Sorption of strontium on bentonite

Khan, Saad Ahmad; Riaz-ur-Rehman,; Khan, Muhammad Ali

doi:10.1016/0956-053x(96)00049-9

Cited by 85 publications

(33 citation statements)

References 21 publications

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“…Various studies have been carried out to examine different aspects of the sorption behavior of Sr on a variety of solid materials [2][3][4][5][6][7][8][9][10][11][12][13]. Whereas the sorption behavior of Sr 2+ on kaolinite was investigated in a limited number of studies [14][15][16][17], our literature survey did not yield information *Author for correspondence (E-mail: talalshahwan@iyte.edu.tr).…”

Section: Introductionmentioning

confidence: 61%

Characterization of Sr²⁺uptake on natural minerals of kaolinite and magnesite using XRPD, SEM/EDS, XPS, and DRIFT

Shahwan¹,

Erten²

2005

Radiochimica Acta

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Sr2+ / Kaolinite / Magnesite Summary. The sorption behavior of Sr 2+ ions on natural minerals rich in kaolinite and magnesite was studied using SEM/EDS, XPS, XRPD, AAS/AES and DRIFT techniques. Quantitative analysis of the XPS data shows that magnesite is more effective in Sr 2+ uptake than kaolinite. DRIFT spectra and XRPD patterns indicate that the structures of both minerals were not affected upon Sr 2+ sorption. Intercalation of DMSO in kaolinite lamellae aiming at increasing the interlayer space did not significantly enhance the sorption capacity of the clay towards Sr 2+ probably due to the lack of a negative charge on the accessible sites. EDS mapping indicated that while the sorbed Sr is equally distributed on surface of natural kaolinite, it was associated -to a larger extent -with the regions richer in Mg in the case of natural magnesite. Comparing the uptake mechanisms of natural magnesite with that of pure MgCO 3 , it was seen that while natural magnesite sorbed Sr 2+ mainly through an ion exchange type mechanism, the formation of SrCO 3 coprecipitate was detected on the surface of the MgCO 3 at higher loadings.

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Section: Introductionmentioning

confidence: 61%

Characterization of Sr²⁺uptake on natural minerals of kaolinite and magnesite using XRPD, SEM/EDS, XPS, and DRIFT

Shahwan¹,

Erten²

2005

Radiochimica Acta

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“…Bentonite as an adsorbent for the removal of malathion (Pradas et al 1993), Sr(II) (Khan et al 1995a), UO 2+ 2 ion (Olguin et al 1997), and Cd(II) and Pb(II) under estuarine and seawater conditions (Kozar et al 1992), Cu(II) (Rauf et al 1999), Cr(III) (Ikram et al 2002), Pb(II) (Naseem and Tahir 2001), Pb(II) and Ni(II) (Lee et al 2000), Zn(II) (Mellah and Chegrouche 1997), and Pb(II), Cu(II), and Zn(II) (Bereket et al 1997) from aqueous solutions has already been reported in the literature.…”

Section: Introductionmentioning

confidence: 99%

Removal of Cu(II), Zn(II) and Co(II) ions from aqueous solutions by adsorption onto natural bentonite

et al. 2007

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In this study, the removal of Cu(II), Zn(II) and Co(II) ions from aqueous solutions using the adsorption process onto natural bentonite has been investigated as a function of initial metal concentration, pH and temperature. In order to find out the effect of temperature on adsorption, the experiments were conducted at 20, 50, 75 and 90°C. For all the metal cations studied, the maximum adsorption was observed at 20°C. The batch method has been employed using initial metal concentrations in solution ranging from 15 to 70 mg L −1 at pH 3.0, 5.0, 7.0 and 9.0. A flame atomic absorption spectrometer was used for measuring the heavy metal concentrations before and after adsorption. The percentage adsorption and distribution coefficients (K d ) were determined for the adsorption system as a function of adsorbate concentration. In the ion exchange evaluation part of the study, it is determined that in every concentration range, adsorption ratios of bentonitic clay-heavy metal cations match to Langmuir, Freundlich and DubininKaganer-Radushkevich (DKR) adsorption isotherm data, adding to that every cation exchange capacity of metals has been calculated. It is shown that the bentonite is sensitive to pH changes, so that the amounts of heavy metal cations adsorbed increase as pH increase in adsorbent-adsorbate system. It is evident that the adsorption phenomena depend on the surface charge density of adsorbent and hydrated ion diameter depending upon the solution pH. According to thȩ adsorption equilibrium studies, the selectivity order can be given as Zn 2+ > Cu 2+ > Co 2+ . These results show that bentonitic clay hold great potential to remove the relevant heavy metal cations from industrial wastewater. Also, from the results of the thermodynamic analysis, standard free energy G 0 , standard enthalpy H 0 and standard entropy S 0 of the adsorption process were calculated.

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“…Uses of bentonite for adsorptive removal of Zn(II) (Mellah and Chegrouche, 1997) and Sr(II) (Khan et al, 1995), natural and Na-exchanged-bentonite for removal of Cr(III), Ni(II), Zn(II), Cu(II) and Cd(II) from water (Alvarez-Ayuso and Garcia-Sanchez, 2003), sepiolite for Co(II) (Kara et al, 2003), and even kaolinite for Mn(II), Co(II), Ni(II), Cu(II) (Yuvaz et al, 2003) have yielded significant adsorption. Other important results include adsorption of Cu(II) and Zn(II) on surfactantmodified montmorillonite (Lin and Juang, 2002), and of Cu(II) on 1:10-phenanthroline grafted Brazilian bentonite (De Leon et al, 2003).…”

Section: Introductionmentioning

confidence: 99%

Adsorption of Fe(III) from water by natural and acid activated clays: Studies on equilibrium isotherm, kinetics and thermodynamics of interactions

Bhattacharyya

Gupta²

2006

Adsorption

111

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The present work investigates the removal of Fe(III) ions from an aqueous solution by kaolinite, montmorillonite and their acid activated forms. The specific surface areas of kaolinite, acid activated kaolinite, montmorillonite and acid activated montmorillonite were 3.8, 15.6, 19.8 and 52.3 m 2 /g respectively whereas the cation exchange capacity (CEC) was measured as 11.3, 12.2, 153.0, and 341.0 meq/100 g for four clay adsorbents respectively. Adsorption increased with pH till Fe(III) became insoluble at pH > 4.0. The kinetics of the interactions is not certain, but the second order kinetics (k 2 = 4.7 × 10 −2 to 7.4 × 10 −2 g mg −1 min −1 ) appears to give a better description. Langmuir and Freundlich isotherms were applied and isotherm coefficients were computed. The Langmuir monolayer capacity of the clay adsorbents was from 11.2 to 30.0 mg g −1 . The process was exothermic with H in the range of −27.6 to −42.2 kJ mol −1 accompanied by decrease in entropy ( S = −86.6 to −131.8 J mol −1 K −1 ) and decrease in Gibbs energy. The results have shown that kaolinite, montmorillonite and their acid activated forms could be used as adsorbents for separation of Fe(III) from aqueous solution. Acid activation enhanced the adsorption capacity compared to the untreated clay minerals.

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Sorption of strontium on bentonite

Cited by 85 publications

References 21 publications

Characterization of Sr²⁺uptake on natural minerals of kaolinite and magnesite using XRPD, SEM/EDS, XPS, and DRIFT

Characterization of Sr²⁺uptake on natural minerals of kaolinite and magnesite using XRPD, SEM/EDS, XPS, and DRIFT

Removal of Cu(II), Zn(II) and Co(II) ions from aqueous solutions by adsorption onto natural bentonite

Adsorption of Fe(III) from water by natural and acid activated clays: Studies on equilibrium isotherm, kinetics and thermodynamics of interactions

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Sorption of strontium on bentonite

Cited by 85 publications

References 21 publications

Characterization of Sr2+uptake on natural minerals of kaolinite and magnesite using XRPD, SEM/EDS, XPS, and DRIFT

Characterization of Sr2+uptake on natural minerals of kaolinite and magnesite using XRPD, SEM/EDS, XPS, and DRIFT

Removal of Cu(II), Zn(II) and Co(II) ions from aqueous solutions by adsorption onto natural bentonite

Adsorption of Fe(III) from water by natural and acid activated clays: Studies on equilibrium isotherm, kinetics and thermodynamics of interactions

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Characterization of Sr²⁺uptake on natural minerals of kaolinite and magnesite using XRPD, SEM/EDS, XPS, and DRIFT

Characterization of Sr²⁺uptake on natural minerals of kaolinite and magnesite using XRPD, SEM/EDS, XPS, and DRIFT