Research Article | Open Access
Priya Meethale Kunnambath, Santhi Thirumalaisamy, "Characterization and Utilization of Tannin Extract for the Selective Adsorption of Ni (II) Ions from Water", Journal of Chemistry, vol. 2015, Article ID 498359, 9 pages, 2015. https://doi.org/10.1155/2015/498359
Characterization and Utilization of Tannin Extract for the Selective Adsorption of Ni (II) Ions from Water
The current paper studies the preparation of a new tannin gel from Acacia nilotica for water purification and waste water remediation. Design of experiments is used for optimizing the tannin gel using tannin extract (Taguchi method) with formaldehyde in the assistance of microwave (TGAN) by the help of iodine number. The feasible combinations were tested in the removal of nickel from simulated and river water. In this study, the effect of adsorbent dosage, pH, and initial metal concentration on Ni (II) biosorption on modified Acacia nilotica tannin gel (TGAN) was investigated. Tannin gel was characterized by SEM, FTIR, XRD, and EDAX. The kinetic data was tested using pseudo-first-order, pseudo-second-order, and intraparticle diffusion model. The results suggested that the pseudo-second-order model (R2 > 0.998) was the best choice among all the kinetic models describing the adsorption behavior of Ni (II) onto TGAN. Langmuir, Freundlich, Temkin, and Dubinin-Radushkevich adsorption models were used to represent the equilibrium data. The best interpretation for the experimental data was given by the Langmuir isotherm and the maximum adsorption capacity 250 mg g−1 of Ni (II) was obtained at pH 5.04 at 296 K. Adsorption of Ni (II) onto TGAN is confirmed qualitatively by the use of atomic absorption spectroscopy. The BOD and COD values are considerably reduced after adsorption.
Heavy metal ions such as Pb, Cd, Hg, Cr, Ni, Zn, and Cu are nonbiodegradable, toxic, and carcinogenic even at very low concentrations and, hence, usually pose a serious threat to the environmental and public health . Many industries discharge heavy metals such as lead, cadmium, copper, nickel, and zinc in their wastewaters . Metals such as copper and nickel are known to be essential to plants, humans, and animals, but they can also have adverse effects if their availability in water exceeds certain threshold values. Nickel is a toxic heavy metal that is widely used in silver refineries, electroplating, zinc base casting, and storage battery industries . The chronic toxicity of nickel to humans and the environment has been well documented. For example, high concentration of nickel causes cancer of lungs, nose, and bone.
For this reason, the advanced treatment processes such as chemical reduction, ion exchange, reverse osmosis, electro dialysis and activated carbon adsorption are generally used. Since the cost of these processes is rather expensive, the use of agricultural residues or industrial by-product having biological activities has been received with considerable attention. In recent years, a number of agricultural materials such as sugar cane waste , grain , palm fibres , Annona squamosa seed , coir pith , and granular Muntingia calabura  have been reported for the removal of toxic metals from aqueous solutions using adsorption.
Tannins, natural biomass containing multiple adjacent hydroxyl groups and exhibiting specific affinity to metal ions, can probably be used as alternative, effective, and efficient adsorbents for the recovery of metal ions. During the last years, the interest on biomaterials and specifically in tannins was growing. The term tannins cover many families of chemical compounds. Traditionally, they have been used for tanning animal skins, hence their name, but one also finds several of them used as water treatment agents. Their natural origin is as secondary metabolites of plants  occurring in the bark, fruit, leaves, and so forth. While Acacia and Schinopsis bark constitute the principal source of tannins for the leather industry, the bark of other nontropical trees such as Quercus ilex, suber, and robur, Castanea, and Pinus can also be tannin-rich. Agricultural by-products have high volume, low value, and underutilized lignocellulosic biomaterials and contain high levels of cellulose, hemicellulose, and lignin.
However, tannins are water-soluble compounds; thus, when they are used directly as an adsorbent for recovery of metals from aqueous systems, they have the disadvantage of being leached by water. To overcome this disadvantage, attempts have been made to immobilize tannins onto various water-insoluble matrices .
More recently, tannin has emerged as a potential alternative for the removal of heavy metals from aqueous solutions [11, 12]. Tannins are natural plant extracts and contain high content of multiple adjacent phenolic hydroxyls in their molecules, and thus they have strong chelating ability towards many heavy metal ions including Cr (III), Pb (II), Hg (II), Cd (II), and Au (II). Biosorption, a biological method of environmental control, can be an alternative to conventional waste-treatment facilities . The concept of biosorption refers to the passive sorption and/or complexation of metal ions by biomass . As tannins contain an abundant amount of adjacent hydroxyl groups more than the adsorbent-like carbon in their molecules, they form chelates with metals. Since tannins are water-soluble compounds, they often need to be immobilized onto water-insoluble matrixes such as cellulose , hydrotalcite , and collagen fiber .
Acacia nilotica is native to Africa and the Indian subcontinent and it grows throughout the drier parts of India. In Haryana, Acacia nilotica based agro forestry systems reduce the yield of wheat. Many researchers synthesized adsorbents from commercial tannins and applied them to remove heavy metals from waste water, such as uranium , chromium , copper , and lead . The objective of this study is to systematically examine adsorption mechanisms, adsorption isotherms, adsorption kinetics, and properties of a tannin gel adsorbent prepared from leaves of Acacia nilotica (TGAN) for removal of Ni (II) ions from aqueous solutions.
2. Experimental Section
All the chemicals used in this study were of analytical reagent grade and were utilized without further purification. The leaves of Acacia nilotica were obtained from the agricultural farm in Coimbatore district (Tamil Nadu). They were washed with distilled water to remove dirt, dust, and surface impurities. Washed leaves are then air-dried in room temperature and powdered in a grinder.
2.2. Preparation of Tannin Extracts
100 g of Acacia nilotica leaves powder was cleaned and it was put in 600 mL of distilled water. Then, 5 g of NaOH was added and the mixture was stirred in magnetic stirrer at 90°C for 1 hour. Solids were separated by filtration and liquid fraction was dried in oven (65°C) overnight. Resultant was considered as tannin resin (TR). Total phenol content of tannin content was calculated. Design of experiments was carried out by using SPSS 14.0 for Windows  and L16 matrix by Taguchi method . Tannin gel was prepared according to this by taking 4 variables. Up to 16 different combinations regarding three variables were attempted. The feasible combinations were just nine of them; the rest did not jellify.
2.3. Preparation of Tannin Gel (TGAN)
Tannin gels were prepared according to the basis of Nakano et al. . Five grams of tannin extract were dissolved in 32 mL of 0.125 mol L−1 NaOH and 30 mL of distilled water at 80°C. When mixture was homogeneous, certain amount of aldehyde was added and reaction was kept at the same temperature for 8 h until polymerization was considered completed. Then, the apparent gummy product led to complete evaporation of water remains and was dried in oven (65°C) overnight. After drying, tannin rigid gels were crushed and sieved to produce tiny diameters. They were washed successively with distilled water and 0.01 mol/L HNO3 to remove unreached sodium hydroxide. Finally, the adsorbent was dried again in oven at 80°C.
2.4. Preparation of Stock Solution
Samples of nickel sulphate hexahydrate (NiSO·6H2O) and other chemicals were obtained from Aluva, Edayar (Spectrum Reagents and Chemicals Pvt. Ltd.). A Stock solution of 1000 mg/L was prepared by dissolving accurately weighed amounts of nickel sulphate hexahydrate in doses of 1000 mL double-distilled water. Working chromium and nickel solutions were prepared just before use by appropriate dilutions of stock solution.
2.5. Batch Mode Experiments
Batch adsorption experiments were carried out to evaluate the effects of pH, contact time, initial concentration, and adsorption dosage on adsorbed amounts. Tests were carried out to evaluate adsorption kinetics, adsorption isotherms, and desorption of Ni (II) on TGAN. In all sets of experiments, a fixed volume of single metal ion solutions of 50 mL of various concentrations (50, 100, 150, and 200 mg L−1) and, for binary metal solution (BMS), 50 mL volume of BMS solution with 25 mL of 50 mg L−1 concentration of working metal and 25 mL of Ni (II) of various concentrations (10, 20, 30, 40, and 50 mL−1) were taken in a conical flask. pH adjustment was fulfilled by adding 0.1 M HCl or 0.1 M NaOH into the solutions with known initial metal concentrations. Batch adsorption experiments were conducted in 250 mL stoppered flasks containing 200 mg of adsorbent and 50 mL of metal solutions with different concentrations (25–200 mg/L) at the optimum solution pH. The flasks were agitated using a mechanical orbital shaker and maintained at room temperature for 2 h at a fixed shaking speed of 120 rpm until the equilibrium was reached. The suspensions were filtered and metal concentrations in the supernatant solutions were measured using a Shimzadu UV-vis spectrophotometer. Supernatants were analyzed by flame atomic absorption spectrophotometer (AAS) for the qualitative analysis. From the initial and final concentrations, percentage removal can be calculated by the use of the following formula: where is the initial concentration of Ni (II) ions in mg/L and is the final concentration of Ni (II) ions in mg/L. The results obtained in batch mode were used to calculate the equilibrium metal uptake capacity. The amounts of uptake and Ni (II) ions by TGAN in the equilibrium () were calculated by the following mass-balance relationship: where is the equilibrium uptake capacity in mg/g, is the sample volume in liters, is the initial metal ion concentration in mg/L, the equilibrium metal ion concentration in mg/L, and is the dry weight of adsorbent in grams.
2.6. BOD and COD Analysis
Biochemical oxygen demand or BOD is the amount of dissolved oxygen needed by aerobic biological organisms in a body of water to break down organic material present in a given water sample at certain temperature over a specific time period.
COD or chemical oxygen demand is the total measurement of all chemicals (organic and inorganic) in the water/waste water. Which are commonly found carbon but it varies based on the industrial process and nature of the raw materials used. These parameters (BOD and COD) are usually associated with sewage, not with drinking water. The ratio of COD/BOD describes organic toxicity because COD is a measure of total (toxic and nontoxic) organic and BOD is a measure of nontoxic organic load. The aim of any waste water treatment should be to reduce this ratio.
3. Result and Discussion
3.1. Optimization of TGAN Preparation Conditions
In order to optimize the preparation conditions of the TGAN, Taguchi experimental design method was used. The variables shown in Table 1 are used for making the orthogonal array. Iodine is considered as probe molecule for assessing the adsorption capacity of adsorbents for solutes of molecular sizes less than 10 Å. Iodine number was normally listed as specification parameter for TGAN. Iodine number and the yield of gel prepared under optimum conditions were 583.16 (mg/g) and 65.08%, respectively. The TGAN was used in the characterization analysis and adsorption experiments which were prepared under optimum conditions .
3.2. XRD Analysis
Adsorption reaction may lead to changes in molecular and crystalline structure of the adsorbent and hence an understanding of the molecular and crystalline structures of the adsorbent and the resulting changes thereof would provide valuable information regarding adsorption reaction. Hence, XRD patterns of the adsorbent before and after adsorption of Ni (II) ions have been studied. As a representative case, the XRD patterns of TGAN before and after treatment with Ni (II) ions are shown in Figure 1. -axis represents the intensity. The results indicated that the diffraction profiles of TGAN before and after adsorption of Ni (II) ions exhibited broad peaks and the absence of a sharp peak revealed a predominantly amorphous structure; the broad peak seems to appear at around 2θ = 42, 53, 35 and 29° is confirmed as a tannin gel which was similar to the peak of crystalline carbonaceous structure such as graphite . Small peaks correspond to impurities naturally present in tannins. It is evident from the figure that the XRD pattern of TGAN loaded with Ni (II) ions exhibits no variation in the crystal structure and this suggests that the Ni (II) ions might diffuse into micropores and sorbs mostly by physisorption without altering the structure of the adsorbent. From the XRD analysis for the adsorbent (TGAN), we concluded that the tannin gel preparation was completed.
3.3. FTIR Analysis
Surface functional groups were detected by Fourier transform infrared (FTIR) spectroscope from the scanning range (4000 cm−1–400 cm−1) and elemental analysis was performed using an elemental analysis. An FTIR spectrum for TGAN before and after adsorption of nickel ions shows in Figure 2 and the wide range of 3200–3600 cm−1 show that phenolic –OH groups are intensively present within the nature of raw tannin. Generally, wide bands in the range of 3550–3100 cm−1 correspond to –OH bridging groups in all systems and, here, bands between 3304 and 3361 cm−1 and show the presence of the same groups. The small peaks in the region of 2854–2927 cm−1 are associated with the methylene (–CH2–) bridges of the tannin resin. The peaks at 1058–1105 cm−1 in the spectrum are due to C–O stretching and C–H deformation. The absorption bands between 1631 cm−1 and 1452 cm−1 are characteristic of the elongation of the aromatic –C–H– bonds. The peak around 1190 cm−1 is due to the presence of ether (C–O–C) groups. The deformation vibration of the carbon–carbon bonds in the phenolic groups absorbs in the region of 1500–1400 cm−1 .
3.4. Scanning Electron Microscope
The surface structure of the adsorbents TGAN before and after adsorption was analyzed by scanning electron microscopy (SEM). SEM images for the samples of TGAN before and after metal ion adsorptions are shown in Figures 3 and 4, respectively. As expected from the textural analysis, the sample TGAN exhibits a rough porous surface. The images obtained with the gel foam shows that strong modifications of the surface occur during the activation process. Ripples and dimples appear on the cell wall surfaces during activation and a consequent increase of the surface area is obtained. The pores are different after adsorption as its size cannot visible clearly because it is completely filed with the metal ions.
3.5. Energy Dispersive X-Ray Spectroscopic Analysis (EDAX)
The adsorption efficiency of TGAN was confirmed by EDAX analysis results. The EDAX spectrum of TGAN shows elements present in tannin gel. The EDAX spectra of TGAN and TGAN-Ni are shown in Figure 4. This micrograph reveals the appearance of Ni (II) ion on the surface of TGAN. EDAX spectra showed the presence of O, C, Ca, K, and Zn in the adsorbent. These have been known as the principle elements of the adsorbents. These are summarized in Table 2.
3.6. Effect of pH on Metal Uptake
Figure 5 shows the effect of pH on the metal adsorption by TGAN. Adsorption of Ni (II) increases due to the fact that the dissociation of active groups on the TGAN surface was also increased with pH, that is, when pH increases from 2 to 7, probably due to the acidic dissociation of the phenolic hydroxyl groups of tannin, resulting in strongly complex ability with metal ions. The maximum uptake for Ni (II) is at pH 5.04. As though, the initial pH was fixed at pH 5 in all sorption. At pH above the zero point charge (pHzpc = 5.12), the negatively charged carboxylate ions (–COOA) have strong coordinative affinity toward positively charged metal ions and also, at high pH values higher than 5.12, these metal ions in the precipitated because of the high concentration at these pH values could not be performed well. Furthermore, the phenolic hydroxyl groups of the TGAN would more readily be oxidized, making it impractical to apply this approach above pH 8.0 . The electrostatic forces of attraction allow the carboxylate ions to capture the metal ions through surface complexation, forming chelate complexes . The degree of surface complexation increases with increasing pH. Hence, maximum adsorption capacity occurs at pH 5.04 for Ni (II). At pH 5.04, adsorption of Ni (II) on tannin gel was found to be 76.5%.
3.7. Effect of Initial Metal Ion Concentration
Figure 6 shows the experimental results of adsorption of Ni (II) ions on the TGAN at various concentrations (25, 50, 75, 100, 125, 150, 175, and 200). The result shows that the percentage of adsorption decreased with the increase in initial nickel ion concentration. This is due to the fact that, at low concentration, the ration of initial number of nickel ion to the available surface area is low and subsequently the effect of adsorption is independent of initial concentration. This is due to the fact that, by increasing the concentration of metal ions in solution, the availability of metal at the interface also increases, thus increasing the amount of adsorption. When the surface active sites are fully covered, the extent of adsorption reaches a limit resulting in saturated adsorption .
3.8. Effect of Contact Time
The percentage removal was found to increase with increasing contact time (Figure 7) and then it became almost stable, denoting attainment of equilibrium as so the maximum value at 35 min for Ni (II) ions. Figure 7 shows the effect of time for the adsorption of Ni (II) onto TGAN. This may be due to the fact that once a certain amount of Ni (II) ions gets doped onto these adsorbents within a given time, no more doping occurs afterward; that is, the doping level might have been reached. That is, initially, all adsorbent sites were vacant and the solute concentration was high, and, after that period, only a very low increase in the metal update was observed because there are few surface active sites on TGAN. From these results, it is suggested that only a minimum time is required for the adsorption of metal ion from tannin gel prepared by Acacia nilotica leaves.
3.9. Effect of Adsorbent Dose
The dependence of Ni (II) adsorption on dose was studied by varying the amount of adsorbents from 0.05 to 1 g/L, by keeping the other parameters (pH, contact time, and initial metals concentration) constant. From Figure 8, it could be observed that removal efficiency of the adsorbent generally increased with increasing dose. The increase in removal efficiency with increasing adsorbent dose is probably due to the greater adsorbent surface area and pore volume available at higher adsorbent dose providing more functional groups and active adsorption sites that result in a higher removable percentage. When the surface active sites are fully covered, the extent of adsorption reaches a limit resulting in saturated adsorption. The drop in adsorption capacity is due to the sites remaining unsaturated during the adsorption process. Thus, further experiments were carried out using 200 mg of adsorbent per 50 mL of Ni (II) ion solutions, as it exhibits appreciable removal capacity, for the optimization of adsorption parameters. The maximum adsorption capacity of Ni (II) on to Acacia nilotica surface was estimated to be 250 mg/L at 100 ppm.
3.10. Application of Adsorption Isotherm Models for the Metal Adsorption
Adsorption isotherm is the most important information which indicates how the adsorbate molecules distribute between the liquid phase and the solid phase when adsorption process reaches equilibrium state. When the system is at equilibrium, this is important to determine the maximum sorption capacity of TGAN towards metal solution. Equilibrium data are a basic requirement for the design of adsorption systems and adsorption models, which are used for the mathematical description of the adsorption equilibrium of the metal ion by the adsorbent. The results obtained for adsorption of Ni (II) ions were analyzed by use of well-known models given by the Langmuir, Freundlich, Temkin, and Dubinin-Radushkevich, adsorption isotherm models [29–31]. For the sorption isotherms, initial metal ion concentration was varied whereas solution pH and amount of adsorbent were held constant. The sorption isotherm for Ni (II) ions was obtained for TGAN at solution pH 5.04. Consider where is the Ni (II) ion concentration in the solution (mg/L), is the Ni (II) concentrations in the solid adsorbent (mg/g), is the maximum adsorption capacity (mg/g), is a constant related to the adsorption capacity (mg/, /), is adsorption intensity, is a constant related to the energy of adsorption (L/g), is a constant related to the energy of adsorption, (L/g) is Temkin constant representing adsorbent-adsorbate interactions and β (mgL−1) is another constant related to adsorption heat, and is the Polanyi constant. The adsorption isotherm parameters for all the four isotherm models are calculated and the values are summarized in Table 3.
It can be seen that the Langmuir isotherm fits the data better than Freundlich; D-R and Temkin isotherms with the linear regression coefficients, , TGAN, have a homogeneous surface for adsorption of metal ions. This high value indicates that the adsorption of nickel ions onto TGAN takes place as monolayer adsorption on a surface that is homogeneous in surface affinity. The Langmuir isotherm equation is therefore expected to best represent the equilibrium adsorption data. The values for the Langmuir model are closer to unity than those for the other isotherm models for TGAN ().
3.11. Kinetics Study for Ni (II) onto TGAN
The study of adsorption kinetics describes the solute uptake rate and evidently this rate controls the residence time of the adsorbate at the solid solution interface. The rate of adsorption can be computed from the kinetic study. In order to find out the mechanism of adsorption and potential rate controlling steps such as chemical reaction, diffusion control, and mass transport process, kinetic models have been used to test experimental data from the adsorption of Ni (II) ions onto TGAN. These kinetic models were analyzed using pseudo-first-order, pseudo-second-order, and intraparticle diffusion models which were, respectively, presented as follows [32–35]: where is the contact time of adsorption experiment (min); (mg/g) and (mg/g) are, respectively, the adsorption capacity at equilibrium and at any time ; (1/min), (g/mg min), (mg/g min), (g/mg), and (mg/g min1/2) are the rate constants for these models, respectively. The correlation coefficients for all the four kinetic models were calculated and the results are shown in Table 4.
The adsorption process of Ni (II) ions can be well fitted by use of the pseudo-second-order rate constant for TGAN. The linear regression coefficient value for Ni (II) obtained for pseudo-second-order kinetics was closer to unity than the value 0.934 for Ni (II) ions for first-order kinetics. This indicates that adsorption of Ni (II) ions by TGAN follows pseudo-second-order kinetics.
3.12. Atomic Absorption Spectroscopy and BOD and COD Analysis
Atomic absorption spectrophotometer analysis was done for the TGAN gel treated with metal solutions nickel. Comparatively, nickel showed better adsorption using TGAN. For tannin gel, nickel content before adsorption onto TGAN is 10.30 mg/L and is decreased to 5.50 mg/L. The values of BOD of water before and after adsorption of Ni (II) and the AAS results are given in the Table 5. This shows that the values decrease from before to after as though it explains the efficiency of the TGAN produced from Acacia nilotica leaves for Ni (II) adsorption.
Desorption studies were carried out using different HCl concentration solutions (0.05, 0.1, 0.2, and 0.3). To keep the cost of biosorption process down, our results indicate that TGAN biosorbent could be used repeatedly in Ni (II) biosorption, the repeated availability of the adsorbents after adsorption. Figure 9 shows the desorption ability and recycling ability. Desorption cycles are crucial to illustrate the stability and potential recovery of the adsorbents. Desorption by 0.2 N HCl solution easily occurring might be related to the intensive competition between H+ ions (introduced by HCl solution) and metal ions on the active sites. Meanwhile, at low pH value, the complexation between the adsorbent and metal ions was destroyed [36, 37]. These results illustrated that the TGAN possesses the ability of regeneration and repeated use in heavy metal removal with slight losses in their initial adsorption capacities.
After desorption, the adsorbents were further used for adsorption of Ni (II) ions. The percentage removal of Ni (II) ion was found to be 59.64% for TGAN at pH 8. The increase in removal of Ni (II) ions at pH 9 may be because of precipitation of metal ions in alkaline medium rather than adsorption.
The present study showed that tannin gel prepared from Acacia nilotica leaf can be an effective adsorbent for the removal of Ni (II) from aqueous solution. The adsorption process is dependent on the contact time, pH, and dosage and initial metal ion concentration. The Langmuir isotherm model gave a better fit than other isotherms for interpreting the adsorption phenomenon. The Ni (II) adsorption system followed a pseudo-second-order kinetic model. The removal efficiency increased with an increase in agitation time and adsorbent dosage. By applying the kinetic models to the experimental data, it was found that the kinetics Ni (II) ions adsorption onto TGAN was followed by the pseudo-second-order rate equation. The amount of metal is reduced and so it is proved qualitatively using atomic absorption spectroscopy. Results of kinetic studies demonstrated that the Ni adsorption was rapid and efficient. Desorption of Ni (II) from the spent adsorbent was achieved with 0.2 N HCl. The use of Acacia nilotica as an adsorbent seems to be an economical and worthwhile alternative compared to conventional methods for the removal of Ni (II) from aqueous solution.
Conflict of Interests
The authors have declared that no conflict of interests exists.
- C. Liu, R. Bai, and Q. San Ly, “Selective removal of copper and lead ions by diethylenetriamine-functionalized adsorbent: behaviors and mechanisms,” Water Research, vol. 42, no. 6-7, pp. 1511–1522, 2008.
- K. K. Krishnani, X. Meng, C. Christodoulatos, and V. M. Boddu, “Biosorption mechanism of nine different heavy metals onto biomatrix from rice husk,” Journal of Hazardous Materials, vol. 153, no. 3, pp. 1222–1234, 2008.
- K. Kadirvelu and C. Namasivayam, “Agricultural by-product as metal adsorbent: sorption of lead(II) from aqueous solution onto coirpith carbon,” Environmental Technology, vol. 21, no. 10, pp. 1091–1097, 2000.
- V. K. Gupta and I. Ali, “Removal of lead and chromium from wastewater using bagasse fly ash—a sugar industry waste,” Journal of Colloid and Interface Science, vol. 271, no. 2, pp. 321–328, 2004.
- K. S. Low, C. K. Lee, and S. C. Liew, “Sorption of cadmium and lead from aqueous solutions by spent grain,” Process Biochemistry, vol. 36, no. 1-2, pp. 59–64, 2000.
- K. S. Low, C. K. Lee, and K. P. Lee, “Sorption of copper by dye-treated oil-palm fibres,” Bioresource Technology, vol. 44, no. 2, pp. 109–112, 1993.
- T. Santhi, S. Manonmani, and T. Smitha, “Kinetics and isotherm studies on cationic dyes adsorption onto annona squmosa seed activated carbon,” International Journal of Engineering Science and Technology, vol. 2, no. 3, pp. 287–295, 2010.
- T. Santhi, S. Manonmani, and S. Ravi, “Uptake of cationic dyes from aqueous solution by biosorption onto granular Muntingia calabura,” E-Journal of Chemistry, vol. 6, no. 3, pp. 737–742, 2009.
- P. Schofield, D. M. Mbugua, and A. N. Pell, “Analysis of condensed tannins: a review,” Animal Feed Science and Technology, vol. 91, no. 1, pp. 21–40, 2001.
- X. Liao, Z. Lu, M. Zhang, X. Liu, and B. Shi, “Adsorption of Cu(II) from aqueous solutions by tannins immobilized on collagen,” Journal of Chemical Technology and Biotechnology, vol. 79, no. 4, pp. 335–342, 2004.
- B. H. Cruz, J. M. Díaz-Cruz, C. Ariño, R. Tauler, and M. Esteban, “Multivariate curve resolution of polarographic data applied to the study of the copper-binding ability of tannic acid,” Analytica Chimica Acta, vol. 424, no. 2, pp. 203–209, 2000.
- H.-W. Ma, X.-P. Liao, X. Liu, and B. Shi, “Recovery of platinum(IV) and palladium(II) by bayberry tannin immobilized collagen fiber membrane from water solution,” Journal of Membrane Science, vol. 278, no. 1-2, pp. 373–380, 2006.
- O. S. Amuda, A. A. Giwa, and I. A. Bello, “Removal of heavy metal from industrial wastewater using modified activated coconut shell carbon,” Biochemical Engineering Journal, vol. 36, no. 2, pp. 174–181, 2007.
- C. Mack, B. Wilhelmi, J. R. Duncan, and J. E. Burgess, “Biosorption of precious metals,” Biotechnology Advances, vol. 25, no. 3, pp. 264–271, 2007.
- A. Nakajima and T. Sakaguchi, “Recovery of uranium by tannins immobilized onagarose,” Journal of Chemical Technology and Biotechnology, vol. 40, no. 4, pp. 223–232, 1987.
- I. Chibata, T. Tosa, T. Mori, T. Watanabe, and N. Sakata, “Immobilized tannin—a novel adsorbent for protein and metal ion,” Enzyme and Microbial Technology, vol. 8, no. 3, pp. 130–136, 1986.
- X. Huang, L. Jiao, X. Liao, and B. Shi, “Adsorptive removal of as(III) from aqueous solution by Zr(IV)-loaded collagen fiber,” Industrial and Engineering Chemistry Research, vol. 47, no. 15, pp. 5623–5628, 2008.
- T. Sakaguchi and A. Nakajima, “Accumulation of uranium by immobilized persimmon tannin,” Separation Science and Technology, vol. 29, no. 2, pp. 205–221, 1994.
- W. Li, Y. Tang, Y. Zeng, Z. Tong, D. Liang, and W. Cui, “Adsorption behavior of Cr(VI) ions on tannin-immobilized activated clay,” Chemical Engineering Journal, vol. 193-194, pp. 88–95, 2012.
- I. A. Sengil and M. Ozacar, “Biosorption of Cu(II) from aqueous solutions by mimosa tannin gel,” Journal of Hazardous Materials, vol. 157, no. 2-3, pp. 277–285, 2008.
- X.-M. Zhan and X. Zhao, “Mechanism of lead adsorption from aqueous solutions using an adsorbent synthesized from natural condensed tannin,” Water Research, vol. 37, no. 16, pp. 3905–3912, 2003.
- Y. Nakano, K. Takeshita, and T. Tsutsumi, “Adsorption mechanism of hexavalent chromium by redox within condensed-tannin gel,” Water Research, vol. 35, no. 2, pp. 496–500, 2001.
- M. Makeswari and T. Santhi, “Removal of malachite green dye from aqueous solutions onto microwave assisted zinc chloride chemical activated Epicarp of Ricinus communis,” Journal of Water Resource and Protection, vol. 5, pp. 222–238, 2013.
- M. Makeswari and T. Santhi, “Tannin gel derived from Leaves of Ricinus Communis as an adsorbent for the Removal of Cu (II) and Ni (II) ions from aqueous solution,” International Journal of Modern Engineering Research (IJMER), vol. 3, pp. 3255–3266, 2013.
- M. Yurtsever and I. A. Şengil, “Biosorption of Pb(II) ions by modified quebracho tannin resin,” Journal of Hazardous Materials, vol. 163, no. 1, pp. 58–64, 2009.
- X. Liao, L. Li, and B. Shi, “Adsorption recovery of thorium(IV) by Myrica rubra tannin and larch tannin immobilized onto collagen fibres,” Journal of Radioanalytical and Nuclear Chemistry, vol. 260, no. 3, pp. 619–625, 2004.
- T. Santhi, S. Manonmani, and T. Smitha, “Removal of malachite green from aqueous solution by activated carbon prepared from the epicarp of Ricinus communis by adsorption,” Journal of Hazardous Materials, vol. 179, no. 1-3, pp. 178–186, 2010.
- M. Mahramanlioglu, I. Kizilcikli, and I. O. Bicer, “Adsorption of fluoride from aqueous solution by acid treated spent bleaching earth,” Journal of Fluorine Chemistry, vol. 115, no. 1, pp. 41–47, 2002.
- I. Langmuir, “The adsorption of gases on plane surfaces of glass, mica and platinum,” The Journal of the American Chemical Society, vol. 40, no. 9, pp. 1361–1403, 1918.
- H. Freundlich, “Über die Adsorption in Lösungen (Adsorption in solution),” Zeitschrift für Physikalische Chemie, vol. 57, pp. 384–470, 1906.
- I. A. W. Tan, B. H. Hameed, and A. L. Ahmad, “Equilibrium and kinetic studies on basic dye adsorption by oil palm fibre activated carbon,” Chemical Engineering Journal, vol. 127, pp. 111–119, 2011.
- M. M. Dubinin, E. D. Zaverina, and L. V. Radushkevich, “Sorption and structure of activated carbons, I. Adsorption of organic vapours,” Zhurnal Fizicheskoi Khimii, vol. 21, pp. 1351–1362, 1947.
- Y. S. Ho and G. McKay, “Sorption of dye from aqueous solution by peat,” Chemical Engineering Journal, vol. 70, no. 2, pp. 115–124, 1998.
- Y. S. Ho and G. Mckay, “Kinetic models for the sorption of dye from aqueous solution by wood,” Journal of Environmental Science Health Part B: Process Safety and Environmental Protection, vol. 76, pp. 184–185, 1998.
- W. J. Weber Jr. and J. C. Morris, “Kinetics of adsorption on carbon from solution,” Journal of Sanitary Engineering Division, vol. 89, no. 2, pp. 31–60, 1963.
- M.-R. Huang, H.-J. Lu, and X.-G. Li, “Efficient multicyclic sorption and desorption of lead ions on facilely prepared poly(-phenylenediamine) particles with extremely strong chemoresistance,” Journal of Colloid and Interface Science, vol. 313, no. 1, pp. 72–79, 2007.
- Y. Ren, N. Li, J. Feng et al., “Adsorption of Pb(II) and Cu(II) from aqueous solution on magnetic porous ferrospinel MnFe2O4,” Journal of Colloid and Interface Science, vol. 367, no. 1, pp. 415–421, 2012.
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