Ni<sup>2+</sup> removal from aqueous solutions using conditioned clinoptilolites: Kinetic and isotherm studies

Çoruh, Semra; Ergun, Osman Nuri

doi:10.1002/ep.10316

Cited by 45 publications

(22 citation statements)

References 32 publications

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“…[3][4][5][6][7] The history of ion exchange on zeolites has been reported by several authors. 3,[8][9][10] One of the important properties of zeolites is that they show selectivity in adsorption, i.e. they possess different affinities for different ions.…”

Section: Introductionmentioning

confidence: 99%

Equilibrium ion exchange studies of Ni2+ on homoionic forms of clinoptilolite

et al. 2014

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Research ArticleHomoionic forms of clinoptilolite forms, respectively. The positive changes in enthalpy provide an indication that the sorption reaction is endothermic for Ni(II). The Gibbs free energy values were all negative except for Ca 2+ -exchanged clinoptilolite at 298.15 K and 308.15 K, for which the values were positive 3.10 kJ/mol and 0.53 kJ/mol, respectively. The entropy values for Ni 2+ sorption were also positive; values of 0.12 kJ/mol.K, 0.08 kJ/mol.K and 0.14 kJ/mol.K were obtained for the Na + , K + and Ca 2+ forms, respectively. As expected, the enthalpy obtained from the Van't Hoff plot is dependent not only on the metal ion being adsorbed, but also on the ion being displaced. Pretreatment of the zeolite enhances the removal efficiency provided that monovalent ions are used for the pretreatment. Thus clinoptilolite is an effective low-cost absorbent for the removal of Ni 2+ from aqueous solutions.

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Section: Introductionmentioning

confidence: 99%

Equilibrium ion exchange studies of Ni2+ on homoionic forms of clinoptilolite

et al. 2014

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“…It has been common practice in the published literature concerning sorption equilibrium studies to linearize isotherm models such as those by Langmuir, Freundlich and Temkin [56]. This latter procedure was not driven by experimental accuracy concerns but more for simplicity of analysis.…”

Section: Non-linear Least Squares (Nlls) Analysis Of Equilibrium Datamentioning

confidence: 98%

Equilibrium and column studies of iron exchange with strong acid cation resin

Millar

Schot

Couperthwaite

et al. 2015

Journal of Environmental Chemical Engineering

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A B S T R A C TThe exchange of iron species from iron(III) chloride solutions with a strong acid cation resin has been investigated in relation to a variety of water and wastewater applications. A detailed equilibrium isotherm analysis was conducted wherein models such as Langmuir-Vageler, Competitive Langmuir, Freundlich, Temkin, Dubinin-Astakhov, Sips and Brouers-Sotolongo were applied to the experimental data. An important conclusion was that both the bottle-point method chosen and solution normality used to generate the ion exchange equilibrium isotherm influenced which sorption model fitted the isotherm profiles optimally. Invariably, the calculated value for the maximum loading of iron on strong acid cation resin was substantially higher than the value of 47.1 g/kg of resin which would occur if one Fe 3 + ion exchanged for three "H + " sites on the resin surface. Consequently, it was suggested that above pH 1, various iron complexes sorbed to the resin in a manner which required less than 3 sites per iron moiety. Column trials suggested that the iron loading was 86.6 g/kg of resin when 1342 mg/L Fe(III) ions in water were flowed at 31.7 BV/h. Regeneration with 5-10% HCl solutions reclaimed approximately 90% of exchange sites.2014 Elsevier Ltd. All rights reserved. IntroductionMetal pollution of our water resources remains a major concern [1-3]. Several methods have been employed to remediate contaminated solutions including precipitation [4], coagulationflocculation [5], adsorption [6-8], ion exchange [9,10], membrane filtration [11], flotation [12,13] and electrochemical means [14]. Physico-chemical techniques are attractive due to a variety of reasons such as process economics, reliability and ease of use [15]. Ion exchange is of particular interest as not only can the metals potentially be recovered but also the technology is well developed, simple and effective [16]. Iron is a common contaminant in natural waters [17], mining effluents [18], hydrometallurgical solutions [19] and a range of other industrial wastes [20]. Demineralization of water and wastewater solutions is widely practiced in industry, usually with a combination of cation and anion resins to remove the dissolved ions [21]. Kaya et al. [22] have shown that the presence of iron even at low concentration can significantly reduce the operating capacity of synthetic strong acid cation resins. Victor-Ortega Abbreviations: A, Temkin isotherm parameter (L/mmol or L/mg); a s , Sips equilibrium isotherm coefficient; a, exponent which represents the inherent energy heterogeneity of the sorbent surface; AIC, Akaike information criterion; ARE, average relative error; b T , Temkin constant related to the heat of adsorption (J/mol); BV, bed volumes; C e , equilibrium concentration of iron ions in solution (mg/L); C o , initial concentration of iron ions in solution (mg/L); e, adsorption potential (J/mol); E, energy of adsorption (J/mol); eq, equivalents; EABS, sum of the absolute errors; HYBRID, hybrid fractional error function; K CL , Competitive Lan...

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“…The mineral mass in solution affects adsorption process, as it monitors accessibility of active sites. Numerous studies reported that higher mineral concentrations resulted in increased metal removal (Coruh and Ergun, 2009;Mishra and Patel, 2009) and reduced amount of ions adsorbed on adsorbent surface (Oren and Kaya, 2006). Decrease in adsorption capacity could be explained as aresult of unsaturated adsorption sites as well as particle aggregation resulted in decreasing total surface area while increasing diffusion path length.…”

Section: Effect Of Bentonite Dosementioning

confidence: 99%

Surface modified bentonite mineral as a sorbent for Pb2+ and Zn2+ ions removal from aqueous solutions

Hassan¹,

Selim²,

Rostom³

et al. 2020

Physicochem. Probl. Miner. Process.

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Environmental pollution by lead (Pb 2+) and zinc (Zn 2+) ions has become an important issue due to its harmful effects on human health and environment. This work aims to evaluate the application of surface modified Egyptian bentonite mineral by acid activation using H2SO4 and thermal treatment as an adsorbent to remove lead (Pb 2+) and zinc (Zn 2+) ions from aqueous solution. X-ray diffraction (XRD), Fourier Transformed Infrared Spectroscopy (FTIR) and Scanning Electron Microscope (SEM) techniques were used to investigate the modified bentonite. The impact of organic and inorganic dispersants on rheological characteristics of bentonite suspensions was investigated. Adsorption of Pb 2+ and Zn 2+ ions using modified bentonite mineral was performed with different adsorbent doses and pH values. Removal efficiencies of lead and zinc are 99.67% and 99%, respectively with adsorbent dose of 25 g/l at pH of 6.2.

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Ni²⁺ removal from aqueous solutions using conditioned clinoptilolites: Kinetic and isotherm studies

Cited by 45 publications

References 32 publications

Equilibrium ion exchange studies of Ni2+ on homoionic forms of clinoptilolite

Equilibrium ion exchange studies of Ni2+ on homoionic forms of clinoptilolite

Equilibrium and column studies of iron exchange with strong acid cation resin

Surface modified bentonite mineral as a sorbent for Pb2+ and Zn2+ ions removal from aqueous solutions

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Ni2+ removal from aqueous solutions using conditioned clinoptilolites: Kinetic and isotherm studies

Cited by 45 publications

References 32 publications

Equilibrium ion exchange studies of Ni2+ on homoionic forms of clinoptilolite

Equilibrium ion exchange studies of Ni2+ on homoionic forms of clinoptilolite

Equilibrium and column studies of iron exchange with strong acid cation resin

Surface modified bentonite mineral as a sorbent for Pb2+ and Zn2+ ions removal from aqueous solutions

Contact Info

Product

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Ni²⁺ removal from aqueous solutions using conditioned clinoptilolites: Kinetic and isotherm studies