Adsorption of cobalt by activated carbon from the rice hulls

Teker, Murat; Saltabaş, Ömer; İmamoğlu, Mustafa

doi:10.1080/10934529709376668

Cited by 43 publications

(42 citation statements)

References 8 publications

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“…A number of works have been carried out using activated carbon from hazelnut husk (Imamoglu and Tekir 2008), rice hulls (Teker et al 1999), apricot stones, coconut shells (Budinova et al 1994) and peanut hulls (Periasamy and Namasivayam 1994) for heavy metals removal. However, no attempt has been made to produce activated carbon using Ipomoea carnea plants for the removal of Cu(II) ions.…”

Section: Introductionmentioning

confidence: 99%

Chemically activated Ipomoea carnea as an adsorbent for the copper sorption from synthetic solutions

et al. 2010

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An indigenously prepared zinc chloride activated Ipomoea carnea (morning glory), a low-cost and abundant adsorbent, was used for removal of Cu(II) ions from aqueous solutions in a batch adsorption system. The chemical activating agent ZnCl 2 was dissolved in deionised water and then added to the adsorbent in two different ratios 1:1 and 1:0.5 adsorbent to activating agent ratio by weight. Studies were conducted as a function of contact time, initial metal concentration, dose of adsorbent, and pH. Activated Ipomoea carnea (AIC) were characterised using scanning electron microscopy (SEM), iodine number and methylene blue number. High iodine numbers indicates development of micro pores with zinc chloride activation. Maximum adsorption was noted within pH range 6.0(±0.05). Adsorption process is fast initially and reaches equilibrium after about 4 hours. The kinetic data were analysed using pseudo-first-order and pseudo-second-order models. The pseudo-second-order kinetic model was found to agree well with the experimental data. Adsorption equilibrium data were analyzed using Langmuir and Freundlich isotherm models. The Langmuir model represented the sorption process better than the Freundlich model. Based on the Langmuir isotherm, the monolayer adsorption capacity of Cu(II) ions was 7.855 mg g −1 for AIC (1:1) and 6.934 mg g −1 for AIC (1:0.5). Nomenclature aRadius of spherical adsorbent particles (m) C 0 Concentration of Cu 2+ before adsorption (mg/l) C e Equilibrium concentration of Cu 2+ in solution (mg/l) C r Concentration of Cu 2+ after adsorption (mg/l) D eff Effective diffusion coefficient (m 2 /s) D 2 Particle diffusion coefficient (m 2 /s) F Fractional attainment of equilibrium at time t K Freundlich constant representing multilayer adsorption capacity (mg/g) K f Pseudo first-order rate constant (min −1 ) K id Initial rate of intraparticle diffusion (mg/(g min 0.5 )) K L Langmuir constant representing adsorption intensity (l/mg) K s Pseudo second-order rate constant (g/mg min) M Mass of the adsorbent (g) n Freundlich constant representing adsorption intensity (g/l) q e Adsorption capacity at equilibrium (mg/g) q tAdsorption capacity at any time t (mg/g) Q 0 Langmuir constant representing maximum monolayer adsorption capacity (mg/g) 76 Adsorption (2010) 16: 75-84 R 2 Regression coefficient t Contact time (min) V Volume of adsorbate solution (l)

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Section: Introductionmentioning

confidence: 99%

Chemically activated Ipomoea carnea as an adsorbent for the copper sorption from synthetic solutions

et al. 2010

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“…Estimating the optimum pH for metal removal is vital since the pH of a solution affects the surface charge of the adsorbents, degree of ionization, and solution composition (metal speciation). Moreover, the level of dissociation of functional groups on the adsorbent surface, solubility of metal ions, and concentration of the counter ions in solution are affected by pH [38][39][40]. The decrease in uptake at higher and lower pH may be attributed to the formation of precipitates of the metal hydroxides at higher pH and formation of more H + ions at lower pH, which might compete with the metal ions for active sites on the adsorbent surface.…”

Section: Effect Of Ph On the Sorption Performance Of The Adsorbentsmentioning

confidence: 99%

Kinetics and equilibrium modeling of lead(II) and chromium(III) ions'' adsorption onto clay from Kono-bowe, Nigeria

Ajemba¹

2014

Turkish J Eng Env Sci

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Abstract:Clay from Kono-bowe, Nigeria, was activated thermally and chemically and used to remove lead(II) and chromium(III) ions from aqueous solution. The effects of adsorption process variables were studied as well as the kinetics and equilibrium of the process. Analysis of the activated samples showed that the surface area, cation exchange capacity, and adsorption performance were positively favored by both activation processes. It was observed that the adsorption rate increased with an increase in temperature, contact time, adsorbent dosage, initial ion concentration, and solution pH values. The pH P ZC of the adsorbents was determined to be 6.5, 7.4, and 7.2, for KBR, KBTA, and KBAA, respectively.It was observed that sample KBAA yielded maximum adsorption efficiency of 99.9% for the removal of chromium(III), and gave maximum adsorption efficiency of 98.7% for lead(II) removal. The results of the kinetics analysis of the adsorption data revealed that adsorption follows pseudo-second-order kinetics. Analysis of the equilibrium data showed that the Langmuir isotherm provided a better fit to the experimental data for KBR, while the Freundlich isotherm fitted the experimental data of KBTA and KBAA. Evaluation of the thermodynamic parameters revealed that the adsorption process is spontaneous and endothermic.

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“…Cu, Zn, Hg and Cd are harmful waste introduced by industries that pose a risk of contamination groundwater and other water resources (Achour and Youcef, 2003). Heavy metals are not biodegradable and tend to accumulate in living organisms, causing various diseases and disorders (Teker and Imamoglu, 2005). As far as cadmium is concerned, it causes serious renal damage anemia and hypertention (Mahvi et al, 2007).…”

Section: Introductionmentioning

confidence: 99%

Adsorption of cadmium(II) ions from aqueous solution onto kaolinite and metakaolinite

Essomba¹,

Nsami²,

Belibi³

et al. 2014

pacs

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The removal of cadmium(II) ions from aqueous solution by adsorption on kaolinite (KAO.1) and metakaolinite (MKB) was investigated depending on the initial concentration, adsorbents dosage, initial pH of solution, and contact time. The influences of those factors have been experimentally verified by a batch method at (27±3 °C). These results have showed that the amount of cadmium(II) ions adsorbed increases with increased contact time and that equilibrium adsorption is reached in 10 minutes, the optimum value of pH was 8.0 and the effect of absorbent dose for the uptake of cadmium(II) ions by kaolinite and metakaolinite was found to decrease by increasing the adsorbent dose. The experimental results obtained are described by Langmuir, Freundlich and Dubinin-Kaganer-Radushkevich (D-K-R) isotherm models. The Langmuir and D-K-R adsorption isotherms described the adsorption data very well. The maximum adsorption capacity; Q max , determined from the Langmuir adsorption isotherm studies was found to be 7.407 and 9.174 mg/g for KAO.1 and MKB respectively. Pseudo-first order, pseudo-second order, Elovich and the intraparticular diffusion kinetic models were used to describe the kinetic data obtained. The experimental data fitted well to the pseudo-second order kinetic model, which indicates that 12Jean Serge ESSOMBA et al.chemical adsorption is the rate-limiting step. The results indicate that kaolinite and metakaolinite adsorb cadmium(II) ions efficiently and could be employed as a low-cost alternative in waste water treatment for the elimination of cadmium(II) ions.

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Adsorption of cobalt by activated carbon from the rice hulls

Cited by 43 publications

References 8 publications

Chemically activated Ipomoea carnea as an adsorbent for the copper sorption from synthetic solutions

Chemically activated Ipomoea carnea as an adsorbent for the copper sorption from synthetic solutions

Kinetics and equilibrium modeling of lead(II) and chromium(III) ions'' adsorption onto clay from Kono-bowe, Nigeria

Adsorption of cadmium(II) ions from aqueous solution onto kaolinite and metakaolinite

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