Personal Research Database

Full Text: 2008\Sep Sci Tec43, 1221.pdf

Abstract: Mercury removal from wastewater is a recognized pollution control challenge today. In the present investigation, the biosorption of Hg(II) onto the dead biomass of four different species of marine Aspergillus, prepared by alkaline treatment, was studied. Among the cultures studied, A. niger was found to be the most efficient for Hg(II) removal. The effects of initial Hg(II) concentration, contact time, pH, temperature, and biosorbent dosage on biosorption were also investigated. It was observed that biosorption equilibriums were established in about 2h. Under the optimum conditions (pH: 3.0, Hg(II) concentration: 250mg/L, biomass dose: 0.8 g/L, temperature: 40°C and contact time: 2h), 40.53 mg Hg(II) was biosorbed per gram of dead biomass of A. niger. Kinetic studies based on fractional power, zero order, first order, pseudo first order, Elovich, second order, and second order rate expressions have also been carried out where the pseudo second order model exhibited best fit to experimental data. The intra-particle diffusion study revealed that film diffusion is the rate-limiting sorption process for Hg(II) on A. niger. The nature of the possible cell-metal ion interactions was evaluated by FTIR, SEM, and EDAX analysis. These examinations indicated the involvement of -OH and -NH2+ groups in the biosorption process present on the surface of the dead fungal biomass. Here, Hg(II) ions were deposited on the surface of the biomass as a film like structure.

Keywords: Activated Carbon, Analysis, Aqueous Solution, Aspergillus Niger, Biomass, Biosorbent, Biosorption, Biosorption, Bone Char, Cadmium Ions, Diffusion, Experimental, First, FTIR, Fungal Biomass, Hg(II), Inorganic Mercury, Intra-Particle Diffusion, Investigation, Kinetic, Kinetics, Lead, Marine Fungi, Mercury, Mercury Removal, Methyl Mercury, Model, pH, Pollution, Removal, SEM, Solution, Sorption, Sorption Process, Structure, Temperature, Treatment, Tree Fern, Waste, Wastewater

? Sahu, A.K., Srivastava, V.C., Mall, I.D. and Lataye, D.H. (2008), Adsorption of furfural from aqueous solution onto activated carbon: Kinetic, equilibrium and thermodynamic study. Separation Science and Technology, 43 (5), 1239-1259.

Full Text: 2008\Sep Sci Tec43, 1239.pdf

Abstract: The present study aims to evaluate the influence of various experimental parameters viz. initial pH (pH(0)), adsorbent dose, contact time, initial concentration and temperature on the adsorptive removal of furfural from aqueous solution by commercial grade activated carbon (ACC). Optimum conditions for furfural removal were found to be pH(0) approximate to 5.9, adsorbent dose approximate to 10g/1 of solution and equilibrium time approximate to 6.0h. The adsorption followed pseudo-second-order kinetics. The effective diffusion coefficient of furfural was of the order of 10^-13 m²/s. Furfural adsorption onto ACC was found to be best represented by the Redlich-Peterson isotherm. A decrease in the temperature of the operation favorably influenced the adsorption of furfural onto ACC. The positive values of the change in entropy (Delta S-0), and the negatived value of heat of adsorption (Delta H-0) and change in Gibbs free energy (Delta G(0)) indicated feasible, exothermic, and spontaneous nature of furfural adsorption onto ACC.

Keywords: Activated Carbon, Adsorbent, Adsorbent Dose, Adsorption, Adsorption Kinetics, Adsorption Thermodynamics, Aqueous Solution, Bagasse Fly-Ash, Carbon, Diffusion, Dioxide, Dye, Entropy, Equilibrium, Experimental, Furfural, Furfurals, Heat of Adsorption, Isotherm, Isotherms, Kinetic, Kinetics, pH, Pseudo-Second-Order Kinetics, Removal, Solution, Temperature

? Boddu, V.M., Abburi, K., Randolph, A.J. and Smith, E.D. (2008), Removal of copper(II) and nickel(II) ions from aqueous solutions by a composite chitosan biosorbent. Separation Science and Technology, 43 (6), 1365-1381.

Full Text: 2008\Sep Sci Tec43, 1365.pdf

Abstract: A composite chitosan biosorbent (CCB) was prepared by coating chitosan on to ceramic alumina. The adsorption characteristics of the sorbent for copper and nickel ions were studied under batch equilibrium and dynamic flow conditions at pH 4.0. The equilibrium adsorption data were correlated with Langmuir, Freundlich, and Redlich-Peterson models. The ultimate monolayer capacities, obtained from Langmuir isotherm, were 86.2 and 78.1mg/g of chitosan for Cu(II) and Ni(II), respectively. In addition, dynamic column adsorption studies were conducted to obtain breakthrough curves. After the column was saturated with metal ions, it was regenerated with 0.1M sodium hydroxide. The regenerated column was used for a second adsorption cycle.

Keywords: Adsorption, Chitosan, Copper(II), Nickel(II), Adsorption Isotherms, Metal-Ions, Adsorption Properties, Equilibrium, Resin, Complexation, Kinetics, Sorption, Flakes, Peat

? Nandi, B.K., Goswami, A., Das, A.K., Mondal, B. and Purkait, M.K. (2008), Kinetic and equilibrium studies on the adsorption of crystal violet dye using kaolin as an adsorbent. Separation Science and Technology, 43 (6), 1382-1403.

Full Text: 2008\Sep Sci Tec43, 1382.pdf

Abstract: Experimental investigations are carried out to adsorb toxic crystal violet dye from aqueous medium using kaolin as an adsorbent. Characterization of kaolin is done by measuring i. particle size distribution using particle size analyzer, ii. BET surface area using BET surface analyzer, iii. structural analysis using X ray diffractometer, and iv. microscopic analysis using scanning electron microscope. The effects of initial dye concentration, contact time, kaolin dose, stirring speed, pH, and temperature are studied for the adsorption of crystal violet in batch mode. Adsorption experiments indicate that the extent of adsorption is strongly dependent on the pH of the solution. Free energy of adsorption (G), enthalpy (H), and entropy (S) changes are calculated to know the nature of adsorption. The calculated values of G are -4.11 and -4.48 kJ/mol at 295K and 323 K, respectively, for 20 mg/L of dye concentration, which indicates that the adsorption process is spontaneous. The estimated values of Ho and So show the negative and positive sign, respectively, which indicate that the adsorption process is exothermic and the dye molecules are organized on the kaolin surface in more random fashion than in solution. The adsorption kinetic has been described by pseudo first order, pseudo second order and intra-particle diffusion models. It is observed that the rate of dye adsorption follows pseudo second order model for the dye concentration range studied in the present case. Standard adsorption isotherms are used to fit the experimental equilibrium data. It is found that the adsorption of crystal violet on kaolin follows the Langmuir adsorption isotherm.

Keywords: Adsorbent, Adsorption, Adsorption Isotherm, Adsorption Isotherms, Adsorption Kinetic, Adsorption Process, Analysis, Aqueous Medium, Aqueous-Solutions, Batch, Batch Mode, BET, BET Surface Area, Changes, Characterization, Concentration, Contact, Crystal Violet, Data, Decolorization, Diffusion, Distribution, Dye, Dye Adsorption, Effects, Energy, Enthalpy, Entropy, Equilibrium, Equilibrium Studies, Exothermic, Experimental, Experiments, First, First Order, Fly-Ash, Intra-Particle Diffusion, Intraparticle, Intraparticle Diffusion, Investigations, Isotherm, Isotherms, Kaolin, Kinetic, Langmuir, Langmuir Adsorption Isotherm, Methyl-Violet, Micellar-Enhanced Ultrafiltration, Mode, Model, Models, Particle Size, Particle Size Distribution, pH, Process, Pseudo, Pseudo First Order, Pseudo Second Order, Pseudo-First-Order, Pseudo-Second-Order, Removal, Second Order, Second-Order, Sem, Size, Size Distribution, Solution, Spontaneous, Structural Analysis, Surface, Surface Area, Temperature, Toxic, Values, Waste-Water, X-Ray, Zero Point Charge

? Biswas, B.K., Inoue, K., Ghimire, K.N., Kawakita, H., Ohto, K. and Harada, H. (2008), Effective removal of arsenic with lanthanum(III)- and cerium(III)-loaded orange waste gels. Separation Science and Technology, 43 (8), 2144-2165.

Full Text: 2008\Sep Sci Tec43, 2144.pdf

Abstract: Orange waste has been chemically modified and loaded with lanthanum(III) and/or cerium(III) to examine its adsorption behavior to both As(V) and As(III). Arsenate removal was found to be favored over a pH range of 6 similar to 9.5 while arsenite removal took place at pH values ranging from 9 to 11. The maximum sorption capacity of the gel for As(III) removal was evaluated as 43 mg/g, while that for As(V) was 42 mg/g. Column-mode tests using the La(III)-loaded gel confirmed a complete removal of As(V). A reasonably high adsorption potential within the design criteria makes the present gel an alternative choice for arsenic removal.

Keywords: Adsorption, Arsenic, Ligand Substitution, Orange Waste Gel, Ligand-Exchange Sorption, Ferric Ion Form, Chelating Resin, Aqueous-Solutions, Adsorption, Biosorption, Anions, Water, Adsorbents, Cadmium

? Ashour, I., Al-Rub, F.A.A., Sheikha, D. and Volesky, B. (2008), Biosorption of naphthalene from refinery simulated waste-water on blank alginate beads and immobilized dead algal cells. Separation Science and Technology, 43 (8), 2208-2224.

Full Text: 2008\Sep Sci Tec43, 2208.pdf

Abstract: The potential use of blank alginate beads and immobilized dead algal cells for the removal of naphthalene from aqueous solutions was investigated in this study. The effects of contact time, solution pH, and naphthalene concentration on the sorption of naphthalene on blank alginate beads or immobilized dead algal cells were studied. The effect of the presence of other pollutants on the sorption of naphthalene on immobilized dead algal cells was also studied. Batch adsorption experiments showed that the removal of naphthalene on both sorbents was pH dependent and significant removal of naphthalene was obtained at pH 4. Dynamic sorption experiments revealed that the biosorption of naphthalene on either sorbent was rapid where the equilibrium uptake occurred within 10 minutes, and the biosorption of naphthalene on either sorbent followed the pseudo-second order kinetics. Analysis of the equilibrium sorption data showed that naphthalene sorption on either sorbent could be fitted to the Langmuir, Freundlich, and Dubinin-Radushkevich (D-R) isotherm equations. Competitive biosorption experiments showed that biosorption of naphthalene on immobilized dead algal cells was adversely affected by the presence of either heavy metals such as copper and nickel, and chelating agents such as citric acid.

Keywords: Activated-Sludge, Adsorption, Alginate, Aqueous Solutions, Aqueous-Solutions, Beads, Binary, Biosorption, Citric Acid, Copper, Degradation, Equilibrium, Experiments, Freundlich, Heavy Metals, Immobilized, Immobilized Dead Algal Cells, Isotherm, Isotherm Equations, Isotherms, Kinetics, Langmuir, Metals, Model, Naphthalene, Nickel, pH, Ph-Dependent, Phenol, Pollutants, Potential, Pseudo Second Order, Pseudo Second Order Kinetics, Pseudo-Second Order, Pseudo-Second Order Kinetics, Pseudo-Second-Order, Removal, Single, Solution, Sorbent, Sorbents, Sorption, Waste Water, Wastewater

? Guibal, E., Gavilan, K.C., Bunio, P., Vincent, T. and Trochimczuk, A. (2008), Cyphos IL 101 (tetradecyl(trihexyl)phosphonium chloride) immobilized in biopolymer capsules for Hg(II) recovery from HCl solutions. Separation Science and Technology, 43 (9-10), 2406-2433.

Full Text: 2008\Sep Sci Tec43, 2406.pdf

Abstract: A composite polymer (made of gelatin and alginate) was used for the synthesis of Cyphos IL 101-immobilized resins. These resins (with varying size and different ionic liquid (IL) content) have been tested for the recovery of mercury from concentrated HCl solutions (0.1-5M HCl concentrations). Prior to the study of sorption performance on resins, the reactivity of Cyphos IL 101 versus mercury was tested using solvent extraction methodology. These results showed that the extraction was hardly affected by the concentration of HCl and that an ion exchange mechanism was probably involved in metal recovery (binding of HgCl₄^2-). The performance of these resins for Hg(II) recovery was tested through sorption isotherms and uptake kinetics, investigating the effect of resin size, ionic liquid content, metal concentration, agitation speed, and resin state (dry state versus wet state). Sorption capacity (which was proportional to the IL content) can reached up to 150mg Hg g^-1 in 1M HCl, this sorption capacity was decreased by increasing chloride concentration. The kinetics were described well by the pseudo-second order equation and by the intraparticle diffusion equation (the so-called Crank’s equation). The intraparticle diffusion coefficient was in the range of 10^-11-1.2×10^-10 m²min^-1. The kinetic profiles were controlled by the IL content, sorbent dosage, and the sorbent particle size. Drying of the resins significantly decreased diffusion rates in the resins. The presence of competitor metals did not affect sorption capacity except when stable chloro-anionic species such as in the case of Zn(II) were formed. Mercury can be desorbed using 6M nitric acid solutions, and the sorbent can be recycled for at least six sorption/desorption cycles without significant decrease in the sorption performance.

Keywords: Affect, Agitation, Alginate, Alginate Microcapsules, Aqueous-Solutions, Aryl Halides, Binding, Biopolymer, Capacity, Capsules, Chitosan, Chloride, Composite, Concentration, Cycles, Cyphos IL 101, Desorption, Diffusion, Diffusion Coefficient, Enclosing Cyanex-302 Extractant, Exchange, Extraction, Gelatin, Hg(II), Immobilization, Immobilized, Intraparticle, Intraparticle Diffusion, Ion Exchange, Ion-Exchange, Ionic Liquid, Isotherms, Kinetic, Kinetics, Lactic-Acid, Liquid, Mechanism, Mercury, Metal, Metals, Methodology, Nanofiltration, Palladium, Particle Size, Performance, Phosphonium Ionic Liquids, Polymer, Profiles, Pseudo Second Order, Pseudo-Second Order, Pseudo-Second Order Equation, Pseudo-Second-Order, Rates, Recovery, Resin, Resins, Size, Solutions, Sorbent, Sorbent Dosage, Sorption, Sorption Capacity, Sorption Isotherm, Sorption Isotherms, Sorption, Desorption, Species, State, Synthesis, Ultrafiltration, Uptake, Uptake Kinetics, Zn(II)

? Mištova, E., Parschová, H., Jelínek, L., Matějka, Z., Plichta, Z. and Beneš, M. (2008), Selective sorption of metal oxoanions from dilute solution by chemicaly modified brown seaweed Ascophyllum nodosum. Separation Science and Technology, 43 (11-12), 3168-3182.

Full Text: 2008\Sep Sci Tec43, 3168.pdf

Abstract: Two samples of chemically modified seaweed Ascophyllum nodosum (NS-1 and DS-1) were used for selective removal of metal (W, Mo, V, Ge, and Sb) oxoanions. All experiments were carried out by dynamic column sorption. The effects of pH, the concentration of the accompanying anions in the feed solution, and the effect of the flow rate were studied. Tungstate, molybdate, and vanadate were adsorbed extensively. Sorption of Sb(III) anion was notable but the sorption capacity was very low and the desorption was difficult. Sorption of Ge(IV) oxoanion was negligible. Stability of the NS-1 and DS-1 sorbents was limited by, 20 and 25 sorption cycles, respectively.

Keywords: Biosorption, Metal Oxoanions, Seaweed, Liquid-Liquid-Extraction, Special Chelating Resin, Arsenic Removal, Aqueous-Solutions, Drinking-Water, Ion-Exchange, Waste-Water, Fungal Biomass, Heavy-Metals, Biosorption

? Arslan, C.S. and Dursun, A.Y. (2008), Biosorption of phenol on dried activated sludge: Effect of temperature. Separation Science and Technology, 43 (11-12), 3251-3268.

Full Text: 2008\Sep Sci Tec43, 3251.pdf

Abstract: In this study, the effectiveness of dried activated sludge in removing phenol from aqueous solutions was examined by biosorption as a function of temperature, pH, and initial phenol concentration. Batch kinetic studies showed that an equilibrium time of 60 min was needed for the biosorption. The maximum phenol biosorption capacity was obtained as 42.7 mg g^-1 at the temperature of 40°C at pH = 8.0. The Freundlich and Langmuir adsorption models were used for the mathematical description of the biosorption equilibrium and it was reported that experimental data fitted very well to the Freundlich model. Adsorption rate data were analyzed using the pseudo-first order kinetic model of Lagergren and the pseudo-second order model to determine adsorption rate constants at 10, 25, and 40°C. It was reported that, the pseudo-second order kinetic model provided the best correlation of the experimental data rather than the pseudo-first order model. The thermodynamic parameters such as, Gibbs free energy changes (G°), enthalpy change (H°) and entropy change (S°) were determined. The results show that biosorption of phenol on dried activated sludge is an endothermic and spontaneous in nature.

Keywords: Adsorption, Aqueous-Solutions, Biomass, Biosorption, Carbon, Dried Activated Sludge, Equilibrium, Equilibrium, Kinetic, Phenol, Pseudo-Second Order, Removal, Sorption, Thermodynamic, Water

? Bhattacharyya, K.G. and Sen Gupta, S. (2008), Uptake of Ni(II) ions from aqueous solution by kaolinite and montmorillonite: Influence of acid activation of the clays. Separation Science and Technology, 43 (11-12), 3221-3250.

Full Text: 2008\Sep Sci Tec43, 3221.pdf

Abstract: Kaolinite and montmorillonite were treated with 0.25 M H₂SO₄ and the acid activated clays along with the parent clays were tested for their uptake capacity for Ni(II) ions from aqueous solution. The batch adsorption experiments were conducted under a set of variables (concentration of Ni(II) ion, amount of clay, pH, time and temperature of interaction). Increasing pH favored Ni(II) uptake till the ions were precipitated as the insoluble hydroxides at pH 8.0. The uptake was rapid up to 40 min and equilibrium was obtained within 180 min. The kinetics of the process was evaluated by subjecting the results to a number of models like the pseudo-first order, second order, Elovich equation, liquid film diffusion, and intra-particle diffusion and it was found that the data more closely resembled a second order process. The experimental data conformed to both Langmuir and Freundlich isotherms showing that the interactions were mostly chemical in nature. The clays had reasonable monolayer adsorption capacity of 10.4, 11.9, 28.4, and 29.5 mg g^-1 for kaolinite, acid activated kaolinite, montmorillonite, and acid-activated montmorillonite respectively. Montmorillonite had much better adsorption capacity than kaolinite and the acid activation boosted the adsorption capacity of both kaolinite and montmorillonite. The interactions were exothermic in nature, accompanied by decrease in both entropy and Gibbs energy. The results have established good potentiality for kaolinite, montmorillonite and their acid-activated forms to take up and separate Ni(II) from aqueous medium through adsorption-mediated immobilization.

Keywords: Acid-Activation, Adsorption, Adsorption, Batch, Catalytic-Activity, Copper, Equilibrium, Fly-Ash, Heavy-Metal, Industry Waste, Intraparticle, Kaolinite, Kinetics, Montmorillonite, Red Mud, Removal, Water

? Anirudhan, T.S., Radhakrishnan, P.G. and Suchithra, P.S. (2008), Adsorptive removal of mercury(II) ions from water and wastewater by polymerized tamarind fruit shell. Separation Science and Technology, 43 (13), 3522-3544.

Full Text: 2008\Sep Sci Tec43, 3522.pdf

Abstract: A novel adsorbent, formaldehyde polymerized tamarind fruit shell (FPTFS) containing sulphonic acid functional groups was prepared and its utility for Hg(II) adsorption from water and wastewater was investigated. The kinetic and isotherm data, obtained at optimum pH value 6.0 for different concentrations and temperatures, could be fitted with the Ritchie modified second-order equation and Sips isotherm model respectively and the coefficients indicated favorable adsorption of Hg(II) on the FPTFS. The complete removal of 23.86 mg/L Hg(II) from chlor-alkali industry wastewater was achieved by 4 g/L FPTFS. The reusability of the FPTFS for several cycles was also demonstrated using 0.1M HCl solution.

Keywords: Adsorbent, Adsorption, Aqueous-Solutions, Biomass, Cadmium, Copper Ions, Data, Desorption, Elovich Equation, Formaldehyde, Functional Groups, Heavy-Metal, Hg(II), Isotherm, Isotherm Model, Kinetic, Kinetics, Mercury(II) Adsorption, Model, Modified, Modified Second Order Equation, Pb(II), pH, pH Value, Removal, Sawdust, Second Order, Second-Order, Second-Order Equation, Solution, Sorption, Tamarind Fruit Shell, Thermodynamic Parameters, Utility, Value, Wastewater, Water

? Pokhrel, D. and Viraraghavan, T. (2008), Arsenic removal from aqueous solution by iron oxide-coated biomass: Common ion effects and thermodynamic analysis. Separation Science and Technology, 43 (13), 3545-3562.

Full Text: 2008\Sep Sci Tec43, 3545.pdf

Abstract: A batch study showed that the presence of anions (sulfate, chloride, and nitrate) in solution did not affect the adsorption process of both As(V) and As(III) by iron oxide-coated A. niger biomass. It was found that the presence of Ca²⁺, Fe²⁺, and Mg²⁺ ions at a concentration of 200 mg/L in solution could increase the removal efficiency of As(V) by 86.5%, 95.4%, and 65.8%, respectively. Similarly, the presence of Ca²⁺, Fe²⁺, and Mg²⁺ ions at a concentration of 200 mg/L in solution could increase the removal efficiency of As(III) by 39.3%, 97%, and 8.4%, respectively. The batch adsorption-desorption study showed that the reactions between the arsenic species and the iron oxide-coated A. niger biomass were reversible. Desorption of As(V) and As(III) at neutral pH was approximately 15%. As(V) desorbed more than As(III) in acidic (pH 1.33) and alkaline (pH 12.56) solutions. At a pH of 1.33, 67% of the adsorbed As(V) desorbed, and the percentage of desorbed As(III) was only 47.1% in the same condition. At a solution pH of 12.56, 73.4% of the As(V), and 43.7% of As(III) desorbed. The thermodynamic study showed the spontaneous nature of the sorption of arsenic on IOCB. The high value of the heat of adsorption {H approximate to-133 kJ/mol for As(V), and 88.9 k/mol for As(III)} indicated that the mechanism of arsenic sorption was chemisorption.

Keywords: Adsorption, Purification, Biosorption, Batch Processing, Thermodynamics, Ion Effect, Fungal Biomass, Adsorption, Groundwater, Adsorbent, Column, Waste, Water, Acid

? Sari, A. and Tuzen, M. (2008), Removal of Cr(VI) from aqueous solution by Turkish vermiculite: Equilibrium, thermodynamic and kinetic studies. Separation Science and Technology, 43 (13), 3563-3581.

Full Text: 2008\Sep Sci Tec43, 3563.pdf

Abstract: The adsorption of Cr(VI) from aqueous solution by Turkish vermiculite were investigated in terms of equilibrium, kinetics, and thermodynamics. Experimental parameters affecting the removal process such as pH of solution, adsorbent dosage, contact time, and temperature were studied. Equilibrium adsorption data were evaluated by Langmuir, Freundlich and Dubinin-Radushkevich (D-R) isotherm models. Langmuir model fitted the equilibrium data better than the Freundlich model. The monolayer adsorption capacity of Turkish vermiculite for Cr(VI) was found to be 87.7mg/g at pH 1.5, 10 g/L adsorbent dosage and 20°C. The mean free energy of adsorption (5.9 kJ/mol) obtained from the D-R isotherm indicated that the type of sorption was essentially physical. The calculated thermodynamic parameters (G, H and S) showed that the removal of Cr(VI) ions from aqueous solution by the vermiculite was feasible, spontaneous and exothermic at 20-50C. Equilibrium data were also tested using the adsorption kinetic models and the results showed that the adsorption processes of Cr(VI) onto Turkish vermiculite followed well pseudo-second order kinetics.

Keywords: Adsorbent, Adsorption, Adsorption, Adsorption Capacity, Adsorption Kinetic, Aqueous Solution, Biomass, Capacity, Chromium(VI) Biosorption, Cr(VI), Cu(II), D-R Isotherm, Data, Energy, Equilibrium, Exothermic, Freundlich, Freundlich Model, Hazelnut Shell, Heavy-Metals, Ion-Exchange-Resins, Isotherm, Kinetic, Kinetic Models, Kinetics, Langmuir, Langmuir Model, Model, Models, Monolayer, Pb(II), pH, Physical, Pseudo Second Order, Pseudo Second Order Kinetics, Pseudo-Second Order, Pseudo-Second Order Kinetics, Pseudo-Second-Order, Removal, Saccharomyces-Cerevisiae, Solution, Sorption, Temperature, Thermodynamic, Thermodynamic Parameters, Thermodynamics, Turkish Vermiculite, Vermiculite

? Sathish, R.S., Sairam, S., Raja, V.G., Rao, G.N. and Janardhana, C. (2008), Defluoridation of water using zirconium impregnated coconut fiber carbon. Separation Science and Technology,