Investigation of performance of bimodal/functionalized mesoprorous silica nanoparticles on the adsorption of methylene blue from aqueous solution
Amir Vahid
1
(
Downstream Devision, Research institute of petroleum industry, Tehran, Iran
)
Keywords: Adsorption, Isotherm, Methylene Blue, Mesoporous silica, Wastewater treatment,
Abstract :
In this study, bimodal mesoporous silica, i.e. UVM-7, was synthesized and functionalized with sulfonic acid and characterized using XRD, nitrogen physisorption, SEM, TEM and acid/base titration. Results displayed that bimodal mesopore structure was firmly formed and acidic functional groups were grafted on the surface of the UVM-7. The concentration of the acidic functional groups was determined via titration by standard NaOH solution. At the second step, the adsorption of methylene blue from aqueous solutions onto UVM-7 and UVM-7/SO3H was investigated. The effect of PH, temperature, dye concentration, salt concentration and contact time on the adsorption of methylene blue was studied. The adsorption equilibrium isotherms were well fitted to Langmuir rather than Freundlich model. Methylene blue adsorption on UVM-7 increases with increasing the temperature and PH, which indicates that the process is endothermic. Maximum adsorption capacity of methylene blue by UVM-7 and UVM-7/SO3H were 107.5 mg/g and 129.9 mg/g, respectively. The adsorption kinetics of methylene blue for both UVM-7 and UVM-SO3H were pseudo ـsecond order and well fitted to Langmuir model.
Abstract
In this study, bimodal mesoporous silica, i.e. UVM-7, was synthesized and functionalized with sulfonic acid and characterized using XRD, nitrogen physisorption, SEM, TEM and acid/base titration. Results displayed that bimodal mesopore structure was firmly formed and acidic functional groups were grafted on the surface of the UVM-7. The concentration of the acidic functional groups was determined via titration by standard NaOH solution. At the second step, the adsorption of methylene blue from aqueous solutions onto UVM-7 and UVM-7/SO3H was investigated. The effect of PH, temperature, dye concentration, salt concentration and contact time on the adsorption of methylene blue was studied. The adsorption equilibrium isotherms were well fitted to Langmuir rather than Freundlich model. Methylene blue adsorption on UVM-7 increases with increasing the temperature and PH, which indicates that the process is endothermic. Maximum adsorption capacity of methylene blue by UVM-7 and UVM-7/SO3H were 107.5 mg/g and 129.9 mg/g, respectively. The adsorption kinetics of methylene blue for both UVM-7 and UVM-SO3H were pseudo ـsecond order and well fitted to Langmuir model.
Keywords: Adsorption; Isotherm; Methylene blue; Mesoporous silica; Wastewater treatment
1. introduction
Color is the first contaminant to be recognized in wastewater streams. Increase in the production of paints and dyes and many uses in variety of industries leading to production of wastewater, which in turn will cause environmental pollution concerns [1,2]. Different industries such as textile, paper, pharmaceutical, food and cosmetic use dyes and paints [3]. The presence of trace amounts of dyes in water, even lower than 1 ppm for some dyes, is unpleasant [4]. Various techniques have been employed for the removal of dyes from wastewaters. The conventional methods for treating dyes containing wastewaters are coagulation and flocculation [5-7], oxidation [8,9], membrane separation [10] and adsorption [11,12]. Adsorption technology is inexpensive and high potential in removal of small molecules, dyes and organic matter, and so one of the most efficient methods for the removal of dyes from wastewater industries than the others [13,14]. Methylene blue (hereinafter MB) is one of the most important dyes which uses in many industries and causes unclearness of water at very low concentrations because of its high adsorption coefficient. Furthermore, MB is not strongly hazardous; it can cause some harmful effects if there is too much such as increased heart rate, vomiting, shock, cyanosis and tissue necrosis in human [5-7]. Various types of adsorbent such as zeolites, mesoporous silicas, activated carbon, clays and nanomaterials have been investigated for removing dyes from aqueous solution [15]. In recent years, nanosize bimodal mesoporous silica, i.e. UVM-7, was synthesized. This mesoporous material with high surface area and bimodal porosity can be combined with functional chemical groups for the removal of polluttants from the environment [16].
In this study UVM-7 synthesized and functionalized with SO3H and used for the absorption of cationic dye, i.e. MB. The effect of different parameters such as PH, temperature, contact time, salt concentration and initial dye concentration were studied. The equilibrium adsorption data were fitted to Langmuir and Freundlich equations to determine the correlation between the experimental data and models.
2. Experimental
2.1. Materials and methods
The reactants used in this study were cetyltrimethylammonium bromide (CTAB), tetraethyl orthosilicate (TEOS) as silica source, teriethanolamine (TEAH3), hydrochloric acid (HCl), Sodium hydroxide) NaOH) and MB as adsorbate. Methylene blue (C16H18N3SCL) is a cationic blue dyestuff with Cl classification Number of 52015 and its chemical structure is shown in Figure 1.
Fig.1. Chemical structure of methylene blue dye
2.2. Synthesis of UVM-7
The general procedure for the synthesis of UVM-7 is the atrane route, in which the presence of polyalcohol is the key to balancing the hydrolysis and condensation reaction rates [18]. In a typical synthesis, TEOS was added to determined amounts of TEAH3. The solution was heated up to 140 °C under vigorous stirring. After cooling down to 90 °C, CTAB was added to this solution. After that, water was added slowly to the solution under stirring until a white suspension resulted. This suspension was aged four hours at room temperature. The solid was filtered, washed with sufficient amounts of water and acetone and dried in oven at 80 °C overnight. The final molar composition of the reactants was 1.0 TEOS: 3.5 TEAH3: 0.25 CTAB: 90 H2O. Thermocalcination of the as synthesized UVM-7 was carried out under a flow of air up to 550 °C for 6 hours with a heating rate of 1 °C/min to remove both the surfactant and TEAH3 from the as-synthesized UVM-7.
2.3. Synthesis of UVM-7/SO3H
For the functionalization of the synthesized UVM-7 with sulfonic acid group, predetermined amount of C9H22SO3Si and 2 g of calcined sample were added to 100 mL of toluene and stirred for 24 hours at 80 °C, followed by filtering and washing with proper amounts of ethanol. Then, SH group was oxidized to SO3H via oxidation using H2O2 (30 %) followed by proton exchange using HNO3 (1 molar). 1 grams of the obtained solid was added to 100 mL water and was titrated by 0.02 molar solution of NaOH and the obtained acid concentration was 1.5 mmol/g.
Fig.2. Mesoporous silica functionalized with sulfonic acid.
2.4. Adsorption experiments
The solution of MB at a concentration of 200 mg/L of distilled water was prepared then diluted to the required solution) 50 ،100،150 mg/L) were converted. The concentration of MB in the supernatant solution before and after the adsorption was determined by Uv ـVis spectrometer. The absorption of the colored solution measured at a wavelength 664 nm to a calibration curve between dye concentration and absorption is drawn. Using calibration curve amount of dye adsorption by UVM-7 after each test according to the amount of absorption in the wavelength 664 nm was calculated. 10 mg of silica UVM-7 was mixed with 10 ml of the aqueous solutions of various initial concentrations (50, 100, 150, 200 mg/g) of MB. The initial PH (4, 6, 8, 10 and 12) of the solutions was adjusted with 0.5 mol/l HCl or 0.5 mol/l NaOH solutions. The flasks with their contents were shaken for the different adsorption times (20, 40, 60, 80, 100 and 120 min) at temperatures 25, 30, 35 and 40◦c. The adsorbing capacity of methyl blue was calculated from the formula:
Where C0 and Ce (mg/g) are respectively the initial and equilibrium concentrations of dye, V (L) is the volume of the solution and M (g) is the mass of adsorbent used.
3. Results and discussion
3.1. Characterization of UVM-7 and UVM-7/SO3H
XRD patterns of UVM-7 and UVM-7/SO3H are shown in Figure 2a–b, respectively. A strong diffraction peak can be seen in all XRD patterns which is characteristic of this type of nanoparticulated meso/macroporous material. However, this strong peak can be attributed to diffraction from the d100 plane and is accompanied with a broad diffraction peak at higher angles in both samples. These broad peaks might be assigned to d110 and the overlap of d200 and d210 diffraction peaks on the basis of hexagonal symmetry [19,20].
Fig.3. XRD pattern of a) UVM-7 and b) UVM-7/SO3H
Figure 4a–b illustrates the nitrogen isotherms of UVM-7 and UVM-7/SO3H, respectively Textural properties of both samples are given in Table 1. Isotherms of both samples display two distinct regions at medium and high relative pressures, which can be attributed to the presence of a bimodal pore system. The inflection at medium relative pressure corresponds to a type IV isotherm which is typical of mesoporous materials and suggests the presence of a well-ordered array of small mesopores in all samples. However, after the functionalization of UVM-7, the sharpness of this region decreases which means a reduction of structural order [20].
Table 1. Textural properties of UVM-7 and UVM-7/SO3H.
Sample name | BET surface area (m2/g) | Total pore volume, (m3/g) | Average pore volume, (nm) |
UVM-7 | 810 | 0.65 | 33 |
UVM-7/SO3H | 416 | 0.33 | 21 |
Figure 4. Adsorption isotherms of nitrogen at 77 K on a) UVM-7 and b) UVM-7/SO3H
Electron microscopy is a useful technique for the direct elucidation of the morphology, as well as the particle size of the nano materials. SEM image UVM-7 is illustrated in Figure 5b. It can be clearly seen, UVM-7 is formed from very small nanoparticles which are also very homogeneous in size.
TEM image of UVM-7 in Figure 5a display small intraparticle mesopores related to the porogenic effect of the surfactant are obvious. The continuous nanometric structures constructed from these nanoparticles generate a hierarchic non-ordered system of large (interparticle) mesopores.
Fig.5. a) TEM image UVM-7 b) SEM imageUVM-7
3.2. Effect of PH on MB adsorption
MB is a cationic dy, and therefore, surface charge on the adsorbent in the absorption of MB is very important. The adsorptive removal of solution during the adsorption process mainly depends on solution pH, since it affects both the ionization degree and surface property of the adsorbents.
Figure 6 depicts the effect of PH on the MB adsorption. It was found that the adsorption capacity increased with increasing PH values. This can be found by considering the electrostatic attraction between the negative charges of the adsorbent surface that leads to the absorption of cationic dye MB. In other words, by increasing the PH, OH ions increase and thereby increases absorption of positive ions on the adsorbent surface [21]. In UVM-7/SO3H Due to the presence of SO3-, the negative charges adsorbent surface enhances that result increased absorption.
Fig.6. Effect of pH on removal of MB.
3.3. Effect of temperature on MB adsorption
The effect of temperature on the adsorption of MB is shown in Figure 7. The results revealed that the adsorption capacity increase with increasing temperature, showing that this process is endothermic. The increased adsorption capacity with temperature may be attributed to increase the rate of diffusion of the adsorbent across the external boundary layer and in the internal pores of the adsorbent particle, owing to the decrease in the viscosity of solution [22].
Fig.7. effect of temperature on removal of MB
In order to gain an insight into the mechanism involved in the adsorption process, thermodynamic parameters for the present system were calculated. The adsorption free energy (ΔG), adsorption enthalpy (ΔH) and adsorption entropy (ΔS) from the Langmuir isotherms at different temperatures were calculated using the following thermodynamic functions:
The slope and intercept of the van't Hoff plot is equal to -ΔH/R and ΔS/R, respectively where R is the universal gas constant (8.314 J (molK)); T is the absolute temperature (K) [23,24]. The change in standard free energy (ΔG) of adsorption was calculated from the following equation:
where R is gas constant, K the equilibrium constant obtained from Langmuir equations and T is temperature in Kelvin. Thermodynamic parameters obtained are summarized in Table 2. It is noted that all ΔG values listed in Table 2 are negative. This suggests that the adsorption process is spontaneous. As seen from Table 2, the positive value of adsorption enthalpy shows that the adsorption process is endothermic.
Table 2
Thermodynamic parameters for the adsorption of MB on UVM-7 and UVM-7/SO3H as a function of temperature.
| UVM-7 | UVM-7/ SO3H | ||||
T(K) | ∆H(kJ/mol) | ∆G(kJ/mol) | ∆S(kJ/mol K) | ∆H(kJ/mol) | ∆G(kJ/mol) | ∆S(kJ/mol K) |
298 | 12.6 | -3.91 | 0.053 | 17.26 | -7.14 | 0.0742 |
303 | 12.6 | -4.56 | 0.053 | 17.26 | -9.6 | 0.0742 |
308 | 12.6 | -7.23 | 0.053 | 17.26 | -11.37 | 0.0742 |
313 | 12.6 | -8.26 | 0.053 | 17.26 | -12.5 | 0.0742 |
3.4. The effect of salt concentration
The effect of various concentration of NaCl and CaCl2 solution on the amount of MB adsorbed onto per unit mass of UVM-7/ SO3H for an initial MB concentration of 200 mgL-1 and adsorbents dose of 10 mg is shown in Figure 8. The wastewater containing dye has commonly higher salt concentration, and effect of ionic strength (or salt concentration) is of some importance in the study of dye adsorption onto adsorbents. From Figure 8, NaCl and CaCl2 existed in solution affected the MB adsorption. It was seen that the increase in the salt concentration resulted in a decrease of MB adsorption. This trend indicated that the adsorbing efficiency decreased when NaCl and CaCl2 concentration increased in the MB solution, which could be attributed to the competitive effect between MB ions and cations from the salt for the sites available for the adsorption process. As Ca+2 has more ionic strength and more positive charge than Na+ so the effect of Ca+2 on adsorption MB is more serious than Na+.
Fig.8.effect of salt concentration on removal of MB
3.5. Effect of contact time
The effect of contact time on the adsorption of MB is shown in Figure 9. The rapid adsorption rate at the beginning of adsorption process may be explained by the increase number of active site on the sorbent surface, which would result in an increased concentration gradient between sorbent in the solution and on the sorbent surface. It can be seen that the adsorption after 80 min, the amount will not increase significantly; the absorption rate is controlled by the transfer of dye adsorbed on the surface of the adsorbent into the adsorbent particles. Therefore, to study the kinetics and adsorption isotherms, duration 80 min as the time required to reach equilibrium is considered.
Fig.9. Effect of contact time on removal of MB
3.6. Effect of initial dye concentration
The experiments conducted with 0.01g of adsorbent, 10 ml of dye solution. Figure 10 shows the effects of initial concentration on the adsorption MB that shows the adsorption of MB increases with an increase in the initial concentration (50, 100, 150, 200 mg/g). This phenomenon was due to the fact that when the initial concentration increases; the mass transfer driving force became larger, hence resulting in higher MB adsorption.
Fig.10. Effect of initial concentration on removal MB.
3.7. Adsorption isotherms
In general, an adsorption isotherm is an invaluable curve describing the phenomenon governing the retention or mobility of a substance from the aqueous media or aquatic environment to a solidـphase at a constant temperature and PH [25, 26]. Study of equilibrium of adsorption isotherms provide information on the capacity of the adsorbent and play an important role in understanding the mechanism of adsorption. Several isotherm models are presented. Langmuir and Freundlich models are the most widely used to describe the adsorption isotherm.
3.7.1. Langmuir adsorption isotherm model to MB adsorption
Langmuir isotherm describes quantitatively the formation of a monolayer adsorbent on the outer surface of the adsorbent, and after that no further adsorption takes place. The model assumes uniform energies of adsorption onto the surface and no transmigration of adsorbent in the plane of the surface and the maximum adsorption capacities for each dye were calculated using the Langmuir adsorption model that can be summarized by the following equation [27, 28]:
Where Ce (mg/L) is the equilibrium concentration, qe (mg/g) the amount of adsorbent adsorbed per unit mass of adsorbent, and qm is a constant that reflects the maximum adsorption capacity and b is a direct measure of the intensity of the adsorption process that is related to the heat of adsorption (L/mg). The essential features of the Langmuir isotherm can be expressed in terms of a dimensionless constant separation factor (RL), which is defined by the following relationship:
According to the value of RL, the isotherm shape may be interpreted as follows [29]:
RL >1.0 Unfavorable
RL = 1.0 Linear
1 >RL >0 Favorable
RL = 0 Irreversible
3.7.2. Freundlich adsorption isotherm model to MB adsorption
The empirical Freundlich model gives an expression encompassing the surface heterogeneity and exponential distribution of active sites and their energies, which is commonly presented as follows [30-32]:
log qe=logKF+1/n log Ce
Where KF is the Freundlich constant and 1/n is the heterogeneity factor. The slope 1/n ranging between 0 and 1 is a measure of adsorption intensity or surface heterogeneity, becoming more heterogeneous as its value gets closer to zero.
The Langmuir and Freundlich parameters for adsorption of MB are listed in Table 3, indicating that the Langmuir isotherm model yielded the best fit with the highest R2 value.
Table 3. Isotherm parameters for adsorption of MB
Langmuir | Freundlich | ||||||||
adsorbent | qm (mg/g) | b (L/mg) | R2
| KL
| RL
| KF (mg/g(L/mg)1/n) | N (L/mg) | R2 | |
UVM-7 | 107.5 | 0.6 | 0.99 | 6.54 | 0˂RL˂1 | 57.3 | 6.8 | 0.98 | |
UVM-7/SO3H | 129.9 | 0.0611 | 0.99 | 79.63 | 0˂RL˂1 | 59.1 | 5 | 0.91 | |
3.8. Adsorption kinetic-study
The kinetic behavior of the adsorption process was studied under the temperature of 24.5±0.5 ◦C and pH 6.3 using different initial dye concentrations (50, 100, 150, 200 mg/L).The controlling mechanisms of adsorption process such as chemical reaction, diffusion control or mass transfer coefficient are used to determine kinetic models. In this respect, the pseudo-first-order model and pseudo-second-order model were used to test the experimental data of different initial concentration [33, 34].
3.8.1 Application of pseudo-first-order model on MB adsorption
The pseudo-first-order kinetic model has been widely used to predict dye adsorption kinetics. The pseudo-first-order model was described by the following equation [35]:
Where qe and qt are the adsorption capacities (mg/g) at equilibrium and at time t, respectively, K1 is the rate constant of pseudo-first order adsorption (L/min).
3.8.2 Application of pseudo-second-order model on MB adsorption
The pseudo-second-order model was applied to predict the adsorption behavior during the entire adsorption period and is in accordance with the adsorption mechanism of rate controlling steps. The pseudo-second-order model was described by the following equation [36]:
Where qe is the equilibrium adsorption capacity, and K2 is the pseudo- second-order constants (g/mg min) can be determined experimentally from the slope and intercept of plot t/qt versus t, is a straight line as shown in Figure 11.
Fig.11.pseudo-second-order kinetic on removal MB
The experimental and calculated parameters of the kinetic equations above are summarized in Table 4, These results suggest that the adsorption of MB dyes be best described by the pseudo-second-order kinetic model at all temperatures with high correlation coefficients.
Table 4. kinetic parameters of adsorption of MB on UVM-7 and UVM-7/SO3H.
pseudo-first-order kinetic | pseudo-second-order kinetic | |||||
adsorbent | qe (mg/g) | K1 (L/min) | R2 | qe (mg/g) | K2 (g/(mg.min)) | R2 |
UVM-7 | 42.2 | 0.03 | 0.912 | 101 | 0.0007 | 0.99 |
UVM-7/SO3H | 15.6 | 0.03 | 0.917 | 99 | 0.003 | 0.99 |
4. conclusion
The present study shows that UVM-7 and UVM-7/HO3 is an effective adsorbent for the removal of methyl blue from aqueous solution. Several adsorption conditions such as PH, initial dye concentration, salt concentration, contact time and the temperature will influence its adsorption capacity for MB. It was found that the adsorption isotherm data fitted well with the Langmuir models, suggesting the adsorption to be monolayer and physical in nature. The kinetic data indicates that the pseudoـsecond order kinetic model was found to be well suited and highly correlated with the experimental data for the adsorption process.
References
[1] Kaur, S., and Singh, V. "TiO 2 mediated photocatalytic degradation studies of Reactive Red 198 by UV irradiation." Journal of hazardous materials 141, no. 1pp. 230-236, 2007.
[2] Nadi, H., Alizadeh, M., Ahmadabadi, M., Yari, A. R., Hashemi, S. "Removal of Reactive Dyes (Green, Orange, and Yellow) from Aqueous Solutions by Peanut Shell Powder as a Natural Adsorbent." Archives of Hygiene Sciences 1, no.2, 2012.
[3] Entezari, M. H., Z. Sharif Al-Hoseini, N. Ashraf. "Fast and efficient removal of Reactive Black 5 from aqueous solution by a combined method of ultrasound and sorption process." Ultrasonics sonochemistry 15.4, no. 4 pp. 433-437,2008.
[4] Crini, Gregorio. "Non-conventional low-cost adsorbents for dye removal: a review." Bioresource technology 97.pp. 1061-1085, no.9, 2006.
[5] Vadivelan, V., K. V. Kumar. "Equilibrium, kinetics, mechanism, and process design for the sorption of methylene blue onto rice husk." Journal of Colloid and Interface Science 286.pp.90-100,no.1,2005
[6] Kumar, K. Vasanth, V. Ramamurthi, S. Sivanesan. "Modeling the mechanism involved during the sorption of methylene blue onto fly ash." Journal of Colloid and Interface Science 284.pp. 14-21,no.1,2005.
[7] Thongchai P., Wongchaisuwan S. "Mechanisms of dye wastewater colour removal by magnesium carbonate-hydrated basic." Water Science & Technology 18.3.pp. 139-144, no.3,1986.
[8] Malik, P. K., Saha. S. K. "Oxidation of direct dyes with hydrogen peroxide using ferrous ion as catalyst." Separation and purification technology 31, 3, pp. 241-250, no.3, 2003.
[9] Koch, M., "Ozonation of hydrolyzed azo dye reactive yellow 84 (CI)." Chemosphere 46.1, pp.109-113, no.1, 2002
[10] Ciardelli, Gianluca, L. Corsi, and M. Marcucci. "Membrane separation for wastewater reuse in the textile industry." Resources, conservation and recycling 31.2, pp. 189-197 ,no.2 ,2001.
[11] Feng-Chin, W. Tseng R. "High adsorption capacity NaOH-activated carbon for dye removal from aqueous solution." Journal of hazardous materials 152.3, pp. 1256-1267, no. 3, 2008.
[12] Thinakaran, N., et al. "Removal of Acid Violet 17 from aqueous solutions by adsorption onto activated carbon prepared from sunflower seed hull." Journal of hazardous materials 151.2, pp. 316-322 no .2 ,2008.
[13] Gómez, V., Larrechi M. S., Callao. M. P. "Kinetic and adsorption study of acid dye removal using activated carbon." Chemosphere 69.7, no. 7, pp. 1151-1158, 2007. [14] Mao-Xu Z., et al. "Removal of an anionic dye by adsorption/precipitation processes using alkaline white mud." Journal of Hazardous Materials 149.3, no. 3, pp. 735-741, 2007. [15] Khan N. A., Hasan, Z., Jhung, S. H, "Adsorptive removal of hazardous materials using metal-organic frameworks (MOFs): A review." Journal of hazardous materials 244, pp. 444-456, 2013. [16] Shao, Y., Wang, X., Kang, Y., Shu, Y., Sun, Q. Li, L. "Application of Mn/MCM-41 as an adsorbent to remove methyl blue from aqueous solution." Journal of colloid and interface science 429, pp. 25-33, 2014. [16] Gil, A., Assis F.C.C., Albeniz S., Korili S. A. "Removal of dyes from wastewaters by adsorption on pillared clays." Chemical Engineering Journal 168, no. 3, pp. 1032-1040, 2011. [17] Pavan, F. A., Mazzocato, A. C., Gushikem, Y. "Removal of methylene blue dye from aqueous solutions by adsorption using yellow passion fruit peel as adsorbent." Bioresource Technology 99, no. 8, pp. 3162-3165, 2008. [18] Gao, C., Sakamoto Y., Sakamoto K., Terasaki O., Che S. "Synthesis and Characterization of Mesoporous Silica AMS-10 with Bicontinuous Cubic Pn [19] Li, W., Yue, Q., Deng, Y., Zhao, D. "Ordered Mesoporous Materials Based on Interfacial Assembly and Engineering." Advanced Materials 25, no. 37, pp. 5129-5152, 2013. [20] Barma, S., Mandal, B." Synthesis and characterization of ordered mesoporous silica membrane: Role of porous support and gas permeation study." Microporous and Mesoporous Materials 210, 10-19, 2015. [21] Gulnaz, O., Sahmurova, A., and Kama, S, "Removal of Reactive Red 198 from aqueous solution by Potamogeton crispus." Chemical Engineering Journal 174, no. 2, pp. 579-585, 2011. [22] Anbia, M., & Hariri, S. A. "Removal of methylene blue from aqueous solution using nanoporous SBA-3." Desalination 261.1, no.1, pp.61-66.2010. [23] Yunus O. "Kinetics of adsorption of dyes from aqueous solution using activated carbon prepared from waste apricot." Journal of hazardous materials 137, no. 3, pp.1719-1728, 2006. [24] Karaca, S., A. Gürses M., Acıkyıldız, Ejder M. "Adsorption of cationic dye from aqueous solutions by activated carbon." Microporous and Mesoporous Materials 115, no. 3 ,pp.376-382.2008. [25] Limousin, G., "Sorption isotherms: a review on physical bases, modeling and measurement." Applied Geochemistry 22.2, no.2, pp. 249-275,2007. [26] Allen, S. J., Mckay G., Porter J. F. "Adsorption isotherm models for basic dye adsorption by peat in single and binary component systems." Journal of Colloid and Interface Science 280.2,no.2, pp. 322-333,2004. [27] Ghanizadeh, G. H., Asgari G. H., "Removal of methylene blue dye from synthetic wastewater with bone char." Iranian Journal of Health and Environment 2.2, no. 2, pp. 104-113, 2009. [28] Cibi, M. C., Mahjoub B., Seffen M.. "Adsorptive removal of textile reactive dye using Posidonia oceanica fibrous biomass." International Journal of Environmental Science & Technology 4.4, no. 4, pp. 433-44, 2007. [29] Amin, N. K. "Removal of reactive dye from aqueous solutions by adsorption onto activated carbons prepared from sugarcane bagasse pith." Desalination 223, no. pp. 152-161, 2008. [30] Oladoja, N. A., Aboluwoye C. O., Akinkugbe A. O. "Evaluation of loofah as a sorbent in the decolorization of basic dye contaminated aqueous system." Industrial & Engineering Chemistry Research 48, no. 6, pp. 2786-2794, 2009. [31] Mehrasbi M. R., "Heavy metal removal from aqueous solution by adsorption on modified banana shell." Iranian Journal of Health and Environment 1, no. 1, pp. 57-66, 2008. [32] Silva J. P., Sousa S., Rodrigues, J., Antunes H., Porter, J. J., Gonçalves, I., Ferreira-Dias, S., "Adsorption of acid orange 7 dye in aqueous solutions by spent brewery grains." Separation and Purification Technology 40, no. 3, pp. 309-315, 2009. [33] Yuh-Shan H. "Review of second-order models for adsorption systems." Journal of hazardous materials 136.3, no 3, pp.681-689, 2006. [34] Repo E., Warchoł J. K., Bhatnagar A., Sillanpää M. "Heavy metals adsorption by novel EDTA-modified chitosan–silica hybrid materials." Journal of colloid and interface science 358.1, no. 1, pp. 261-267, 2011. [35] Shao, Y., Wang, X., Kang, Y., Shu, Y., Sun, Q., Li, L. "Application of Mn/MCM-41 as an adsorbent to remove methyl blue from aqueous solution." Journal of colloid and interface science 429, pp. 25-33, 2014. [36] Ho Y. S., McKay, G. "Pseudo-second order model for sorption processes." Process biochemistry 34.5, no.5, pp. 451-465, 1999.
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