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ISRN Physical Chemistry
Volume 2013 (2013), Article ID 171865, 8 pages
Biosorption of Pb(II) from Aqueous Solution Using Cow Hooves: Kinetics and Thermodynamics
1Department of Chemical Sciences, Afe Babalola University, PMB 5454, Ado Ekiti 360101, Nigeria
2Department of Chemistry, Federal University of Technology, PMB 704, Akure 340252, Nigeria
Received 23 April 2013; Accepted 23 May 2013
Academic Editors: T. Panczyk, X. Rozanska, and R. Spezia
Copyright © 2013 I. Osasona 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.
Biosorption of Pb(II) ions from aqueous solution by cow hooves (CHs) was investigated as a function of initial pH, contact time, and biosorbent dosage through batch studies. Equilibrium experiments were performed at three different temperatures (298, 308, and 318 K) using initial Pb2+ concentration ranging from 15 to 100 mgg−1. This study revealed that maximum uptake (96.2% removal) of Pb2+ took place within 30 minutes of agitation, and the process was brought to equilibrium within 60 minutes of equilibration. The equilibrium data were modelled using Langmuir, Freundlich, and Dubinin-Radushkevich (D-R) isotherm models. The Langmuir isotherm model fitted the data best at all temperatures considered. The Lagergren second-order kinetic model fitted the biosorption process better than the first-order model. The negative values obtained for both Gibb’s free energy change and enthalpy change are an indication of the spontaneous and exothermic nature of the sorption of Pb2+ onto CH. A study of the FTIR spectral obtained before and after Pb2+ sorption showed that carbonyl, hydroxyl, amino, and carboxyl groups were involved in the sorption process.
The presence of heavy metals in the environment, particularly the aquatic environment, cannot be over emphasized. Their presence in the environment has become a great threat all over the years because of their nonbiodegradability, toxicity, persistency, and bioaccumulation tendency [1, 2]. Heavy metals are introduced majorly into the environment through wastewater generated from various industrial activities such as mining, electroplating, metal finishing, dyeing, battery manufacturing processes, and production of paints and pigments [3, 4]. Lead is one of the most toxic heavy metals and important contaminants in aquatic environments. Lead can exist in organic and inorganic forms. Both forms have been identified to be poisonous with the former being more poisonous . The maximum allowable limit of Pb considered safe in drinking water by the World Health Organization (WHO) is 50 ppb, whereas less than 15 pp is adopted by the United States Environmental Protection Agency (US EPA) . The permissible limit of lead for effluent discharge to inland surface water is 0.1 mg/L .
Therefore, to conform to these standards and to keep a safe environment, it becomes absolutely necessary to reduce the amount of this deleterious metal from aqueous wastes generated from industries before they are released into the environment. This necessity has seriously enhanced the demand for new technologies for metal removal from wastewater . Various treatment technologies have been developed for the removal of heavy metals from wastewater. The most widely used conventional methods for removing heavy metals from wastewater include ion exchange, chemical precipitation, reverse osmosis, evaporation, and electrodialysis [3, 9]. But most of these treatment technologies are associated with a lot of demerits which include high chemical or energy requirements (which implies high capital and operational cost) and generation of toxic sludge or other secondary products that need to be disposed [8, 10, 11]. Besides, the conventional methods have inadequate efficiencies at low metal concentrations, particularly in the range of 1–100 mg/L .
In recent decades, adsorption has proved to be one of the simplest and most effective treatment methods for the removal of heavy metals from wastewater. Adsorption of heavy metals from wastewater using activated carbon has gained a wide acceptability industrially because of its high porosity, large internal surface area, relatively high mechanical strength, high degree of surface activity, and high affinity for metals [12–14]. However, the use of activated carbon is highly expensive, thereby limiting its use as adsorbent for heavy metal removal from industrial wastewater especially in the third-world countries [15, 16]. This has necessitated the search for low-cost adsorbents, which are cheaply available and environmentally friendly, that can be effective as or even more effective than activated carbon.
Biosorption can be defined as the passive uptake of toxicants by dead/inactive biological materials or by materials derived from biological sources . The major advantages of biosorption over conventional treatment methods include low cost, good efficiency, minimization of chemical and biological sludge, regeneration of biosorbent, and possibility of metal recovery . A number of low-cost biosorbents have been exploited for the removal of lead from wastewaters. These include Pleurotus florida and Trichoderma viride , Streptoverticillium cinnamoneum waste biomass , Pseudomonas putida , Pleurotus ferulae , and native and chemically modified corn corb , Corynebacterium glutamicum .
Cow hoof is an inedible byproduct that can be obtained freely from local abattoirs in Nigeria. Cow hoof is known to contain insoluble protein called keratin  which contains some functional groups such as amino and carboxyl, which may likely enhance biosorption processes. Thousands of cow hooves are burnt off in different abattoirs in Nigeria every day. It has been reported that keratin extracted from cow hooves has been exploited in making a special fire extinguishing foam specifically designed to quell the hotter, high-intensity fires triggered by aviation fuel across the UK . This study is another attempt aimed at turning this agricultural waste into valuable use.
This study was aimed at investigating the feasibility of using cow hoof powder as an alternative biosorbent for the removal of Pb2+ ions from aqueous solution. The Langmuir, Freundlich, and Dubinin-Raduskevich (D-R) isotherm models were used to fit the equilibrium data while Lagergren kinetic models were used for kinetic modelling.
Cow hooves were obtained from an abattoir along Ekiti State University Road, Ado Ekiti, Nigeria. The hooves were thoroughly washed with distilled water and sun-dried for a month. After sun drying, the hooves were washed again with distilled water and oven-dried at 105°C. The dried hooves were ground and sieved using sieve of mesh size 212 μm. A stock solution containing 1000 mgL−1 of Pb(II) was prepared by weighing 1.5984 g of analytical grade Pb(NO3)2 into a 1 L standard flask. This was dissolved and made to mark with distilled water. Standard solutions of different concentrations as might be required were prepared (by dilution) from this stock solution.
2.2. General Procedure for Biosorption Studies
The influence of different parameters like solution pH, equilibration time, and sorbent dosage on the removal of Pb(II) was investigated through batch experiments at 298 K. Half gramme (0.5 g) of CH was suspended in 50 mL of 50 mgL−1 Pb(II) solution in 150 mL conical flasks for each experimental run. This mixture was agitated using thermostatic water bath shaker (SearchTech 82) for 60 minutes unless stated otherwise at a constant speed. The effects of solution pH on the biosorption process were assessed by adjusting the solution pH between 2.0 and 6.0 using dilute HCl or dilute NaOH solution. The solution pH was not adjusted above 6 because precipitation was noticed at pH above 6. HI 2210 pH metre, Hanna Instruments, was used for pH measurement. The effect of contact time was investigated by varying the agitation time from 0 to 150 minutes. For each experimental run, the mixture of the biosorbent and the solution was centrifuged after agitation and the concentration of metal ion present in the liquid phase (supernatant) was determined using atomic absorption spectrometer (AAS). The amount of metal ions adsorbed per unit mass of biosorbent was determined according to the following equation: where is the mass of CH (g), is the volume of the solution , is the initial concentration of metal (mgL−1), is the final concentration of Pb(II) in the liquid phase (mgL−1), and is the amount of metal biosorbed at equilibrium (mgg−1). The percentage biosorption (%), for Pb(II), was calculated using the following expression:
2.3. Equilibrium Studies
Equilibrium isotherm studies were conducted by agitating 0.5 g of CH with 50 mL of lead(II) solution (pH of 3.5) for 60 minutes at 298, 308, and 318 K. The initial metal concentration ranged from 15 to 100 mgL−1. The samples were then centrifuged and analysed as described earlier.
3. Results and Discussion
3.1. FTIR Analysis
The possibility of functional groups involvement in the biosorption of Pb(II) by CH was determined using FTIR spectroscopic analysis. The major functional groups that can be noticed on the biosorbent surface are OH (3314 cm−1 band), C=O (1658.6 cm−1 absorption, band), C-O (1239.11 cm−1 and 1039.63 cm−1), C-C (2931.42 cm−1), and amino group (1530.58 cm−1 and 1393 cm−1) (Figure 1(a)). Most of these absorption bands were altered after Pb(II) biosorption (Figure 1(b) and Table 1), which is an indication of the involvement of these functional groups in the biosorption process.
3.2. Effect of pH on Pb Removal
The effect of pH on the biosorption of Pb(II) by CH is presented in Figure 2. The figure reveals that the biosorption of Pb onto CH was pH dependent. There was little removal of Pb under highly acidic conditions. The biosorption of Pb onto CH increased gradually from pH of 2 (about 50% Pb removal) to 3.5 (about 99% Pb removal) while a decrease in the percentage removal of Pb was noticed at pH above 4. The maximum removal percent of Pb occurred between the pH of 3 and 4. The pH dependence of metal biosorption can be explained by both solution chemistry and the functional groups present on the surface of the biosorbent . At low pH, the surface of the biosorbent is saturated with hydrogen/hydrozonium ions. This creates a competition between the Pb cation and the hydrogen ions for the active sites on the biosorbent surface. This competition brings about decrease in the amount of Pb(II) adsorbed at low pH.
3.3. Effect of Contact Time on Biosorption of Pb(II)
Figure 3 presents the effect of contact time on the adsorption capacity and percentage removal of Pb(II) by CH biomass. The result presented in Figure 3 indicates that there was a rapid removal of Pb(II) within the first ten minutes. In fact, more than 80% removal of Pb(II) occurred within this period. The biosorption rate increased gradually until equilibrium was attained after 60 minutes of agitation. Therefore, an equilibration time of 60 minutes was used for further experiments. The initial high biosorption rate might be linked to the abundance of free binding sites on the biosorbent, which become saturated resulting in decreased biosorption rate . The optimum adsorption capacity () and percentage removal were 4.81 mgg−1 and 96.2%, respectively.
3.4. Effect of CH Dosage
The effect of biosorbent dosage on the removal of lead (II) ions by CH was investigated by agitating CH powder of different masses ranging from 0.3 g to 2.5 g with 50 mL of 50 mgg−1 Pb(II) solution at 298 K. The result of this investigation is presented in Figure 4. The figure reveals that the removal of lead is a function of the mass of CH used. The percentage of metal biosorbed slightly increased from 94.24% to 95.48% when the amount of cow hoof was increased from 0.3 g to 2.5 g. This could happen because the greater the mass of the adsorbent in solution, the greater the number of binding sites available for metal uptake. Conversely, the amount of metal adsorbed per unit mass of CH decreased from 7.85 to 0.95 mgg−1 when the sorbent mass used was increased from 0.3 to 2.5 g.
3.5. Biosorption Isotherms
Analysis of the equilibrium data is important to develop an equation which could be used for design purposes . Several isotherm equations are available for equilibrium modelling in biosorption processes. The biosorption data in this study were described using Langmuir, Freundlich, and Dubinin-Radushkevich isotherm models.
The Langmuir model assumes that the uptake of metal ions occurs on a homogeneous surface by monolayer biosorption without any interaction between the biosorbed ions. The linear form of this model can be expressed as where (mgg−1) is the maximum adsorption capacity and (Lmg−1) is a constant related to the affinity of binding sites or enthalpy of biosorption and should vary with temperature . Straight lines were obtained when a plot of versus was made for different temperatures (Figure 5). Langmuir parameters are important in predicting the affinity between the biosorbate and biosorbent using the dimensionless separation factor , defined as where is the initial concentration of metal (mgL−1) and is Langmuir constant. The affinity between biosorbent and adsorbate is described as irreversible, if ; favourable, if ; linear if , and unfavourable if . The values in this study are shown in Table 2. The values indicate that the biosorption of Pb(II) is favourable and this is more favourable as both the initial metal concentration and temperature increased.
The Freundlich isotherm model gives an expression encompassing the surface heterogeneity and the exponential distribution of active sites and their energies . This model can be expressed linearly as where and are Freundlich constants which are related to sorption capacity and intensity, respectively.
The Dubinin-Radushkevich isotherm which also assumes a heterogeneous surface can be expressed in the following linear form: where is the , is the adsorption capacity of the biosorbent (mgg−1), is a constant related to the adsorption energy (mol2 kJ−2), is the gas constant (kJK−1 mol−1), and is the temperature . D-R isotherm model is important for determining the mean adsorption energy. This sorption energy can be estimated by using the following relationship: The magnitude of the mean adsorption energy is useful for estimating the nature of the biosorption process. If the value of is less than 8 kJmol−1, the biosorption process can be explained by physisorption mechanism, if is between 8 and 16 kJmol−1, the process is dominated by ion exchange mechanism, and if is >16 kJmol−1, the biosorption process is dominated by chemisorption .
The Langmuir, Freundlich, and D-R isotherm parameters at different temperatures are presented in Table 3. A critical look at the correlation coefficients (Table 3) for the three isotherm models reveals that the biosorption process was best fitted by Langmuir model at all temperatures. The maximum adsorption capacities, , calculated from Langmuir equation at 298 K, 308 K, and 308 K are 8.64, 8.912, and 9.52 mgg−1, respectively. The maximum adsorption capacities obtained from Freundlich and D-R models at these temperatures are 3.097, 3.394, and 2.909 L1/n g−1 mg−1/n, and 5.719, 6.948, and 7.38 mgg−1, respectively. The mean biosorption energies were 2.386, 2.312, and 1.694 kJmol−1 at 298 K, 308 K, and 308 K, respectively (Table 3). This shows that the biosorption process was dominated by physisorption mechanism.
A comparison of the adsorption capacities for the biosorption of Pb(II) ions on different biosorbents used in the literature with cow hoof is summarized in Table 4. Although direct comparison of adsorption capacities of different biosorbents is difficult due to the differences in experimental conditions, yet the adsorption capacity of Pb by CH compares favourably well with those reported in the literature.
3.6. Adsorption Kinetics
The adsorption kinetics of the biosorption of Pb(II) were analysed using Lagergren first-order and Lagergren second-order kinetic models . The Lagergren first-order equation is expressed as follows: where is the rate constant for Lagergren first-order equation (min−1) and = amount of metal biosorbed at equilibrium (mgg−1). A plot of log versus gave a straight line confirming the applicability of the Lagergren first-order rate equation. Lagergren second-order sorption rate equation can be expressed as where is the second-order rate constant (gmg−1 min−1). A straight line plot of versus indicates the applicability of second-order model.
The rate constants , , the calculated equilibrium adsorption capacity (cal) from first-order and second-order equations, and the experimental equilibrium adsorption capacity , (exp) (mg/g) are presented in Table 5. It can be observed from the table that the equilibrium adsorption capacity calculated from the first-order equation is different from the experimental value. This coupled with its correlation coefficient can make one conclude that the biosorption process was not properly described by the first-order kinetic. On the other hand, the calculated from the second-order kinetic model is similar to the experimentally determined . Furthermore, the correlation coefficients (Table 5 and Figure 6) for the second-order equation is higher than the corresponding value for the first-order model. This shows that the biosorption of Pb(II) onto CH is better described by Lagergren second-order model suggesting that chemisorption was the rate-determining step.
3.7. Determination of Thermodynamic Parameters
Thermodynamic parameters are important factors that determine the feasibility and spontaneity of an adsorption process. These parameters were determined by carrying out equilibrium studies at different temperatures to obtain corresponding values of and . The equilibrium constant can be calculated from and values using where represents adsorption in mgL−1 at equilibrium and is the equilibrium concentration of the metal in mgL−1. The value of can be obtained from the lowest experimental metal concentration . Vant’ Hoff’s equation is a useful expression that links and with the equilibrium constant as shown below : where is the temperature in Kelvin and is the gas constant (kJmol−1 K−1). The values of the standard enthalpy change () and standard entropy change () were calculated from the slope and intercept of the linear plot of against while the values of at different temperatures were determined using the equation: The thermodynamic parameters are shown in Table 6. The negative values of at all temperatures considered indicate the spontaneous nature of the biosorption process. The removal of Pb by CH can further be described as exothermic based on the negative value of . The low value of indicates that no remarkable change on entropy is associated with the biosorption process, and its negative value is an indication that the biosorption process is spontaneous at low temperatures precisely at temperatures less than 432 K (159°C).
It can be concluded from this study that powder obtained from cow hooves can be utilized as a low-cost biosorbent for the removal of Pb2+ from aqueous solutions with 96.2% efficiency within 30 minutes of agitation. The biosorption process is a function of the biosorbent dosage, the initial solution pH, and temperature. The efficiency of Pb2+ removal increased with increase in the amount of CH dosed while the pH of 3.5 was recorded for maximum Pb2+ removal. The isotherm studies revealed that Langmuir model fitted the equilibrium data better than Freundlich and D-R models. The Langmuir maximum adsorption capacities increased from 8.64 to 9.52 mgg−1 when the temperature was raised from 298 K to 318 K. The FTIR spectral of the unloaded and Pb2+ loaded CH revealed that carbonyl, carboxyl, hydroxyl, and amino groups played a vital role in the biosorption process. The thermodynamic parameters revealed that the biosorption process was exothermic and spontaneous.
- M. Jain, V. K. Garg, and K. Kadirvelu, “Adsorption of hexavalent chromium from aqueous medium onto carbonaceous adsorbents prepared from waste biomass,” Journal of Environmental Management, vol. 91, no. 4, pp. 949–957, 2010.
- Y. Bulut and Z. Baysal, “Removal of Pb(II) from wastewater using wheat bran,” Journal of Environmental Management, vol. 78, no. 2, pp. 107–113, 2006.
- M. E. Argun, S. Dursun, C. Ozdemir, and M. Karatas, “Heavy metal adsorption by modified oak sawdust: thermodynamics and kinetics,” Journal of Hazardous Materials, vol. 141, no. 1, pp. 77–85, 2007.
- A. Sari and M. Tuzen, “Biosorption of cadmium(II) from aqueous solution by red algae (Ceramium virgatum): equilibrium, kinetic and thermodynamic studies,” Journal of Hazardous Materials, vol. 157, no. 2-3, pp. 448–454, 2008.
- K. R. Krishna and L. Phillip, “Bioremediation of Cr (VI) in contaminated soils,” Journal of Hazardous Materials, vol. 121, pp. 109–117, 2005.
- B. Volesky, “Detoxification of metal-bearing effluents: biosorption for the next century,” Hydrometallurgy, vol. 59, no. 2-3, pp. 203–216, 2001.
- TERI Energy Data Directory & Yearbook, Tata Energy Research Institute, New Delhi, India, 2005-2006.
- A. Ratnakumari and K. Sobha, “Biosorption of Cu2+ using animal polymers: chick and duck feathers,” International Journal of Research in Pharmaceutical and Biomedical Sciences, vol. 3, no. 2, pp. 664–669, 2012.
- S. Khatoon, J. Anwar, M. Hassan, R. Farooq, H. B. Fatima, and H. N. Khalid, “Removal of chromium (VI) by biosorption on Eucalptus bark,” World Applied Science Journal, vol. 6, no. 12, pp. 1638–1643, 2009.
- M. A. Tofighy and T. Mohammadi, “Adsorption of divalent heavy metal ions from water using carbon nanotube sheets,” Journal of Hazardous Materials, vol. 185, no. 1, pp. 140–147, 2011.
- M. A. Khan, R. A. K. Rao, and M. Ajmal, “Heavy metal pollution and its control through nonconventional adsorbents (1998–2007): a review,” Journal of International Environmental Application & Science, vol. 3, no. 2, pp. 101–141, 2008.
- P. S. Kumar, S. Ramalingam, R. V. Abhinaya, S. D. Kirupha, A. Murugesan, and S. Sivanesan, “Adsorption of metal ions onto the chemically modified agricultural waste,” Clean—Soil, Air, Water, vol. 40, no. 2, pp. 188–197, 2012.
- N. Nasuha, B. H. Hameed, and A. T. M. Din, “Rejected tea as a potential low-cost adsorbent for the removal of methylene blue,” Journal of Hazardous Materials, vol. 175, no. 1–3, pp. 126–132, 2010.
- M. A. Hossain, H. H. Ngo, W. S. Guo, and T. V. Nguyen, “Biosorption of Cu (II) from water by banana peel base biosorbent: experiments and models of adsorption and desorption,” Journal of Water Sustainability, vol. 1, pp. 87–104, 2012.
- I. Osasona, A. O. Adebayo, and O. O. Ajayi, “Adsorptive removal of chromium (VI) from aqueous solution using cow hooves,” Journal of Scientific Research and Reports, vol. 2, no. 1, pp. 288–303, 2013.
- L. Wang, J. Zhang, R. Zhao, Y. Li, C. Li, and C. Zhang, “Adsorption of Pb(II) on activated carbon prepared from Polygonum orientale Linn.: kinetics, isotherms, pH, and ionic strength studies,” Bioresource Technology, vol. 101, no. 15, pp. 5808–5814, 2010.
- K. Vijayaraghavan and Y.-S. Yun, “Bacterial biosorbents and biosorption,” Biotechnology Advances, vol. 26, no. 3, pp. 266–291, 2008.
- A. S. A. Prasad, G. Varatharaju, C. Anushri, and S. Dhivyasree, “Biosorption of lead by Pleurotus florida and Trichoderma viride,” British Biotechnology Journal, vol. 3, no. 1, pp. 66–78, 2013.
- P. R. Puranik and K. M. Paknikar, “Biosorption of lead and zinc from solutions using Streptoverticillium cinnamoneum waste biomass,” Journal of Biotechnology, vol. 55, no. 2, pp. 113–124, 1997.
- R. Pardo, M. Herguedas, E. Barrado, and M. Vega, “Biosorption of cadmium, copper, lead and zinc by inactive biomass of Pseudomonas putida,” Analytical and Bioanalytical Chemistry, vol. 376, no. 1, pp. 26–32, 2003.
- A. O. Adebayo, “Investigation on Pleurotus ferulae potential for the sorption of Pb (II) from aqueous solution,” Bulletin of Chemical Society of Ethiopia, vol. 27, no. 1, pp. 25–34, 2013.
- G. Tan, H. Yuan, Y. Liu, and D. Xiao, “Removal of lead from aqueous solution with native and chemically modified corncobs,” Journal of Hazardous Materials, vol. 174, no. 1–3, pp. 740–745, 2010.
- S. B. Choi and Y.-S. Yun, “Lead biosorption by waste biomass of Corynebacterium glutamicum generated from lysine fermentation process,” Biotechnology Letters, vol. 26, no. 4, pp. 331–336, 2004.
- E. Fuchs, “Keratins and the skin,” Annual Review of Cell and Developmental Biology, vol. 111, pp. 23–153, 1995.
- BBC News, “The unsual uses for animal body parts,” June 2011, http://www.bbc.co.uk/news/mobile/science-environment-13670184.
- M. Riaz, R. Nadeem, M. A. Hanif, T. M. Ansari, and K.-U. Rehman, “Pb(II) biosorption from hazardous aqueous streams using Gossypium hirsutum (Cotton) waste biomass,” Journal of Hazardous Materials, vol. 161, no. 1, pp. 88–94, 2009.
- Z. Aksu, “Determination of the equilibrium, kinetic and thermodynamic parameters of the batch biosorption of nickel(II) ions onto Chlorella vulgaris,” Process Biochemistry, vol. 38, no. 1, pp. 89–99, 2002.
- S. Tunali, A. Çabuk, and T. Akar, “Removal of lead and copper ions from aqueous solutions by bacterial strain isolated from soil,” Chemical Engineering Journal, vol. 115, no. 3, pp. 203–211, 2006.
- C.-C. Lin and Y.-T. Lai, “Adsorption and recovery of lead(II) from aqueous solutions by immobilized Pseudomonas aeruginosa PU21 beads,” Journal of Hazardous Materials, vol. 137, no. 1, pp. 99–105, 2006.
- G. Vazquez, G. Antorrena, J. Gonzalez, and M. D. Doval, “Adsorption of heavy metal ions by chemically modified Pinus pinaster bark,” Bioresource Technology, vol. 48, no. 3, pp. 251–255, 1994.
- S. V. Kertman, G. M. Kertman, and Z. S. Chibrikova, “Peat as a heavy metal sorbent,” Journal of Applied Chemistry of the USSR, vol. 66, no. 2, pp. 465–466, 1993.
- W.-B. Lu, J.-J. Shi, C.-H. Wang, and J.-S. Chang, “Biosorption of lead, copper and cadmium by an indigenous isolate Enterobacter sp. J1 possessing high heavy-metal resistance,” Journal of Hazardous Materials, vol. 134, no. 1–3, pp. 80–86, 2006.
- R. Zacaria, C. Gerente, Y. Andres, and P. le Cloirec, “Adsorption of several metal ions onto a low-cost biosorbent: kinetic and equilibrium studies,” Environmental Science and Technology, vol. 36, no. 9, pp. 2067–2073, 2002.
- I. Mobasherpour, E. Salahi, and M. Pazouki, “Removal of nickel (II) from aqueous solutions by using nano-crystalline calcium hydroxyapatite,” Journal of Saudi Chemical Society, vol. 15, no. 2, pp. 105–112, 2011.
- B. S. Krishna, D. S. R. Murty, and B. S. J. Prakash, “Thermodynamics of chromium(VI) anionic species sorption onto surfactant-modified montmorillonite clay,” Journal of Colloid and Interface Science, vol. 229, no. 1, pp. 230–236, 2000.
- Q. Li, J. Zhai, W. Zhang, M. Wang, and J. Zhou, “Kinetic studies of adsorption of Pb(II), Cr(III) and Cu(II) from aqueous solution by sawdust and modified peanut husk,” Journal of Hazardous Materials, vol. 141, no. 1, pp. 163–167, 2007.
- R. Han, W. Zou, W. Yu, S. Cheng, Y. Wang, and J. Shi, “Biosorption of methylene blue from aqueous solution by fallen phoenix tree's leaves,” Journal of Hazardous Materials, vol. 141, no. 1, pp. 156–162, 2007.
- J. O. Babalola, N. A. A. Babarinde, O. A. Popoola, and V. O. Oninla, “Kinetic, isothermal and thermodynamic studies of the biosorption of Ni(II) and Cr(III) from aqueous solutions by Talinum triangulare (water leaf),” The Pacific Journal of Science and Technology, vol. 10, no. 1, pp. 439–450, 2009.