Research Article  Open Access
Thermodynamics of Biosorption for Removal of Co(II) Ions by an Efficient and Ecofriendly Biosorbent (Saccharum bengalense): Kinetics and Isotherm Modeling
Abstract
In this research work, a lowcost biomass derived from the pulp of Saccharum bengalense (SB) was used as an adsorbent material/biosorbent for the removal of Co(II) ions from aqueous solution. Langmuir, Freundlich Timken, and DubininRadushkevich (DR) adsorption isotherms have been applied to further define the mechanism of sorption. From the comparison of different adsorption isotherm models, it was found that biosorption of Co(II) by SB followed Langmuir and Freundlich models. The sorption capacity for cobalt of Saccharum bengalense was ( mg/g) at 323K. A comparison of kinetic models applied to the adsorption of Co(II) onto Saccharum bengalense was evaluated for the pseudofirstorder, pseudosecondorder, Elovich, and intraparticle diffusion and Bangham's kinetics models. It was found that the pseudosecondorder mechanism is predominant. Activation parameters evaluated from thermodynamics and kinetic parameters such as free energy change , kJ/mol), enthalpy change , kJ/mol), and entropy change , kJ/mol) revealed the spontaneous, endothermic, and feasible nature of adsorption process. The results of the present investigation suggested that Saccharum bengalense (SB) can be used as an environmentally and economically feasible biosorbent for the removal of Co(II) from aqueous solutions.
1. Introduction
Cobalt is one of the various metals that is found naturally in the body, but as with all other metals, in excess amounts it becomes toxic and leads to many harmful and potentially permanent side effects. Cobalt present in industrial wastewaters can produce a variety of adverse effects on humans. It may cause interstitial pneumonitis, interstitial fibrosis, myocardial and thyroid disorders, and sensitization of the respiratory tract and skin [1, 2]. Chronic cobalt poisoning may also produce hyperplasia and polycythemia of the bone marrow [3]. Cobalt poisoning also caused cardiomyopathy, hypothyroidism, neuropathy, seizures, blindness, headaches, liver damage, and neurological damage as well as impairing the senses. Acute exposure to cobalt can induce neurotoxicological and genotoxicity disorders in human beings and in unrelenting cases may cause gastrointestinal troubles and even cancer [4, 5].
The most extensively used methods for removing Co(II) metal ions from wastewaters included adsorption, ion exchange, reverse osmosis, evaporation, membrane filtration and chemical precipitation [6, 7]. Most of these methods suffer from drawbacks such as the disposal of the residual metal sludge; high capital and operational cost; not suitable for smallscale industries [8]. Adsorption, by activated carbons, has the most extensive applications in this regard. It has high adsorption capacity, mesoporous nature, and highsurface area, but it has limited use due to nonregenerable features and high operational cost. For this reason, there is a need for developing ecofriendly and economic alternative methods and materials for waste treatment [9]. Agricultural waste and Natural materials that are accessible in huge quantities may have potential as alternate and cost effective sorbents. The profusion and accessibility of agricultural byproducts make them good sources of raw materials for natural biosorbents [10].
The common name of Saccharum bengalense (SB) is “Kana” or “Sarkanda” and is distributed from north and North West India to Pakistan and Afghanistan. A valuable fiber can be extracted from the upper leaf sheaths of the flowering Culm [11]. It can produce large quantities of biomass that may offer a good basis for the selection of SB economic and ecofriendly alternative biosorbent. To the best of our knowledge, no investigations have been reported to explore the biosorption characteristics of this plant for the removal of metal ions such as Co(II). The aim of the present research work is to investigate the biosorption capacity of Saccharum bengalense to remove Co(II) metal ions from aqueous solution in a batch procedure. Mechanism of adsorption was explained by using two parameters adsorption isotherms. Efficiency of adsorption has been studied in terms of kinetic models. Spontaneity and feasibility of the sorption process is confirmed by determining thermodynamically parameters such as , , and .
2. Methods
2.1. Collection of Biosorbent
Large pieces of Saccharum bengalense (SB) were collected from the bank of the river Satluj Bahawalpur, Pakistan. SB samples were washed with deionized water to remove any dust or other particles and dried under shade, then the samples were knifemilled. The 60–400 μm particles were collected and washed with deionized water. Finally, the samples were oven dried (at 333 K) to constant mass and stored in air tight plastic bottles and labeled as Saccharum bengalense (SB).
2.2. Characterization of SB
The biomass SB was characterized by FTIR, elemental analysis, and BET surface area. BET surface area and singlepoint surface area of SB were determined from the adsorption isotherm at 77 K in the range of relative pressure to 1.0 with a surface area and pore size analyzer (Autosorb 1, Quantachrome Instruments, USA). Before measurement, the sample was degassed at 300°C for 2 h. Elemental analyses were accomplished by (PerkinElmer 2400 Series II CHNS/O, USA) elemental analyzer using sulfanilamide as the standard. A potassium bromide (KBr) disc method was used to scan the FTIR spectra in 4000–600 cm^{−1} range by using FTIR spectrophotometer (Tensor 27, Bruker, Germany).
2.3. Adsorption Experiments
All analytical grade chemical reagents including atomic absorption spectrometric standards were purchased from Fluka Chemicals. Cobalt stock solution (1000 mg/L) was prepared from Co(NO_{3})_{2}6H_{2}O by dissolving the calculated amount in doubly distilled water. Further dilutions were prepared freshly as per requirement. A PekinElmer 2380 Atomic Absorptions Spectrophotometer with airacetylene flame was employed for the determination of cobalt concentration. The percentage removal efficiency of adsorbent (% A), the sorption capacity at time (mg/g) and the sorption capacity at equilibrium (mg/g) were calculated as follows: where (mg/L) and (mg/L) were the liquidphase concentrations of solutes at the initial and a given time , respectively. (mg/L) was the concentration of Co(II) at equilibrium, V is the volume of the solution in liter and m is the mass of the adsorbent in grams.
3. Results and Discussion
3.1. FTIR, Physicochemical Analysis of the Biosorbent
SB generally considered as structures built by cellulose molecules and surrounded by hemicellulosic materials (glucomannans, galactans, and arabogalactans), lignin, and pectin. The results of physical analysis, elemental analysis, and FTIR are shown in Table 1.

In the FTIR spectrum of SB, the intense peak at 1039.40 cm^{−1} along with the weak peak at 1240.00 cm^{−1} and the shoulder at 1159.41 cm^{−1} are C–O stretching vibration of ethers and alcohols. The band at 1601.3 cm^{−1} is due to carbonyl groups of aldehydes and ketones. The absorption band at 1730.90 cm^{−1} is attributed to the vibrations by carbonyl groups of ester and carboxylic acid groups. The single peak at 2913.29 cm^{−1} is due to C–H stretching vibration of CH, CH_{2}, and CH_{3} groups present in lignin. The broad band centered at 3356.93 cm^{−1} is a characteristic band of O–H stretching vibration. Thus, SB mainly consists of compounds having oxygencontaining functional groups.
Comparing and assignments of SB before and after Co(II) sorption are too important to indicate the functional groups responsible for Co(II) binding. Regarding FTIR for SB after Co(II) uptake, it was found that oxygen containing functional groups like phenolic –OH, carboxy –COOH, and methoxy –OCH_{3} groups are affected after uptake process (Figure not shown). This was confirmed by shifts in their position or band intensity from 3356.93 cm^{−1} to 3373.26, 1039.44 to 1037.39, and from 1730.99 to 1658.26 cm^{−1} [12] as indicated in Table 1.
3.2. Effect of the Adsorbent Dosage
Adsorbent quantity is very imperative feature as it determines the extent of removal of metal and may be used to determine the cost of adsorbent per unit volume of solution to be treated.
With increase in the adsorbent dosage, from 0.1 to 2.0 g/50 mL, the amount of adsorbed Co(II) ions increases from 72% to 89.2%. It was noticed that the extent of adsorption increased with the increase in adsorbent dosage (see Figure 1(a)). Adsorbent dosage has a direct effect on adsorbate removal of Co(II) because of the following reasons: (a) it may increase in SB surface, (b) availability of more adsorption sites on SB [13].
(a)
(b)
It is obvious that the optimum amount of SB for further adsorption experiments was selected as 0.5 g/50 mL. On the other hand, with further increase in adsorbent amount, the adsorption capacity decreases. This may be due to (i) the overlapping or aggregation of adsorption sites of SB resulting a decrease in total adsorbent surface area available to Co(II) ions, (ii) adsorption density increases with the decrease in adsorbent dosage due to higher amount of Co(II) per unit weight of adsorbent, (iii) the time required to reach the equilibrium decreased at higher doses of SB.
3.3. Effect of pH
In this present investigation, the biosorption of cobalt was studied at pH range of 2–10 with the adsorbent dose of 0.5 g/50 mL and adsorbate concentration of 50 mg/L. The maximum removal efficiency was 85.4% at pH 6. Acidic conditions are required for metal uptake as it increases the affinity of SB to Co(II) ions. It was observed that pH significantly affects the adsorption process. As the pH of the medium is increased, the competition between positively charged metal ions and H^{+} ions decreases, and metal ions become the dominant species to sorb on the biosorbent [14]. This is true as far as the metal ions are present as positively charged species in the solution. So an optimum pH is expected to lie in the acidic region [15]. At lower pH (2–6), H^{+} ions compete with Co(II) ions for the available adsorption site whereas at higher pH, adsorption sites are inactive. Above optimum pH, Co(II) ions react with hydroxide ions and precipitate as metal hydroxide (see Figure 1(b)).
3.4. Adsorption Kinetics
Adsorption kinetics describes the relationship of solute uptake rate of the adsorption and the adsorption time. In order to clarify the adsorption kinetics in different kinetic models, the pseudofirstorder, pseudosecondorder, Elovich, and intraparticle diffusion and Bangham's models were applied to the sorption data.
3.4.1. PseudoFirstOrder Model
The pseudofirstorder model is based on the assumption that the adsorption rate is proportional to the number of available sites [16].
The pseudofirstorder model is expressed by the following equation: where and (mg/g) are the amount of metal ions adsorbed on per unit weight of adsorbent at time t and equilibrium, respectively; (min^{−1}) is the pseudofirstorder rate constant of the sorption process.
By applying the boundary conditions to and to and integrating, the following equation is obtained: Linear plots of ln() versus t can be plotted to evaluate this kinetic model and to determine and rate constant from intercept and the slop, respectively.
3.4.2. PseudoSecondOrder Model
It is based on the assumption that adsorption rate is proportional to the square of the number of unoccupied sites where (gm g^{−1} min^{−1}) is the rate constant of the pseudosecondorder model. Integrating the above equation from to and to , the following equation is obtained: The most often used linearized form is given as [17] The parameters and can be calculated from the intercept and the slope of the plot versus t.
3.4.3. Elovich Model
Elovich equation is a rate equation based on the adsorption capacity (mg/g). The kinetic sorption data may also be analyzed using the Elovich equation. Rate equation can be expressed as This equation can be simplified by assuming and by applying the boundary conditions: at and at , the linear form obtained is [18] where β is related to the extent of surface coverage and activation energy for chemisorption (g/mg). α is the initial sorption rate constant (mg/g min). The constant can be obtained from the slope and intercept of the plot of versus ln t.
3.4.4. The Intraparticle Diffusion Equation
The intraparticle diffusion equation [19] can be written as follows: where is the intraparticle diffusion rate constant (mg g^{−1} min^{−1/2}), and C is the intercept.
By using this model, the plot of (mg g^{−1}) versus the square root of time (t^{1/2}) should be linear if the intraparticle diffusion is involved in the adsorption process, and if these lines pass through the origin, then the intraparticle diffusion is the ratecontrolling step [20].
3.4.5. Bangham's Equation
Kinetic data were further used to know about the controlling step occurring in the present adsorption system using Bangham's equation [21] where α(<1) and are constants, is the initial concentration of adsorbate in solution (mg/L), V is the volume of solution (L), m is the weight of adsorbent per liter of solution (g/L), (mg/g) is the amount of adsorbate retained at time t.
Here are two indicators for pseudofirstorder and pseudosecondorder kinetic models to decide whether the system follows them or not, that is, value and comparison of experimental and calculated values.
The kinetic parameters for the adsorption of Co(II) ions onto (S.B) are summarized in Table 2 and shown in Figures 2(a)–2(e).

(a)
(b)
(c)
(d)
(e)
These results show that the adsorption of Co(II) on SB followed the pseudosecondorder kinetic model at alltime intervals. The calculated values agree with experimental values, and the correlation coefficient values for the pseudosecondorder kinetic plots were high as shown in Figure 2(b). But in case of pseudofirstorder model, calculated values did not agree well with experimental values, and the value of correlation coefficients was low.
The correlation coefficient value obtained from Figure 2(d) was (0.855) indicating that the Elovich expression could not fit properly those experimental data.
The correlation coefficients for the intraparticle diffusion model are lower than that of the pseudosecondorder kinetic model, whereas this model indicates that the adsorption of Co(II) ions on SB also followed the intraparticle diffusion model as shown in Figure 2(c). As the plots of (mg g^{−1}) versus the square root of time () did not pass through the origin, this is indicative of some degree of boundary layer control, and this further shows that the intraparticle diffusion is not the only ratelimiting step, but also other kinetic models may direct the rate of adsorption [22].
Kinetic data can further be used to verify whether pore diffusion was the only ratecontrolling step or not in the adsorption system using Bangham's equation. The correlation coefficient, , value obtained was 0.906 indicating that that pore diffusion was not solely the rate limiting and the Bangham’s expression could not as well fit properly those experimental data.
3.5. Equilibrium Parameters of Biosorption
The equilibrium adsorption isotherms are considered one of the most important aspects in understanding the mechanism of the adsorption. The results obtained were analyzed using different isotherm equations (Langmuir, Freundlich, Temkin, and Dubinin–Radushkevich isotherm equations).
3.5.1. Langmuir Adsorption Isotherm
The Langmuir adsorption isotherm model assumes that adsorption takes place at specific homogeneous sites within the adsorbent [23] The different linear forms of the Langmuir isotherm model [24] are where (mg g^{−1}) is the adsorption capacity at equilibrium; (mg/L) is the concentration of Co(II) at equilibrium; is the monolayer adsorption capacity of the adsorbent (mg g^{−1}); is the Langmuir constant (L mg^{−1}) related to the free energy of adsorption. Equations (13) and (14) are commonly applied to biosorption process.
Klotz Equation. It is multiplied inverse of (13), a plot of versus for the Klotz method for Langmuir adsorption gives a straight line of slope 1/() and intercept . The values for these parameters are calculated from Figure 3(a) and are given in Table 3.

(a)
(b)
(c)
(d)
3.5.2. Freundlich Isotherm
The linear equation of the Freundlich adsorption model is [25] where (dm^{3} g^{−1}) and (dimensionless) are the Freundlich adsorption isotherm constants, being indicative of the extent of the adsorption and the degree of nonlinearity, respectively. The plot of ln versus ln for the adsorption was employed to generate the intercept value of and the slope value of n, respectively, as shown in Figure 3(b).
The “n” value provides information about the process to be favorable or unfavorable under studied conditions. The value of “n” was “1.33” for SB. This shows that the adsorption onto the heterogeneous systems is quite favorable. The value is 0.98; thus, the sorption of Co(II) by SB followed Freundlich model, and the sorption is favorable under the specific set of conditions.
3.5.3. DubininRadushkevich (DR) Isotherm
The linear form of (DR) isotherm model [26] is where β is a constant connected with the mean free energy of adsorption per mole of the adsorbate (mol^{2} kJ^{−2}), is the theoretical saturation capacity (mg g^{−1}), and is the Polanyi potential [27], which is equal to where R (J mol^{−1} K^{−1}) is the gas constant, and T (K) is the absolute temperature. Hence, by plotting ln versus , it is possible to generate the value of from the intercept and the value of from the slope. The description of the sorption of Co(II) on SB by the DubininRadushkevich (DR) equation is a pointer to the heterogeneity of the surface of the SB [28]. The biosorption mean free energy (kJ/mol) is as follows [29]: The (DR) constants for Co(II) were calculated from Figure 3(c), and results are given in Table 3.
Here are two indicators for DR model to decide whether the system follows it or not, that is, value and comparison of calculated and experimental values. The calculated value for SB is 3.01 mg/g which is not comparable with experimental value (2.5 mg/g). The values were less than 0.98; hence, it is indicated that the adsorption of cobalt onto SB did not follow the DubininRadushkevich isotherm.
The mean free energy of biosorption () was found to be 0.353 kJ/mol for SB. This value showed that the adsorption was physical in nature. Since DR model is not being followed by this system, this value provides only an estimation of the nature of the biosorption processes.
3.5.4. Temkin Isotherm
Temkin isotherm assumes that heat of adsorption decreases linearly with the adsorption onto the surface at a particular temperature, and the adsorption is characterized by a uniform distribution of binding energies. Temkin isotherm is expressed in linear form by the following equation [30, 31]: where is related to the heat of adsorption, T (K) is the absolute temperature, R is the universal gas constant (8.3143 J/mol), b indicates the adsorption potential of the adsorbent (J/mol), and is the equilibrium binding constant (L/mg). The parameters for the Temkin model are obtained from the plot of versus ln (Figure 3(d)). The values for these parameters are given in Table 3. The values indicated that the adsorption of Co(II) on SB did not follow Temkin model.
From the comparison of different adsorption isotherm models, it was found that biosorption of Co(II) by SB followed Langmuir and Freundlich models. The values were quite close for other adsorption models.
4. Thermodynamic Parameters of Adsorption
Thermodynamic parameters for adsorption of Co(II) onto SB were calculated using the following relations [27, 41, 42]: where R is the universal gas constant (8.314 J/mol K), T the temperature (K), and () is the distribution coefficient. is the adsorption capacity (mg g^{−1}), (mg/L) is the concentration of Co(II) at equilibrium (mgL^{−1}). The Gibbs free energy indicates the degree of spontaneity of the sorption process, and the higher negative value reflects a more energetically favorable sorption. The negative values of confirm the thermodynamic feasibility of the process and spontaneous nature of adsorption on SB [43]. The positive value of indicated the endothermic nature of the adsorption, while the positive values of reflected the increase in randomness for solidsolution interface and affinity of the adsorbent material [44]. The values of , and were calculated from Figure 4(a), and results were discussed in Table 4.

(a)
(b)
4.1. Activation Energy
The kinetic parameters at different temperatures were plotted in terms of the Arrhenius Equation [45] as where is the pseudosecondorder rate constant (g mg^{−1} min^{−1}), is the independent temperature factor (g mg^{−1} min^{−1}), R is the gas constant (J mol^{−1} K^{−1}), and T is the solution temperature (K). A plot of ln versus 1/T gives a straight line, and the corresponding activation energy was determined from the slope of linear plot shown in Figure 4(b). The activation energy for the biosorption of Co(II) on SB is given in Table 4. The magnitude of activation energy gives an idea about the type of adsorption, which is mainly physical or chemical. Low activation energies (5–50 kJ mol^{−1}) are characteristics for physical adsorption process, while higher activation energies (60–800 kJmol^{−1}) suggest chemical adsorption process [46].
4.2. Determination of Activation Parameters
Activation parameters such as enthalpy (), entropy (), and free energy () can be calculated from the Eyring equation [47]: where is the Boltzmann constant ( J K^{−1}), h is Planck’s constant ( J s), and is the pseudosecondorder rate constant. The plot of ln () against 1/T is shown in Figure 4(c).
Gibbs energy of activation can be calculated as The change of activation Gibbs energy (ΔG^{#}) for adsorption of Co(II) ions on SB was calculated as +84.61k J mol^{−1} at 323K. It indicates that adsorption reactions require energy to convert reactants into products. The value determines the rate of the reaction; rate increases as decreases, and as the energy requirement is fulfilled, the reaction proceeds [48]. The positive value of confirms the endothermic process, demonstrating that the reaction consumes energy [49]. The negative value of suggests that adsorption of Co(II) on SB surface is an associated mechanism [50, 51].
4.3. Comparison of Adsorption Capacity of SB with Different Adsorbents
SB has been compared with various adsorbents in terms of adsorption capacity (mg/g). Table 5 shows such a comparison. It can be easily observed that the adsorption capacity of SB is high as compared to a number of other materials.

5. Conclusion
It can be concluded that Saccharum bengalense is an effective biosorbent for the removal of Co(II) ions from aqueous water. The biosorption of Co(II) by SB followed Langmuir and Freundlich models. The rate constant increased with increase in temperature indicating endothermic nature of adsorption. The values of , and predicting the adsorption of Co(II) onto SB were diffusion controlled and an associative mechanism. The adsorption capacity increased with the rise in temperature was indicating that the adsorption was a spontaneous, feasible, and endothermic process.
References
 G. J. Hathaway, N. H. Proctor, and J. P. Hughes, Proctor and Hughes' Chemical Hazards of the Workplace, Van Nostrand Reinhold, New York, NY, USA, 3rd edition, 1991.
 L. Parmeggiani, 3rd Encyclopaedia of Occupational Health and Safety: Volume 1 A–K, International Labour Organisation, Geneva, Switzerland, 1983.
 N. J. D. H. Trenton, Department of Health, New Jersey, 1985.
 H. Benaïssa and M. A. Elouchdi, “Biosorption of copper (II) ions from synthetic aqueous solutions by drying bed activated sludge,” Journal of Hazardous Materials, vol. 194, pp. 69–78, 2011. View at: Publisher Site  Google Scholar
 N. Kuyucak and B. Volesky, “Accumulation of cobalt by marine alga,” Biotechnology and Bioengineering, vol. 33, pp. 809–814, 1989. View at: Publisher Site  Google Scholar
 J. W. Moore, Springer, New York, NY, USA, 1994.
 A. Sarı and M. Tuzen, “Biosorption of total chromium from aqueous solution by red algae (Ceramium virgatum): equilibrium, kinetic and thermodynamic studies,” Journal of Hazardous Materials, vol. 160, pp. 349–355, 2008. View at: Publisher Site  Google Scholar
 M. Kobya, E. Demirbas, E. Senturk, and M. Ince, “Adsorption of heavy metal ions from aqueous solutions by activated carbon prepared from apricot stone,” Bioresource Technology, vol. 96, no. 13, pp. 1518–1521, 2005. View at: Publisher Site  Google Scholar
 Ö. Gerçel and H. F. Gerçel, “Adsorption of lead(II) ions from aqueous solutions by activated carbon prepared from biomass plant material of Euphorbia rigida,” Chemical Engineering Journal, vol. 132, no. 13, pp. 289–297, 2007. View at: Publisher Site  Google Scholar
 D. Nayak and S. Lahiri, “Biosorption of toxic, heavy, nocarrieradded radionuclides by calcium alginate beads,” Journal of Radioanalytical and Nuclear Chemistry, vol. 267, pp. 59–65, 2005. View at: Publisher Site  Google Scholar
 S. A. Tirmzi et al., “Inorganic Nutrients of Saccharum bengalense,” Journal of the Chemical Society of Pakistan, vol. 27, pp. 186–189, 2005. View at: Google Scholar
 E. M. Soliman, S. A. Ahmed, and A. A. Fadl, “Reactivity of sugar cane bagasse as a natural solid phase extractor for selective removal of Fe(III) and heavymetal ions from natural water samples,” Arabian Journal of Chemistry, vol. 4, no. 1, pp. 63–70, 2011. View at: Publisher Site  Google Scholar
 O. D. Uluozlu, A. Sari, M. Tuzen, and M. Soylak, “Biosorption of Pb(II) and Cr(III) from aqueous solution by lichen (Parmelina tiliaceae) biomass,” Bioresource Technology, vol. 99, no. 8, pp. 2972–2980, 2008. View at: Publisher Site  Google Scholar
 A. Sarı and M. Tuzen, “Kinetic and equilibrium studies of biosorption of Pb(II) and Cd(II) from aqueous solution by macrofungus (Amanita rubescens) biomass,” Journal of Hazardous Materials, vol. 164, pp. 1004–1011, 2009. View at: Publisher Site  Google Scholar
 U. Farooq, J. A. Kozinski, M. A. Khan, and M. Athar, “Biosorption of heavy metal ions using wheat based biosorbents  A review of the recent literature,” Bioresource Technology, vol. 101, no. 14, pp. 5043–5053, 2010. View at: Publisher Site  Google Scholar
 Y. Jiang, H. Pang, and B. Liao, “Removal of copper(II) ions from aqueous solution by modified bagasse,” Journal of Hazardous Materials, vol. 164, no. 1, pp. 1–9, 2009. View at: Publisher Site  Google Scholar
 Y. S. Ho and G. McKay, “Pseudosecond order model for sorption processes,” Process Biochemistry, vol. 34, no. 5, pp. 451–465, 1999. View at: Publisher Site  Google Scholar
 S. Liang, X. Guo, N. Feng, and Q. Tian, “Isotherms, kinetics and thermodynamic studies of adsorption of Cu2+ from aqueous solutions by Mg2+/K+ type orange peel adsorbents,” Journal of Hazardous Materials, vol. 174, no. 13, pp. 756–762, 2010. View at: Publisher Site  Google Scholar
 J. C. M. W. J. Weber Jr., Journal of the Sanitary Engineering Division, pp. 31–60, 1963.
 R. H. W. Zou, Z. Chen, Z. Jinghua, and J. Shi, “Kinetic study of adsorption of Cu(II) and Pb(II) from aqueous solutions using manganese oxide coated zeolite in batch mode,” Colloids and Surfaces A, vol. 279, pp. 238–246, 2006, 10.1016/j.colsurfa.2006.01.008. View at: Google Scholar
 V. S. Mane, I. Deo Mall, and V. Chandra Srivastava, “Kinetic and equilibrium isotherm studies for the adsorptive removal of Brilliant Green dye from aqueous solution by rice husk ash,” Journal of Environmental Management, vol. 84, no. 4, pp. 390–400, 2007. View at: Publisher Site  Google Scholar
 J. Febrianto, A. N. Kosasih, J. Sunarso, Y. H. Ju, N. Indraswati, and S. Ismadji, “Equilibrium and kinetic studies in adsorption of heavy metals using biosorbent: A summary of recent studies,” Journal of Hazardous Materials, vol. 162, no. 23, pp. 616–645, 2009. View at: Publisher Site  Google Scholar
 I. Langmuir, “The constitution and fundamental properties of solids and liquids. Part I. Solids,” The Journal of the American Chemical Society, vol. 38, no. 2, pp. 2221–2295, 1916. View at: Google Scholar
 B. Hameed and K. Y. Foo, “Insights into the modeling of adsorption isotherm systems,” Chemical Engineering Journal, vol. 156, pp. 2–10, 2010. View at: Publisher Site  Google Scholar
 O. Hamdaoui and E. Naffrechoux, “Modeling of adsorption isotherms of phenol and chlorophenols onto granular activated carbon. Part I. Twoparameter models and equations allowing determination of thermodynamic parameters,” Journal of Hazardous Materials, vol. 147, no. 12, pp. 381–394, 2007. View at: Publisher Site  Google Scholar
 M. M. MontazerRahmati, P. Rabbani, A. Abdolali, and A. R. Keshtkar, “Kinetics and equilibrium studies on biosorption of cadmium, lead, and nickel ions from aqueous solutions by intact and chemically modified brown algae,” Journal of Hazardous Materials, vol. 185, no. 1, pp. 401–407, 2011. View at: Publisher Site  Google Scholar
 R. A. Anayurt, A. Sari, and M. Tuzen, “Equilibrium, thermodynamic and kinetic studies on biosorption of Pb(II) and Cd(II) from aqueous solution by macrofungus (Lactarius scrobiculatus) biomass,” Chemical Engineering Journal, vol. 151, no. 13, pp. 255–261, 2009. View at: Publisher Site  Google Scholar
 P. A. M. Mourão, P. J. M. Carrott, and M. M. L. Ribeiro Carrott, “Application of different equations to adsorption isotherms of phenolic compounds on activated carbons prepared from cork,” Carbon, vol. 44, no. 12, pp. 2422–2429, 2006. View at: Publisher Site  Google Scholar
 S. N. Milmile, J. V. Pande, S. Karmakar, A. Bansiwal, T. Chakrabarti, and R. B. Biniwale, “Equilibrium isotherm and kinetic modeling of the adsorption of nitrates by anion exchange Indion NSSR resin,” Desalination, vol. 276, no. 13, pp. 38–44, 2011. View at: Publisher Site  Google Scholar
 M. I. Temkin, Zhurnal Fizicheskoi Khimii, vol. 15, pp. 296–332, 1941.
 B. Hameed, I. Tan, and A. Ahmad, “Adsorption isotherm, kinetic modeling and mechanism of 2,4,6trichlorophenol on coconut huskbased activated carbon,” Chemical Engineering Journal, vol. 144, pp. 235–244, 2008. View at: Publisher Site  Google Scholar
 Ö. Yavuz, Y. Altunkaynak, and F. Güzel, “Removal of copper, nickel, cobalt and manganese from aqueous solution by kaolinite,” Water Research, vol. 37, no. 4, pp. 948–952, 2003. View at: Publisher Site  Google Scholar
 A. H. Sulaymon, B. A. Abid, and J. A. AlNajar, “Removal of lead copper chromium and cobalt ions onto granular activated carbon in batch and fixedbed adsorbers,” Chemical Engineering Journal, vol. 155, no. 3, pp. 647–653, 2009. View at: Publisher Site  Google Scholar
 T. Gotoh, K. Matsushima, and K. I. Kikuchi, “Preparation of alginatechitosan hybrid gel beads and adsorption of divalent metal ions,” Chemosphere, vol. 55, no. 1, pp. 135–140, 2004. View at: Publisher Site  Google Scholar
 M. He, Y. Zhu, Y. Yang, B. Han, and Y. Zhang, “Adsorption of cobalt(II) ions from aqueous solutions by palygorskite,” Applied Clay Science, vol. 54, pp. 292–296, 2011. View at: Publisher Site  Google Scholar
 S. Dahiya, R. M. Tripathi, and A. G. Hegde, “Biosorption of heavy metals and radionuclide from aqueous solutions by pretreated arca shell biomass,” Journal of Hazardous Materials, vol. 150, no. 2, pp. 376–386, 2008. View at: Publisher Site  Google Scholar
 H. Parab, S. Joshi, N. Shenoy, A. Lali, U. S. Sarma, and M. Sudersanan, “Determination of kinetic and equilibrium parameters of the batch adsorption of Co(II), Cr(III) and Ni(II) onto coir pith,” Process Biochemistry, vol. 41, no. 3, pp. 609–615, 2006. View at: Publisher Site  Google Scholar
 E. Erdem, N. Karapinar, and R. Donat, “The removal of heavy metal cations by natural zeolites,” Journal of Colloid and Interface Science, vol. 280, no. 2, pp. 309–314, 2004. View at: Publisher Site  Google Scholar
 F. T. Awadalla and B. Pesic, “Biosorption of cobalt with the AMTTM metal removing agent,” Hydrometallurgy, vol. 28, no. 1, pp. 65–80, 1992. View at: Google Scholar
 A. Pal, S. Ghosh, and A. K. Paul, “Biosorption of cobalt by fungi from serpentine soil of Andaman,” Bioresource Technology, vol. 97, pp. 1253–1258, 2006, 10.1016/j.biortech.2005.01.043. View at: Google Scholar
 A. Martin, M. Klauck, A. Grenner, R. Meinhardt, D. Martin, and J. Schmelzer, “Liquidliquid(Liquid) equilibria in ternary systems of aliphatic hydrocarbons (Heptane or Octane) + phenols + water,” Journal of Chemical & Engineering Data, vol. 56, no. 4, pp. 741–749, 2011. View at: Publisher Site  Google Scholar
 A. Sari, D. Mendil, M. Tuzen, and M. Soylak, “Biosorption of Cd(II) and Cr(III) from aqueous solution by moss (Hylocomium splendens) biomass: Equilibrium, kinetic and thermodynamic studies,” Chemical Engineering Journal, vol. 144, no. 1, pp. 1–9, 2008. View at: Publisher Site  Google Scholar
 S. Chowdhury, R. Mishra, P. Saha, and P. Kushwaha, “Adsorption thermodynamics, kinetics and isosteric heat of adsorption of malachite green onto chemically modified rice husk,” Desalination, vol. 265, no. 13, pp. 159–168, 2011. View at: Publisher Site  Google Scholar
 O. S. Lawal, A. R. Sanni, I. A. Ajayi, and O. O. Rabiu, “Equilibrium, thermodynamic and kinetic studies for the biosorption of aqueous lead(II) ions onto the seed husk of Calophyllum inophyllum,” Journal of Hazardous Materials, vol. 177, no. 13, pp. 829–835, 2010. View at: Publisher Site  Google Scholar
 A. Tassist, H. Lounici, N. Abdi, and N. Mameri, “Equilibrium, kinetic and thermodynamic studies on aluminum biosorption by a mycelial biomass (Streptomyces rimosus),” Journal of Hazardous Materials, vol. 183, no. 13, pp. 35–43, 2010. View at: Publisher Site  Google Scholar
 M. AlGhouti, M. A. M. Khraisheh, M. N. M. Ahmad, and S. Allen, “Thermodynamic behaviour and the effect of temperature on the removal of dyes from aqueous solution using modified diatomite: A kinetic study,” Journal of Colloid and Interface Science, vol. 287, no. 1, pp. 6–13, 2005. View at: Publisher Site  Google Scholar
 K. J. Laidler and J. M. Meiser, Physical Chemistry, vol. 852, Houghton Mifflin, New York,, 1999.
 T. Mahmood, M. T. Saddique, A. Naeem et al., “Kinetic and thermodynamic study of Cd(II), Co(II) and Zn(II) adsorption from aqueous solution by NiO,” Chemical Engineering Journal, vol. 171, no. 3, pp. 935–940, 2011. View at: Publisher Site  Google Scholar
 A. E. Ofomaja and E. B. Naidoo, “Kinetic modeling of the interaction between copper(II) and calcium hydroxide treated pine cone powder,” Journal of the Taiwan Institute of Chemical Engineers, vol. 42, no. 3, pp. 480–485, 2011. View at: Publisher Site  Google Scholar
 M. Doğan, H. Abak, and M. Alkan, “Adsorption of methylene blue onto hazelnut shell: Kinetics, mechanism and activation parameters,” Journal of Hazardous Materials, vol. 164, no. 1, pp. 172–181, 2009. View at: Publisher Site  Google Scholar
 P. G. R. T.S. Anirudhan, “Thermodynamics and kinetics of adsorption of Cu(II) from aqueous solutions onto a new cation exchanger derived from tamarind fruit shell,” The Journal of Chemical Thermodynamics, vol. 40, pp. 702–709, 2008. View at: Publisher Site  Google Scholar
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Copyright © 2013 Muhammad Imran Din et al. This is an open access article distributed under the Creative Commons Attribution License, which permits unrestricted use, distribution, and reproduction in any medium, provided the original work is properly cited.