Nickel(II) and zinc(II) removal using Amberlite IR-120 resin: Ion exchange equilibrium and kinetics

Franco, Pietro Escobar; Veit, Márcia Teresinha; Borba, Carlos Eduardo; Gonçalves, Gilberto da Cunha; Fagundes‐Klen, Márcia Regina; Bergamasco, Rosângela; Silva, Edson Antônio da; Suzaki, Pedro Yahico Ramos

doi:10.1016/j.cej.2013.02.006

Cited by 61 publications

(19 citation statements)

References 27 publications

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“…In the first variant, the solution concentration is kept at a constant value and the resin mass varied [30][31][32]. The second version employs a constant resin mass and a range of solutions of varying metal ion concentration [33,34].…”

Section: Equilibrium Studiesmentioning

confidence: 99%

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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Section: Equilibrium Studiesmentioning

confidence: 99%

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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“…Ni(II) species present in the forms of Ni 21 , Ni(OH) 1 , Ni(OH) 2 , and Ni(OH) 3 from low to high pH values. At pH 2.0-8.0, the predominant Ni(II) species is Ni 21 , at pH > 8.2, the predominant Ni(II) species are Ni(OH) 1 , Ni(OH) 2 , and Ni(OH) 3 - [43]. According to the results obtained, it could be deduced that there would be electrostatic attraction between Ni(II) and laponite particles in the pH range of 2.0-8.0.…”

Section: Effect Of Solution Phmentioning

confidence: 99%

“…The adsorption of Ni(II) from aqueous solution on laponite as a function of contact time, pH, ionic strength, laponite dosage, and temperature was studied via batch technique. Different methods, such as chemical precipitation [2], ion exchange [3], membrane separation [4], electrocoagulation [5,6] have been used to remove heavy metal ions from aqueous solutions. Adsorption of Ni(II) on laponite is strongly dependent on pH but independent on ionic strength.…”

mentioning

confidence: 99%

“…Therefore, decreasing Ni(II) concentration before discharge to the environment is important to protect environmental and human health. Different methods, such as chemical precipitation [2], ion exchange [3], membrane separation [4], electrocoagulation [5,6] have been used to remove heavy metal ions from aqueous solutions. However, most of these techniques have some disadvantages such as complicated treatment process, high cost, and energy use.…”

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confidence: 99%

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Use of laponite as adsorbents for Ni(II) removal from aqueous solution

Cao

Yan

Huang

et al. 2017

Env Prog and Sustain Energy

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Silicate‐bearing hectorites (laponite) were synthesized by hydrothermal method, and the laponite sample was characterized by Fourier transform infrared (FTIR) spectroscopy, X‐ray diffraction (XRD), zeta potential, Brunauer‐Emmett‐Teller (BET) surface area, and pore size analyses. The adsorption of Ni(II) from aqueous solution on laponite as a function of contact time, pH, ionic strength, laponite dosage, and temperature was studied via batch technique. The maximum removal of 99% (approx) could be achieved at the optimum adsorbent dosage of 2.5 g L−1 and near‐neutral pH. Adsorption of Ni(II) on laponite is strongly dependent on pH but independent on ionic strength. At low pH, the adsorption of Ni(II) was dominated by ion exchange with Li+ on laponite surfaces, whereas inner‐sphere surface complexation and surface precipitation were the main adsorption mechanisms at near‐neutral pH and alkaline environment, respectively. The adsorption kinetic data of Ni(II) on laponite were well described by the pseudo‐second‐order kinetics model. The intraparticle diffusion was involved in the adsorption process but was not the only rate‐controlling step. The adsorption isotherms of Ni(II) on laponite can be described well by the Langmuir model and the maximum Ni(II) adsorption capacity of laponite obtained from Langmuir model was 65.79 mg g−1. The thermodynamic studies indicated that the adsorption of Ni(II) on laponite was endothermic and spontaneous. The laponite exhibited excellent adsorption properties for Ni(II) uptake compared with various adsorbents, indicating that it is a suitable material as an adsorbent for preconcentration and immobilization of Ni(II) from aqueous solution. © 2017 American Institute of Chemical Engineers Environ Prog, 37: 942–950, 2018

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“…Recently, one of the major challenges in developing countries is the removal of toxic metals from water. The methods such as chemical precipitation [17,19], solvent extraction [2], ion exchange [8], reverse osmosis and adsorption [18] have been adopted to remove the heavy metal ions from water. Among these techniques adsorption with suitable adsorbent is the mostly used method.…”

Section: Introductionmentioning

confidence: 99%

Facile Synthesis of Magnetic Activated Carbon Composite for Arsenic Adsorption

Karki

Pandey

Rajbhandari

et al. 2019

J. Inst. Engineering

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Porous activated carbon (AC) and magnetic iron oxide nanoparticles (NPs) are widely used for the removal of arsenic from water body. Fabrication of composite material of iron oxide NPs on the surface of porous AC can further enhance this activity for commercial application. In this research, a magnetic AC composite for arsenic adsorption was prepared by facile hydrothermal treatment of aqueous solution containing activated carbon obtained from lapsi seed stone, iron(II) chloride, polyvinylpyrrolidone (PVP) and ethanol. Several analytical techniques such as scanning electron microscopy (SEM), energy dispersive x-ray (EDX), X-ray diffraction (XRD) and Fourier-transform infrared spectroscopy (FTIR) confirmed the formation of magnetite (Fe3O4) nanoparticles on the surface of porous AC. The prepared materials were accessed for their arsenic adsorption capacity using arsenic (III) trioxide solution and found that composite Fe2O3/AC can remove the arsenic from water far more effectively than activated carbon alone. For 0.5 g/ltr loading of composite sample with contract time of 5 hours, the arsenic content was significantly reduced, which shows that as-fabricated composite can be used potentially for water treatment.

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Nickel(II) and zinc(II) removal using Amberlite IR-120 resin: Ion exchange equilibrium and kinetics

Cited by 61 publications

References 27 publications

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

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

Use of laponite as adsorbents for Ni(II) removal from aqueous solution

Facile Synthesis of Magnetic Activated Carbon Composite for Arsenic Adsorption

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