816 | DOI:10.1039/d4ra04483e
  • Kristina Filipović; Miloš Kostić; Slobodan Najdanović; Miljana Radović-Vučić; Nena Velinov; Danijela Bojić; Aleksandar Bojić Effects of pH, contact time and initial dye concentration on methyl orange sorption via layered double hydroxides, Advanced Technologies, Volume 12 (2023) no. 1, p. 75 | DOI:10.5937/savteh2301075f
  • Nnabuk Okon Eddy; Rajni Garg; Rishav Garg; Augustine O. Aikoye; Benedict I. Ita Waste to resource recovery: mesoporous adsorbent from orange peel for the removal of trypan blue dye from aqueous solution, Biomass Conversion and Biorefinery, Volume 13 (2023) no. 15, p. 13493 | DOI:10.1007/s13399-022-02571-5
  • Ruolin Wang; Zhiting Wu; Xiying Chen; Baijie Cheng; Wenhua Ou Water purification using a BiVO4/graphene oxide multifunctional hydrogel based on interfacial adsorption-enrichment and photocatalytic antibacterial activity, Ceramics International, Volume 49 (2023) no. 6, p. 9657 | DOI:10.1016/j.ceramint.2022.11.137
  • Lébé Prisca Marie-Sandrine Kouakou; Daouda Karidioula; Max Robin Wedjers Manouan; Aliou Guillaume Lemeyonouin Pohan; Gaoussou Cissé; Léon Koffi Konan; Jonas Yao Andji-Yapi Use of two clays from Côte d'Ivoire for the adsorption of methyl red from aqueous medium, Chemical Physics Letters, Volume 810 (2023), p. 140183 | DOI:10.1016/j.cplett.2022.140183
  • Nnabuk Okon Eddy; Unwana Edo Edet; Joseph Olusola Oladele; Herientta Ijeoma Kelle; Emeka Chima Ogoko; Anduang O Odiongenyi; Paul Ameh; Richard Alexis Ukpe; Raphael Ogbodo; Rajni Garg; Rishav Garg Synthesis and application of novel microporous framework of nanocomposite from trona for photocatalysed degradation of methyl orange dye, Environmental Monitoring and Assessment, Volume 195 (2023) no. 12 | DOI:10.1007/s10661-023-12014-x
  • Chunyan Cao; Weiwei Xuan; Shiying Yan; Qi Wang Zeolites synthesized from industrial and agricultural solid waste and their applications: A review, Journal of Environmental Chemical Engineering, Volume 11 (2023) no. 5, p. 110898 | DOI:10.1016/j.jece.2023.110898
  • Jaqueline F. de Souza; Emilly C. da Silva; André F. P. Biajoli; Daísa H. Bonemann; Anderson S. Ribeiro; André R. Fajardo Alginate/Phosphine-Functionalized Chitosan Beads Towards the Removal of Harmful Metal Ions from Aqueous Medium, Journal of Polymers and the Environment, Volume 31 (2023) no. 1, p. 249 | DOI:10.1007/s10924-022-02599-8
  • Alvin Romadhoni Putra Hidayat; Liyana Labiba Zulfa; Alvin Rahmad Widyanto; Romario Abdullah; Yuly Kusumawati; Ratna Ediati Selective adsorption of anionic and cationic dyes on mesoporous UiO-66 synthesized using a template-free sonochemistry method: kinetic, isotherm and thermodynamic studies, RSC Advances, Volume 13 (2023) no. 18, p. 12320 | DOI:10.1039/d2ra06947d
  • Yunfeng Tan; Yangyang Zhang; Bo Zu; Yunxia Zhang; Chunli Zheng; Kejun Chen Removal of Methyl Orange in Aqueous Solutions Using Hydrochloric Acid-Modified Kaolinite Supported Nanosized Zero-Valent Iron, Water, Air, Soil Pollution, Volume 234 (2023) no. 7 | DOI:10.1007/s11270-023-06417-2
  • Abdelhay El Amri; Jaouad Bensalah; Abdennacer Idrissi; Kadiri Lamya; Abdelkarim Ouass; Said Bouzakraoui; Abdelkader Zarrouk; El Housseine Rifi; Ahmed Lebkiri Adsorption of a cationic dye (Methylene bleu) by Typha Latifolia: Equilibrium, kinetic, thermodynamic and DFT calculations, Chemical Data Collections, Volume 38 (2022), p. 100834 | DOI:10.1016/j.cdc.2022.100834
  • Xisen Wang; Jessica Baker; Kristen Carlson; Zhaohui Li Mechanisms of Selected Anionic Dye Removal by Clinoptilolite, Crystals, Volume 12 (2022) no. 5, p. 727 | DOI:10.3390/cryst12050727
  • Qamar Riaz; Madiha Ahmed; Muhammad Nadeem Zafar; Muhammad Zubair; Muhammad Faizan Nazar; Sajjad Hussain Sumrra; Iqbal Ahmad; Ahmad Hosseini-Bandegharaei NiO nanoparticles for enhanced removal of methyl orange: equilibrium, kinetics, thermodynamic and desorption studies, International Journal of Environmental Analytical Chemistry, Volume 102 (2022) no. 1, p. 84 | DOI:10.1080/03067319.2020.1715383
  • Tomohiro Iwasaki; Yasuyuki Shimamura Experimental analysis of synthesis process of lanthanum nickelate nanoparticles as an anionic dye adsorbent via a coprecipitation–flux method, Journal of Environmental Chemical Engineering, Volume 10 (2022) no. 1, p. 107113 | DOI:10.1016/j.jece.2021.107113
  • Madhu Agarwal; Karishma Maheshwari; Yogendra Singh Solanki Investigation of Dye Effluent Treatment Using Unmodified and Modified Biobased Sorbent and Its Process Economics, Journal of Hazardous, Toxic, and Radioactive Waste, Volume 26 (2022) no. 1 | DOI:10.1061/(asce)hz.2153-5515.0000650
  • Jin Hou; Yongcheng Ye Design of Copper Oxide Nanosheets-Loaded Zeolite with Efficient Inhibition of Marine Bacteria, Journal of Ocean University of China, Volume 21 (2022) no. 5, p. 1237 | DOI:10.1007/s11802-022-5240-7
  • Ahmed Zaghloul; Ridouan Benhiti; Hassan Ait Ahsaine; Amina Soudani; Amal BaQais; Mohamed Chiban; Fouad Sinan RETRACTED ARTICLE: Fabrication, characterization and competitive study of toxic dyes adsorption onto Mg3Al-CO32− clay adsorbent, Nanotechnology for Environmental Engineering, Volume 7 (2022) no. 4, p. 955 | DOI:10.1007/s41204-022-00245-1
  • Abiodun Musa Aibinu; Taliha Abiodun Folorunso; Abdulkareem Ambali Saka; Lawal Adewale Ogunfowora; Kingsley O. Iwuozor; Joshua O. Ighalo Green synthesis of CuO nanocomposite from watermelon (Citrullus lanatus) rind for the treatment of aquaculture effluent, Regional Studies in Marine Science, Volume 52 (2022), p. 102308 | DOI:10.1016/j.rsma.2022.102308
  • Soumya Ranjan Mishra; Md. Ahmaruzzaman CuO and CuO-based nanocomposites: Synthesis and applications in environment and energy, Sustainable Materials and Technologies, Volume 33 (2022), p. e00463 | DOI:10.1016/j.susmat.2022.e00463
  • Mostafa R. Abukhadra; Merna Mostafa; Ahmed M. El-Sherbeeny; Mohammed A. El-Meligy; Ahmed Nadeem Instantaneous Adsorption of Synthetic Dyes from an Aqueous Environment Using Kaolinite Nanotubes: Equilibrium and Thermodynamic Studies, ACS Omega, Volume 6 (2021) no. 1, p. 845 | DOI:10.1021/acsomega.0c05430
  • Nilay Baylan; Tuba Dedecan; İrem İlalan; İsmail İnci Preparation of Copper Oxide Nanoparticles as a Novel Adsorbent for the Isolation of Tartaric Acid, Analytical Letters, Volume 54 (2021) no. 13, p. 2113 | DOI:10.1080/00032719.2020.1842434
  • Dimitra Das; Amit Kuamr Sharma; Kalyan Kumar Chattopadhyay; Diptonil Banerjee Dye Removal Ability of Pure and Doped Graphitic Carbon Nitride, Current Analytical Chemistry, Volume 18 (2021) no. 3, p. 309 | DOI:10.2174/1573411017666210108092850
  • Kingsley O. Iwuozor; Joshua O. Ighalo; Ebuka Chizitere Emenike; Lawal Adewale Ogunfowora; Chinenye Adaobi Igwegbe Adsorption of methyl orange: A review on adsorbent performance, Current Research in Green and Sustainable Chemistry, Volume 4 (2021), p. 100179 | DOI:10.1016/j.crgsc.2021.100179
  • Ahmed Zaghloul; Ridouan Benhiti; Rachid Aziam; Abdeljalil Ait Ichou; Mhamed Abali; Amina Soudani; Fouad Sinan; Mohamed Zerbet; Mohamed Chiban A Brief Comparative Study on Removal of Toxic Dyes by Different Types of Clay, Dyes and Pigments - Novel Applications and Waste Treatment (2021) | DOI:10.5772/intechopen.95755
  • S Mustapha; JO Tijani; MM Ndamitso; AS Abdulkareem; DT Shuaib; A.K Mohammed Adsorptive removal of pollutants from industrial wastewater using mesoporous kaolin and kaolin/TiO2 nanoadsorbents, Environmental Nanotechnology, Monitoring Management, Volume 15 (2021), p. 100414 | DOI:10.1016/j.enmm.2020.100414
  • Joshua O. Ighalo; Patience A. Sagboye; Great Umenweke; Oluwaseun J. Ajala; Fredrick O. Omoarukhe; Comfort A. Adeyanju; Samuel Ogunniyi; Adewale G. Adeniyi CuO nanoparticles (CuO NPs) for water treatment: A review of recent advances, Environmental Nanotechnology, Monitoring Management, Volume 15 (2021), p. 100443 | DOI:10.1016/j.enmm.2021.100443
  • Alvin Romadhoni Putra Hidayat; Dety Oktavia Sulistiono; Irmina Kris Murwani; Budiani Fitria Endrawati; Hamzah Fansuri; Liyana Labiba Zulfa; Ratna Ediati Linear and nonlinear isotherm, kinetic and thermodynamic behavior of methyl orange adsorption using modulated Al2O3@UiO-66 via acetic acid, Journal of Environmental Chemical Engineering, Volume 9 (2021) no. 6, p. 106675 | DOI:10.1016/j.jece.2021.106675
  • Juliê S. da Costa; Emanuel G. Bertizzolo; Daniela Bianchini; André R. Fajardo Adsorption of benzene and toluene from aqueous solution using a composite hydrogel of alginate-grafted with mesoporous silica, Journal of Hazardous Materials, Volume 418 (2021), p. 126405 | DOI:10.1016/j.jhazmat.2021.126405
  • Sher Ali Shah; Zubair Ahmad; Shahid Ali Khan; Youssef O. Al-Ghamdi; Esraa M. Bakhsh; Noureen Khan; Mujeeb ur Rehman; Mahjoub Jabli; Sher Bahadar Khan Biomass impregnated zero-valent Ag and Cu supported-catalyst: Evaluation in the reduction of nitrophenol and discoloration of dyes in aqueous medium, Journal of Organometallic Chemistry, Volume 938 (2021), p. 121756 | DOI:10.1016/j.jorganchem.2021.121756
  • R. Ediati; W. Aulia; B.A. Nikmatin; A.R.P. Hidayat; U.M. Fitriana; C. Muarifah; D.O. Sulistiono; F. Martak; D. Prasetyoko Chitosan/UiO-66 composites as high-performance adsorbents for the removal of methyl orange in aqueous solution, Materials Today Chemistry, Volume 21 (2021), p. 100533 | DOI:10.1016/j.mtchem.2021.100533
  • Ahmed Zaghloul; Ridouan Benhiti; Abdeljalil Ait Ichou; Gabriela Carja; Amina Soudani; Mohamed Zerbet; Fouad Sinan; Mohamed Chiban Characterization and application of MgAl layered double hydroxide for methyl orange removal from aqueous solution, Materials Today: Proceedings, Volume 37 (2021), p. 3793 | DOI:10.1016/j.matpr.2020.07.676
  • Kingsley Ogemdi Iwuozor; Joshua O. Ighalo; Ebuka Chizitere Emenike; Lawal Adewale Ogunfowora; Chinenye Igwegbe Adsorption of Methyl Orange: An Empirical Study on Adsorbent Performance, SSRN Electronic Journal (2021) | DOI:10.2139/ssrn.3903971
  • Truong Thi Phuong Nguyet Xuan Trinh; Do Minh Nguyet; Tran Hoang Quan; Trinh Ngoc Minh Anh; Doan Ba Thinh; Le Tan Tai; Nguyen Thi Lan; Dinh Ngoc Trinh; Nguyen Minh Dat; Hoang Minh Nam; Mai Thanh Phong; Nguyen Huu Hieu Preparing three-dimensional graphene aerogels by chemical reducing method: Investigation of synthesis condition and optimization of adsorption capacity of organic dye, Surfaces and Interfaces, Volume 23 (2021), p. 101023 | DOI:10.1016/j.surfin.2021.101023
  • Adewale Adewuyi; Claudio A. Gervasi; María V. Mirífico Synthesis of strontium ferrite and its role in the removal of methyl orange, phenolphthalein and bromothymol blue from laboratory wastewater, Surfaces and Interfaces, Volume 27 (2021), p. 101567 | DOI:10.1016/j.surfin.2021.101567
  • Mansouri Taki Eddine Mohammed; Nibou Djamel; Trari Mohamed; Samira Amokrane Study of the adsorption of an organic pollutant onto a microporous metal organic framework, Water Science and Technology, Volume 83 (2021) no. 1, p. 137 | DOI:10.2166/wst.2020.566
  • Mohammad Shahedur Rahman Adsorption of Methyl Blue onto Activated Carbon Derived from Red Oak (Quercus rubra) Acorns: a 26 Factorial Design and Analysis, Water, Air, Soil Pollution, Volume 232 (2021) no. 1 | DOI:10.1007/s11270-020-04943-x
  • Essam A. Mohamed; Ali Q. Selim; Sayed A. Ahmed; Lotfi Sellaoui; Adrián Bonilla-Petriciolet; Alessandro Erto; Zichao Li; Yanhui Li; Moaaz K. Seliem H2O2-activated anthracite impregnated with chitosan as a novel composite for Cr(VI) and methyl orange adsorption in single-compound and binary systems: Modeling and mechanism interpretation, Chemical Engineering Journal, Volume 380 (2020), p. 122445 | DOI:10.1016/j.cej.2019.122445
  • Zaharaddeen N. Garba; Weiming Zhou; Mingxi Zhang; Zhanhui Yuan A review on the preparation, characterization and potential application of perovskites as adsorbents for wastewater treatment, Chemosphere, Volume 244 (2020), p. 125474 | DOI:10.1016/j.chemosphere.2019.125474
  • Umair Baig; Mohammad Kashif Uddin; M.A. Gondal Removal of hazardous azo dye from water using synthetic nano adsorbent: Facile synthesis, characterization, adsorption, regeneration and design of experiments, Colloids and Surfaces A: Physicochemical and Engineering Aspects, Volume 584 (2020), p. 124031 | DOI:10.1016/j.colsurfa.2019.124031
  • Arup Roy Microwave‐assisted synthesis of mesoporous γ‐Fe2O3 for dye removal, Micro Nano Letters, Volume 15 (2020) no. 13, p. 943 | DOI:10.1049/mnl.2020.0012
  • Muhammad Asif Raja; Azamal Husen Role of nanomaterials in soil and water quality management, Nanomaterials for Agriculture and Forestry Applications (2020), p. 491 | DOI:10.1016/b978-0-12-817852-2.00020-2
  • Mekatel Elhadj; Amokrane Samira; Trari Mohamed; Ferhat Djawad; Aid Asma; Nibou Djamel Removal of Basic Red 46 dye from aqueous solution by adsorption and photocatalysis: equilibrium, isotherms, kinetics, and thermodynamic studies, Separation Science and Technology, Volume 55 (2020) no. 5, p. 867 | DOI:10.1080/01496395.2019.1577896
  • Yousef Rashtbari; Juliana Heloisa Pinê Américo-Pinheiro; Shima Bahrami; Mehdi Fazlzadeh; Hossein Arfaeinia; Yousef Poureshgh Efficiency of Zeolite Coated with Zero-Valent Iron Nanoparticles for Removal of Humic Acid from Aqueous Solutions, Water, Air, Soil Pollution, Volume 231 (2020) no. 10 | DOI:10.1007/s11270-020-04872-9
  • Elhadj Mekatel; Samira Amorkrane; Mohamed Trari; Djamel Nibou; Nadjib Dahdouh; Samir Ladjali Combined Adsorption/Photocatalysis Process for the Decolorization of Acid Orange 61, Arabian Journal for Science and Engineering, Volume 44 (2019) no. 6, p. 5311 | DOI:10.1007/s13369-018-3575-6
  • Zakaria Anfar; Mohamed Zbair; Hassan Ait Ahsaine; Youness Abdellaoui; Abdellah Ait El Fakir; El Hassan Amaterz; Amane Jada; Noureddine El Alem Preparation and Characterization of Porous Carbon@ZnO‐NPs for Organic Compounds Removal: Classical Adsorption Versus Ultrasound Assisted Adsorption, ChemistrySelect, Volume 4 (2019) no. 17, p. 4981 | DOI:10.1002/slct.201901043
  • Wenjuan Xu; Zhichao Shao; Chao Huang; Ruixue Xu; Bingzhe Dong; Hongwei Hou Alkenone-enol-alkenone [2+2+2] Cyclotrimerization Producing Functional Coordination Polymers with Excellent Adsorption Performance, Inorganic Chemistry, Volume 58 (2019) no. 6, p. 3959 | DOI:10.1021/acs.inorgchem.9b00037
  • Nazia Rahman; Nirmal Chandra Dafader; Abdur Rahim Miah; S. Shahnaz Efficient removal of methyl orange from aqueous solution using amidoxime adsorbent, International Journal of Environmental Studies, Volume 76 (2019) no. 4, p. 594 | DOI:10.1080/00207233.2018.1494930
  • Radouane Laib; Samira Amokrane-Nibou; Djamel Nibou; Mohamed Trari Recovery of recycled paper in the removal of the textile dye basic yellow 28: characterization and adsorption studies, Nordic Pulp Paper Research Journal, Volume 34 (2019) no. 2, p. 218 | DOI:10.1515/npprj-2018-0071
  • Jian Liu; Quan Yin; Huiping Zhang; Ying Yan; Zhengji Yi Continuous removal of Cr(VI) and Orange II over a novel Fe0-NaA zeolite membrane catalyst, Separation and Purification Technology, Volume 209 (2019), p. 734 | DOI:10.1016/j.seppur.2018.07.030
  • Bayram ÇİMEN; Sonya ŞENGÜL; Memduha ERGÜT; Ayla ÖZER CuO Nanopartiküllerinin Yeşil Sentezi ve Karakterizasyonu: Telon Blue AGLF ve Metilen Mavisi Adsorpsiyonu, Sinop Üniversitesi Fen Bilimleri Dergisi, Volume 4 (2019) no. 1, p. 1 | DOI:10.33484/sinopfbd.315643
  • Priya Kumari; Masood Alam; Weqar Ahmed Siddiqi Usage of nanoparticles as adsorbents for waste water treatment: An emerging trend, Sustainable Materials and Technologies, Volume 22 (2019), p. e00128 | DOI:10.1016/j.susmat.2019.e00128
  • G. Mecheri; S. Hafsi; N. Gherraf Preparation and characterization of a porous material from an Algerian desert sand, Acta Scientifica Naturalis, Volume 5 (2018) no. 2, p. 48 | DOI:10.2478/asn-2018-0020
  • Y. Azoudj; Z. Merzougui; G. Rekhila; M. Trari The adsorption of HCrO4− on activated carbon of date pits and its photoreduction on the hetero-system ZnCo2O4/TiO2, Applied Water Science, Volume 8 (2018) no. 4 | DOI:10.1007/s13201-018-0755-1
  • Mohammad Nikpassand; Leila Zare Fekri; Afshin Pourahmad One-pot Synthesis of new azo-linked 4H-benzo[d][1,3]oxazine-2,4-diones from carbon dioxide using CuO@RHA/MCM-41 nanocomposite in green media, Journal of CO2 Utilization, Volume 27 (2018), p. 320 | DOI:10.1016/j.jcou.2018.08.011
  • Mohamed Mobarak; Ali Q. Selim; Essam A. Mohamed; Moaaz K. Seliem A superior adsorbent of CTAB/H2O2 solution−modified organic carbon rich-clay for hexavalent chromium and methyl orange uptake from solutions, Journal of Molecular Liquids, Volume 259 (2018), p. 384 | DOI:10.1016/j.molliq.2018.02.014
  • Dilek Gümüş; Fatih Gümüş Potasyum permanganat kaplı zeolit ve demir oksit kaplı zeolitle metil oranjın adsorpsiyon çalışmaları, Kahramanmaraş Sütçü İmam Üniversitesi Mühendislik Bilimleri Dergisi, Volume 21 (2018) no. 1, p. 43 | DOI:10.17780/ksujes.342939
  • Nitin Goyal; Sanghamitra Barman; Vijaya Kumar Bulasara Efficient removal of bisphenol S from aqueous solution by synthesized nano-zeolite secony mobil-5, Microporous and Mesoporous Materials, Volume 259 (2018), p. 184 | DOI:10.1016/j.micromeso.2017.10.015
  • Farheen Khan; Rizwan Wahab; Mohamed Hagar; Rua Alnoman; Lutfullah; Mohd Rashid Nanotransition Materials (NTMs): Photocatalysis, Validated High Effective Sorbent Models Study for Organic Dye Degradation and Precise Mathematical Data’s at Standardized Level, Nanomaterials, Volume 8 (2018) no. 3, p. 134 | DOI:10.3390/nano8030134
  • Asma Aid; Samira Amokrane; Djamel Nibou; Elhadj Mekatel; Mohamed Trari; Vasile Hulea Modeling biosorption of Cr(VI) onto Ulva compressa L. from aqueous solutions, Water Science and Technology, Volume 77 (2018) no. 1, p. 60 | DOI:10.2166/wst.2017.509
  • Shuangzhen Guo; Jian Zhang; Xianlong Li; Fan Zhang; Xixi Zhu Fe3O4-CS-L: a magnetic core-shell nano adsorbent for highly efficient methyl orange adsorption, Water Science and Technology, Volume 77 (2018) no. 3, p. 628 | DOI:10.2166/wst.2017.602
  • Muhammad Imran Khan; Muhammad Ali Khan; Shagufta Zafar; Muhammad Naeem Ashiq; Muhammad Athar; Ashfaq Mahmood Qureshi; Muhammad Arshad Kinetic, equilibrium and thermodynamic studies for the adsorption of methyl orange using new anion exchange membrane (BII), Desalination and Water Treatment, Volume 58 (2017), p. 285 | DOI:10.5004/dwt.2017.1715
  • Mohammad Nahid Siddiqui Developing an effective adsorbent from asphaltene for the efficient removal of dyes in aqueous solution, Desalination and Water Treatment, Volume 67 (2017), p. 371 | DOI:10.5004/dwt.2017.20450
  • Pan Hu; Lujie Zhang; Jing Wang; Ruihua Huang Removal of methyl orange from aqueous solution with crosslinked quaternized chitosan/bentonite composite, Desalination and Water Treatment, Volume 80 (2017), p. 370 | DOI:10.5004/dwt.2017.20895
  • Tholiso Ngulube; Jabulani Ray Gumbo; Vhahangwele Masindi; Arjun Maity An update on synthetic dyes adsorption onto clay based minerals: A state-of-art review, Journal of Environmental Management, Volume 191 (2017), p. 35 | DOI:10.1016/j.jenvman.2016.12.031
  • Venkata Subbaiah Munagapati; Vijaya Yarramuthi; Dong-Su Kim Methyl orange removal from aqueous solution using goethite, chitosan beads and goethite impregnated with chitosan beads, Journal of Molecular Liquids, Volume 240 (2017), p. 329 | DOI:10.1016/j.molliq.2017.05.099
  • Rizwan Wahab; Farheen Khan; Nagendra Kumar Kaushik; Javed Musarrat; Abdulaziz A. Al-Khedhairy Photocatalytic TMO-NMs adsorbent: Temperature-Time dependent Safranine degradation, sorption study validated under optimized effective equilibrium models parameter with standardized statistical analysis, Scientific Reports, Volume 7 (2017) no. 1 | DOI:10.1038/srep42509
  • Jing Zhang; Mao Liu; Tao Yang; Kai Yang; Hongyu Wang Synthesis and characterization of a novel magnetic biochar from sewage sludge and its effectiveness in the removal of methyl orange from aqueous solution, Water Science and Technology, Volume 75 (2017) no. 7, p. 1539 | DOI:10.2166/wst.2017.014
  • Lele Gao; Qiurong Li; Xiaohui Hu; Xinpei Wang; Heru Song; Li Yan; Haiyan Xiao One-pot synthesis of biomorphic Mg-Al mixed metal oxides with enhanced methyl orange adsorption properties, Applied Clay Science, Volume 126 (2016), p. 299 | DOI:10.1016/j.clay.2016.03.034
  • Zaharaddeen N. Garba; Nkole I. Ugbaga; Amina K. Abdullahi Evaluation of optimum adsorption conditions for Ni (II) and Cd (II) removal from aqueous solution by modified plantain peels (MPP), Beni-Suef University Journal of Basic and Applied Sciences, Volume 5 (2016) no. 2, p. 170 | DOI:10.1016/j.bjbas.2016.03.001
  • Jie Yan; Yao Zhu; Fengxian Qiu; Hao Zhao; Dongya Yang; Jie Wang; Wenya Wen Kinetic, isotherm and thermodynamic studies for removal of methyl orange using a novel β-cyclodextrin functionalized graphene oxide-isophorone diisocyanate composites, Chemical Engineering Research and Design, Volume 106 (2016), p. 168 | DOI:10.1016/j.cherd.2015.12.023
  • Bentao Wang; Jun Qu; Xuewei Li; Xiaoman He; Qiwu Zhang; R. Riman Precursor Preparation to Promote the Adsorption of Mg‐Al Layered Double Hydroxide, Journal of the American Ceramic Society, Volume 99 (2016) no. 9, p. 2882 | DOI:10.1111/jace.14404
  • Y. Belaissa; D. Nibou; A.A. Assadi; B. Bellal; M. Trari A new hetero-junction p -CuO/ n -ZnO for the removal of amoxicillin by photocatalysis under solar irradiation, Journal of the Taiwan Institute of Chemical Engineers, Volume 68 (2016), p. 254 | DOI:10.1016/j.jtice.2016.09.002
  • S.S. Batool; Z. Imran; Safia Hassan; Kamran Rasool; Mushtaq Ahmad; M.A. Rafiq Enhanced adsorptive removal of toxic dyes using SiO 2 nanofibers, Solid State Sciences, Volume 55 (2016), p. 13 | DOI:10.1016/j.solidstatesciences.2016.02.001
  • B. Boutra; M. Trari; N. Nassrallah; B. Bellal Adsorption and Photodegradation of Solophenyl Red 3BL on Nanosized ZnFe2O4 Under Solar Light, Theoretical and Experimental Chemistry, Volume 52 (2016) no. 5, p. 303 | DOI:10.1007/s11237-016-9482-6
  • Islem Chaari; Bechir Moussi; Fakher Jamoussi Interactions of the dye, C.I. direct orange 34 with natural clay, Journal of Alloys and Compounds, Volume 647 (2015), p. 720 | DOI:10.1016/j.jallcom.2015.06.142
  • Ting Jiang; Yao-dong Liang; Yong-jun He; Qing Wang Activated carbon/NiFe2O4 magnetic composite: A magnetic adsorbent for the adsorption of methyl orange, Journal of Environmental Chemical Engineering, Volume 3 (2015) no. 3, p. 1740 | DOI:10.1016/j.jece.2015.06.020

Cité par 83 documents. Sources : Crossref


Commentaires - Politique