Journal of the Chilean Chemical Society
versión On-line ISSN 0717-9707
J. Chil. Chem. Soc. v.54 n.1 Concepción 2009
J. Chil. Chem. Soc, 54, N° 1 (2009); págs: 73-76
EQUILIBRIUM AND KINETIC STUDIES OF PHENOL SORPTION BY CHITOSAN COATED MONTMORILLONITE
JINLONG YAN* AND GUIXIANG QUAN
School of Chemical and Biological Engineering, Yancheng Institute of Technology, Yancheng 224003, China *e-mail address: firstname.lastname@example.org
In order to provide physical support for chitosan and increase the accessibility of the binding sites for sorption process applications, chitosan was coated on the surface of montmorillonite. For the optimization of the sorption of phenol on chitosan coated montmorillonite (CCM), effects of pH, initial concentration and temperature on the sorption of phenol by CCM were investigated. In order to find the sorption characteristics, the isothermal data were applied to Langmuir and Freundlich linear isotherm equation, and the thermodynamic parameters (ΔH, ΔG and ΔS) were also calculated according to the values of binding Langmuir constant KL . The L type sorption isotherm between phenol and CCM suggests a relatively high affinity between the adsórbate and adsorbent, and the mechanism involved in the association of phenol with CCM were protón transfer, hydrogen bonding, London-Van der Waals forces because of lots of the OH and NH2 groups in the chitosan chain. The negative ΔH constant confirmed that the more phenol was adsorbed by CCM at lower temperature and the driving force for sorption process is an enthalpy effect. The kinetics of the sorption process of phenol on CCM were also investigated using the pseudo-first order and pseudo-second order kinetics, results showed that the second order equation model provided the best correlation with the experimental results. It was reached that modification of chitosan with montmorillonite increased the possibility of utilization of chitosan for phenol remo ve from aqueous solution.
Keywords: Sorption; Chitosan; Phenol; Kinetics; Equilibrium
Phenols are common soil and groundwater pollutants. These chemicals are classified as priority pollutants due to their toxic health effects at very low concentrations. Phenols in soil and groundwater are derivatives of natural bio-geochemical processes or have their origins in anthropogenic materials such as pesticide mixtures. Soils contaminated with anthropogenic phenols are of specific environmental concern because of the ecological risk associated with their high toxicity and relatively high mobility in the soil and groundwater environment. The ingestion of such contaminated water in the human body causes protein degeneration, tissue erosion, and paralysis of the central nervous system and also damages of the kidney, liver and pancreas. The threshold value of phenol in water is 4000 µg/L1. Therefore, it is considered necessary to remove the phenol form industrial effluents before discharging into the water stream. Sorption is superior in simplicity of design, initial cost, ease of operation and insensitivity to toxic substances in comparation with other physicochemical and biological techniques, such as the membrane filtrations coagulation/flocculation, ion exchange, advanced oxidation (chlorination, ozonation), flotation, chemical reduction and biological treatment (bacterial and fungal biosorption, biodegradation in aerobic or anaerobic conditions)2. Several investigations have studied the sorption of phenol on active carbón because of its large surface area, micro-porous nature, high adsorption capacity, high purity and easy availability3-7.
Natural materials that are available in large quantities or certain waste form agricultural operations may has potential to be used as low cost adsorbents, as they represent unused resources, widely available and are environmentally friendly. Chitosan (2-amino-2-deoxy-ß-D-glucan) is a partially deacetylated polymer of chitin by deacetylation with a strong alkaline solution. Many attention have been focused on the remove of trace metals from water by chitosan because of the coordination betweens the metal and the NH2 groups in the chitosan chain8, and the sorption of phenol from aqueous solution and its affecting parameters were also reported in our previous study9, but it is slightly soluble at low pHs and poses problems for developing commercial applications. It is also soft and has a tendency to agglomerate or form a gel in aqueous solutions. In addition, the active binding sites of chitosan are not readily available for sorption. Transport of the contaminants to the binding sites plays a very important role in process design. Therefore, it is necessary to provide physical support and increase the accessibility of the binding sites for process applications10,11.
Clays are widely used as adsorbents due to their high specific surface area. On the other hand, their sorption capacity is very low for organic molecules that are highly water soluble, polar, or cationic. This is due to the hydrophilic nature of the mineral surfaces. Natural clay has a negative charge that is compensated by exchangeable cations, such as Na+ and Ca2+ on their surfaces. This study concerns the applicability of montmorillonite as a physical support for coating chitosan to remove phenol. Over the last 20 years, several studies have been carried out on the use of quaternary ammonium salt exchanged clays as adsorbents of many organic compounds from water12.
In the present investigation an attempt was made to overcome these mass transfer limitations by synthesizing a biosorbent by coating chitosan on the surface of montmorillonite and evaluating its equilibrium sorption properties. The combination ofthe useful properties of montmorillonite and that of natural chitosan, could introduce a composite matrix with many application and superior sorption capabilities. Batch studies are carried out involving process parameters such as the effects of pH, the initial phenol concentration, temperature and contact time. Equilibrium analysis was conducted to understanding sorption process.
METERIALS AND METHODS
Na-montmorillonite used was provided by 184 Bentonite Company ofthe 10th Agriculture Division of Xinjiang Construction Group in China, which is a fine powder with an average particle size of 75 um in the dry state, a purity of 90%, an interlayer spacing of 1.44 nm, and a cation exchange capacity (CEC) of 92 mmol/100g. Stock solution of 1000 mg/L phenol (AR) was prepared with distilled water and stored in a refrigerator. Working solutions were prepared by diluting the stocking solution with distilled water just prior to use. Chitosan with the deacetylation degree 88% was obtained from Kabo Co. (Shanghai, China), which was ground and sieved to 100-150 mesh. The viscosity [η] of chitosan in 0.1 mol/L CH3COONa+0.2 mol/L CH3COOH solution was determined by the NDT-1 type viscometer at 30±0.ID. The weight-average molecular weight was calculated by Mark-Houwink equation11: [η]=kMwα, where α= -1.02x10-2xDD+1.82, k = 1.64x10-30xDD, and DD is the degree of deacetylation of chitosan. The weight-average molecular mass (Mw) of sample used in this experiment is 280,000.
Preparation of chitosan coated montmorillonite (CCM)
One gram montmorillonite was ground into paste in 100 mL deionized water, and then added in 100 ml 2 g/L chitosan solution with constant stirring for 1 h at 25□. The pH ofthe solution was adjusted to 7.0-7.5 with 20 g/L sodium hydroxide solution and then was precipitated for 0.5 h at 25□. The resulting CCM was filtered and washed with deionized water, and then dried at 40 □. XRD data was obtained using a DX-2000/DX-2500 X-ray diffractometers (Dandong, China) at room temperature without any further heat treatment. %OC (organic carbon)value of CCM was measured with HC1 (10%, V/V) using a CNS Macro Elemental Analyzer (Elementar Analysen Systeme GmbH, Germany). The specific surface areas of montmorillonite and CCM were determined by using BET method after N2 adsorption-desorption at 77 K with Sorptomatic 1990, Germany.
The sorption experiments were performed by batch method where samples of 0.1 g of CCM were equilibrated with 50 mL of solution containing various amount of phenol, under an intermittent stirring. Solutions pH was adjusted by using diluted solution of NaOH or HC1. The temperature (25D, 35 □ and 45 □ ) of the thermostatic bath was controlled within ±0.5 □. In pH dependent experiments, the phenol concentration was constant at 40 mg/L for each sample. After a determined time (usually 24h), the suspensions were centrifuged at 5000 rpm for 20 min, the concentration of phenol in the clear supernatant was determined using spectrophotometricallymeasurements. ASP-1105E 721-model spectrophotometer (Shanghai, China) was used throughout for the concentration determination of phenol at wavelength 510 nm using 4-aminoantipyrine as the chromogenic reagent. The pH measurements were carried out with a 25 pHS-2C model acidity meter (Leici Instrumental Factory, Shanghai, China), using a combination electrode.
The sorption capacity of CCM (qe ) was evaluated by amount of phenol sorbed: qe=(C0-Ce) x Vx10-3/G, (mg of phenol /g of sorbent) and by percent of phenol removal: R%=(C0 -Ce) x100/C0, where: C0 and Ce are initial and the equilibrium concentration of phenol in solution (mg/L), G is amount of sorbent (g) and V is volume of solution (mL).
Effect of contact time was determined by the "limited bath" technique. A sample (1 g) of CCM was added to 500 mL volume of phenol solution, with initial phenol concentration 40 mg/L. Under stirring, the temperature of solution was held constant at 25 °C with a thermostatic bath and solutions pH was adjusted to 4.0 by using diluted solution of NaOH or HC1. After different time intervals (from 30 minutes to 24 hours), volumes of 1 mL supernatant were taken for spectrophotometrically measurements of phenol content.
RESULTS AND DISCUSSIONS
Characterization of CCM
XRD data was used to see the basal peak and investigated the d001 value, there was no difference with the d001 values of montmorillonite and CCM, which meant that chitosan could not enter the interior channels of montmorillonite. %OC value of CCM was found to be 5.22, the specific surface areas of montmorillonite and CCM were 256 m2/g and 187 m2/g, respectively. The amount of chitosan deposited on the surface of montmorillonite was calculated theoretically to be about 11.5% in CCM when chitosan was assumed to be with the formula (C8H13N05)n.
Optimization of the sorption of phenol on CCM
pH is an important parameter for adsorption of phenol from aqueous solution because it affects the solubility of phenol, concentration ofthe counter ions on the functional groups of the adsorbent and the degree of ionization of the adsórbate during reaction. To examine the effect of pH on the phenol removal efficiency, the pH was varied from 2.0 to 10.0. The amount of phenol adsorbed show a declining trend with higher as well as with lower pH, and the maximum removal of phenol (more than 88% by the adsorbents) was observed at pH 4.0 (Figure 1). Several researchers have studied the sorption-desorption of phenolic chemicals in soil-water and sediment-water systems13-15. Phenols have been found to possess relatively high mobility in the aquifer environment because their sorption to mineral surfaces were usually minimal16, soil organic matter (SOM) was found to be a dominant factor that influenced the fate of organic contaminants in soils and aquifer material17,18, so the sorption of phenol by CCM was mainly contributed to chitosan. At low pH (below 4.0), the amine group on chitosan is protonated to varying degree but phenol is not dissociated because phenol is a very weak acid and has resonance stability due to its anionic structure (the pKa value of phenol is 9.98). Simultaneously physical and chemical adsorption were known as sorption, so the results indicated at pH 4.0 the chemical affinity between the OH and NH2 groups in the structure of chitosan and the OH group in the structure of phenol reached the top. Non-polar portions play an important role in hydrophobic interactions, the mechanism involved in the association of phenol with CCM were protón transfer, hydrogen bonding, London-Van der Waals forces because of lots of the OH and NH2 groups in the chitosan chain.
The sorption capacity of the powdered adsorbent CCM for phenol was determined at different initial phenol concentrations. The results presented in Table 1 shown that the phenol amount adsorbed increased with increasing phenol concentration but the percent of phenol removal decreased. At low initial phenol concentration, the ratio of the number of phenol ions to the number of available adsorption sites was small and consequently the sorption was independent ofthe initial concentration, but as the concentration of phenol increased, the situation changes and the competition for adsorption sites became fierce. As a result, the extent of sorption carne down considerably, but the amount adsorbed per unit mass ofthe adsorbent rose.
The sorption capacity of the powdered adsorbent CCM for phenol was determined at different temperature (Table 1). It indicated that less phenol was adsorbed at high temperature. The effect of ionic strength to sorption of phenol was also examined, sorption capacities of CCM for phenol increased with the increased in ionic strength.
Isotherms were the equilibrium relation between the concentration of the adsórbate on the solid phase and in the liquid phase. Phenol adsorption isotherms for CCM were drawn as the amount of phenol adsorbed as a function of equilibrium phenol concentration and shown in Figure 2. In terms of the slope of the initial portion of the curves, the shapes of the isotherms corresponding to 25 □, 35 □ and 45 □ may be classified as L type isotherm of Giles classification19. All of these curve shown convex initial curvature reaching a saturation plateau at a definite value. The L type isotherm suggested a relatively high affinity between the adsórbate and adsorbent. A competition may be seen for the sorption sites between water and phenol. Generally, L type isotherm reflected the occurrence of chemisorption.
To optimize the design of an sorption system for the removal of adsorbates, it was important to establish the most appropriate correlation for the equilibrium curves. Experimental data related to the sorption of phenol by chitosan was applied to the Freundlich equation20,
where k parameter was relative to the sorption capacity and n was a measure of sorption intensity; a favorable sorption corresponded to a value of 1<n<10.
The linear form of Freundlich equation was used to interpret the results in the following form,
Binding parameters of phenol on CCM, which were calculated from intercepts and slopes of these plots, were presented in Table 2, together with the correlation coefficient (r2) as a goodness of fit criterion. As can be seen from the results of linear form of Freundlich equation, the n values of the phenol sorption isotherms on CCM confirmed L-shape. Based on the linear form of Freundlich equation, greater k value was used to like sorption at lower temperature.
Experimental data related to the adsorption of phenol by CCM was also applied to the Langmuir isotherm equation20,
where KL was related to energy of the sorption and q0 was the maximum value of sorption capacity (corresponding to complete monolayer coverage).
The values in Table 2 show that the experimental data were more suitable to the Langmuir model than the Freundlich model. This was in accordance with the shape of the sorption isotherms, which corresponded to type L2 (Langmuir type) in the Giles classification system for sorption of a solute from its solution19.
As seen from Table 2 the values q of maximum sorption capacity, corresponding to monolayer coverage of the binding sites available in the sorbent, was obtained at different temperature. In the range 25-45□ an decrease of q0 was found with the increasing temperature.
Using the values of binding Langmuir constant KL, and the following equations, one can calculate the thermodynamic parameters (ΔH, ΔG, ΔS) (Table 3) of phenol sorption on CCM,
The negative values of apparent free energy change (ΔG, kJ/mol) confirmed that the sorption process of phenol on CCM was a spontaneous process. The negative apparent enthalpy change (ΔH, kJ/mol) computed from the slope of linear dependence of logKL on 1/T confirmed that more phenol was adsorbed by CCM at lower temperature. The negative apparent entropy change (ΔS, J/mol K) characterized a decreased disorder of the system and the apparent entropy change values were almost. It can be suggested that the driving force for sorption process was an enthalpy effect.
Kinetic study of the adsorption
Effect of contact time on remo val of phenol on CCM was shown in Figure 3. Sorption results revealed fast uptake of adsórbate species at the initial stages of the contact period, a gradual slow down as it approached equilibrium, with more or less a constant rate of adsorption at the intermedíate stage. The values of the residual concentrations at 6 h contact time was found to be almost same than those obtained after 24 h contact time. As seen in Figure 3, the equilibrium period required for maximum removal was found to be 4-6 hours. However the sorption half-time (t½ ) were of 45-60 min. This effect may probably be because of more available surfaces in the initial stage for adsorption leading to faster rate, in contrast to final stage where available adsorption site might have reduced with increasing repulsive force by already adsorbed particles, thus resulting in slow rate of adsorption.
The numerical analysis of sorption kinetic models assuming external mass transfer and intra-particle diffusion (pore diffusion, surface diffusion) was frequently applied to describe the sorption kinetics in batch systems theoretically. However, the complicated mathematical computation limited their use from the viewpoint of engineering applications. Therefore, some lumped kinetic models such as the pseudo-first-order, pseudo-secondorder, and Elovich equations were adopted to simulate the kinetic data. The kinetics of the sorption process of phenol on CCM was investigated using two different models, the pseudo-first order and pseudo-second order kinetics1. The pseudo-first order lagergren model, traditionally used for describing sorption kinetics, is generally expressed by the equation,
Where k1 was the lagergren rate constant of the first order sorption, evaluated from the slope of the plot log (q0-qt) versus t, mg/(g·min).
According to the pseudo-second order model, the kinetics was described by the equation,
Where k2 was the rate constant of the second order sorption, g/(mg·min) and k2q02=h was the initial sorption rate, mg/(g·min). By plot t/qt versus t, a straight line could be obtained and q0 k2 and h can be calculated.
The experimental kinetic data were adjusted according to the indicated models and the coefficients of correlation as well as the kinetic parameters of phenol on CCM were given in Table 4. The results showed that the second order equation model provided the best correlation with experimental results. This finding was similar to other studies on the biosorption of several dyes. For instance, pseudo second-order kinetics was also observed in the biosorption of Remazol Black B on biomass20.
For the sorption of phenol by CCM on the basis of the experimental results obtained, the sorption with maximum sorption capacity must be conducted at high concentration, low temperature, and pH=4.0. The L type sorption isotherm between phenol and CCM suggested a relatively high affinity between the adsorbate and adsorbent, and the mechanism involved in the association of phenol with CCM were protón transfer, hydrogen bonding, London-Van der Waals forces because of lots of the OH and NH2 groups in the chitosan chain. The negative ΔH constant at lower temperature confirmed that more phenol is adsorbed by CCM at lower temperature, and the driving force for sorption process is an enthalpy effect. The kinetics of the sorption process of phenol on CCM was investigated using the pseudo-first order and pseudo-second order kinetics; results showed that the second order equation model provided the best correlation with the experimental results. From the standpoint of industrial applications, CCM was suitable and attractive adsorbent due to low price and high sorption capacity.
1. R. Qadeer, A.H. Rehan, Turk. J. Chem. 26, 357, (2002) [ Links ]
2. D. Suteu, D. Bilba, Acta Chim. Slov. 52, 73, (2005) [ Links ]
3. E. Costa, G. Calleja, L. Marjuan, Adsorp. Sci. Technol. 5, 213, (1988) [ Links ]
4. M. Kastelan-Malan, S. Cerjan-Stefanovic, M. Petrovic, Chromatographic. 27, 297, (1989) [ Links ]
5. S. Biniak, J. Kazmierczak, Adsorp. Sci. Technol. 6, 182, (1989) [ Links ]
6. N.S. Abuzeid, I.M. Harrozim, J. Envirn. Sci. Health A. 26, 257, (1991) [ Links ]
7. K. Radeke, H.D. Loseh, K. Struve, E. Weiss, Zeolites. 13, 69, (1993) [ Links ]
8. M. Y. Lee, K. J. Hong, Y. Shin-Ya, T. Kejiuchi, J. Appl. Polym. Sci. 96, 44, (2005) [ Links ]
9. J.L. Yan, Chin. J. Polymer Sci. 24, 497, (2006) [ Links ]
10. S. Babel, T. A. Kurniawan, Chemosphere. 54, 951, (2004) [ Links ]
11. W. Wang, S. Bo, S. Li, W. Qin, Int. J. Biol. Macromol. 13, 281, (1991) [ Links ]
12. M. Houari, B. Hamdi, J. Brendle, J. Hazard. Mater. 147, 738, (2007) [ Links ]
13. P. J. Isaacson, C. R. Frink, Environ. Sci. Technol. 18, 43, (1984) [ Links ]
14. K. G. Robinson, J. T. Novak, Water Res. 28, 445, (1994) [ Links ]
15. B. Xing, W. B. McGill, M. J. Dudas, L.G. Hepler, C. Dobrogowska, Chemosphere CMSHAF. 26, 1311, (1993) [ Links ]
16. I. Sabbah, M. Rebhun, Water Environ. Res. 69, 1032, (1997) [ Links ]
17. P. M. Gschwend, S.C. Wu, Environ. Sci. Technol. 19, 90, (1985) [ Links ]
18. L. S. Lee, P. S. C. Rao, P. Nkedi-Kkizza, Environ. Sci. Technol. 24, 654, (1990) [ Links ]
19. C.H. Giles, T.H. McEwan, S.N. Nakhwa, D. Smith, J. Chem. Soc. 4, 3973, (1960) [ Links ]
20. C. H. Ko, C.H Fan, P.N. Chiang, M.K. Wang, K.C. Lin, J. Hazard. Mater. 149, 275, (2007). [ Links ]
(Received 25 June 2008 - Accepted 11 August 2008)