The effect of some operating variables on the adsorption of lead and cadmium ions on kaolinite clay

Adebowale, Kayode O.; Unuabonah, Emmanuel I.; Olu-Owolabi, Bamidele I.

doi:10.1016/j.jhazmat.2005.10.056

Cited by 214 publications

(134 citation statements)

References 54 publications

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“…This indicates an interaction between the metal ions and the modified material (Olu-Owolabi et al 2010). With modification of the kaolinite clay with a binary of goethite and humic acid, cation exchange capacity of the clay increase from 7.81 meq/100 g to 40 meq/100 g while the specific surface area (13 m 2 /g) was the same as that reported by Adebowale et al (2006). This increase in CEC might be as result of the humic acid portion of the mixture which have been shown by Saito et al (2004) to mask the charges of geothite and increase overall negative charges on the surface of a geothite-humic acid mixture.…”

Section: Resultssupporting

confidence: 78%

“…The band assignments of the infrared spectrum of 5 % GHAmodified kaolinite clay adsorbent are shown in Table 1. The adsorption band at 3700, 3619 and 3394 cm -1 for unmodified clay shows the presence of inner surface -OH stretching vibrations from the octahedral surface of the clay layers, while those at 1026, 914 and 772 cm -1 represent the Si-O, Al-OH bending vibrations and Si-O stretching, respectively (Adebowale et al 2006;Jiang et al 2009). The adsorption bands at 1615 cm -1 represent -OH bending vibration of water molecule (Jiang et al 2009).…”

Section: Resultsmentioning

confidence: 98%

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Competitive adsorption of metal ions onto goethite–humic acid-modified kaolinite clay

Unuabonah

Olu-Owolabi

Adebowale

2016

Int. J. Environ. Sci. Technol.

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A binary mixture of humic acid and geothite was prepared and used to modify kaolinite to produce geothite-humic acid (GHA)-modified kaolinite adsorbent useful for the adsorption of Pb 2? , Cd 2? , Zn 2? , Ni 2? and Cu 2? from Single and Quinary (5) metal ion systems. The cation exchange capacity (CEC) and specific surface area of GHA-modified kaolinite clay adsorbent were found to be 40 meq/100 g and 13 m 2 /g, respectively, with the CEC being five times that of raw kaolinite clay (7.81 meq/ 100 g). The Langmuir-Freundlich equilibrium isotherm model gave better fit to experimental data as compared with other isotherm models. In Quinary metal ion system, the presence of Zn . The GHA-modified kaolinite showed strong preference for the adsorption of Pb 2? in both metal ion systems. BrouersWeron-Sotolongo (BWS) kinetic model gave better fit to kinetic data compared with other kinetic models used. Data from BWS kinetic model indicate that adsorption of metal ions onto GHA-modified adsorbent in both metal ion systems followed strictly, diffusion-controlled mechanism with adsorption reaction proceeding to 50 % equilibrium in\2 min in the Single metal ion system and\1 min in the Quinary metal ion system. Adsorption of metal ions onto GHA-modified kaolinite is fairly spontaneous and endothermic in nature in both metal ion systems although the rate of metal ion uptake and spontaneity of reaction are reduced in the Quinary metal ion system.

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Section: Resultssupporting

confidence: 78%

Section: Resultsmentioning

confidence: 98%

Competitive adsorption of metal ions onto goethite–humic acid-modified kaolinite clay

Unuabonah

Olu-Owolabi

Adebowale

2016

Int. J. Environ. Sci. Technol.

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“…The application of cationic surfactants increases both the anionic adsorptive capacity and the cation affinity of clays, although the modification is limited to their external surfaces [76,79,80]. Surfactant-modified clays can be applied for the removal of heavy metal from water through ion exchange, precipitation-dissolution, and counter-ion binding mechanisms [8,81].…”

Section: Claysmentioning

confidence: 99%

Use of Surfactant-Modified Zeolites and Clays for the Removal of Heavy Metals from Water

Jiménez-Castañeda

Medina

2017

Water

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Abstract:The presence of heavy metals in water for human use or consumption represents a major risk to human health. It is therefore important to find materials to remove or minimise the concentration of these pollutants. The adsorption process for the removal of heavy metals is favoured by the use of low-cost materials that exhibit a porous structure and a high cation exchange capacity, such as zeolites and clays. On the other hand, chemical treatments, e.g., using acids and bases, can modify the properties of these materials, but more recently the application of surfactants has also shown to be successful for broadening their metal affinity and allowing the removal of diverse organic and inorganic pollutants from water. This paper reviews the application of modified zeolites and clays for the removal of heavy metals from water.

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“…Thus, the adsorbent surface was dominated by negative charges that attracted positively charged metallic ions. It is widely reported that the surface charges on most clay crystals emanate from hydroxyl (OH) groups (Adebowale et al, 2006;Bradl, 2004), however this study did not measure any Infra-Red (IR)-related parameters to identify functional groups.…”

Section: Monometal Systemmentioning

confidence: 99%

“…Similarly, for monometal experiment, six concentration levels of 0, 2.5, 5, 10, 25 and 50 mg/L of each bimetal combination were maintained and sorption experiments were achieved by weighing 20 mg of the soil mineral matrix (clay extract) into 50 mL propylene tubes and equilibrating with a 20 mL of a binary-metal solution. In both experiments (mono and binary-metal), the tubes were shaken in a horizontal shaker for 3h at 25±2 °C, a previously determined optimal equilibration time (Alumaa, Kirso, Petersell, & Steinnes, 2002;Adebowale, Unuabonah, & Olu-Owalabi, 2006;Ghorbel-Abid & Trabeisi-Ayadi, 2011) followed by centrifuging at 3000 rpm for 20 min and subsequent filtration through a filter paper (Whatman No. 42) to obtain a clear filtrate.…”

Section: Adsorption Experimentsmentioning

confidence: 99%

Sorption of Heavy Metals by Ferralic-Arenosol and Vertic-Luvisol: A Comparative Isothermal Study

Mosekiemang¹,

Dikinya²,

Toteng³

2014

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Modeling of sorption data is essential for characterizing retention of heavy metals by the soil matrices as well as to predict the fate of heavy metals in the environment. We carried out a study to evaluate adsorption characteristics of metallic ions (Cr 3+ , Pb 2+ and Cu 2+ ) as sole sorbates as well as in coexistence onto clay extracts of Vertic-Luvisol and Ferralic-Arenosol, the generally under-researched yet wide-spread semi-arid soils. Additionally, sorption kinetics of these heavy metals was evaluated in these soils. Equilibrium sorption data for both non-competitive and competitive metal systems were found to obey the Langmuir isotherm. Overall metal loading capacity was higher in Vertic-Luvisol than Ferralic-Arenosol whereas metal-wise affinity to binding sites favoured sorption of Cr 3+ over Pb 2+ and Cu 2+ in that order. Contrary to the hypothesis of this study, the preferential sorption process was found to be driven by cationic properties as opposed to soil properties. Adsorption of metallic ions onto soils was significantly reduced in competitive systems than non-competitive systems, a phenomenon attributable to the antagonistic effects of coexisting species. Cr 3+ suppressed sorption of Pb 2+ and Cu 2+ on both soils as validated by the competitive adsorption capacity ratios which were < 1 in all instances where Cr 3+ coexisted with either one of Pb 2+ or Cu 2+ . The adsorption kinetics of metal ions in both soils followed the pseudo-second-order rate law, suggesting chemical sorption as the rate-limiting step of the adsorption process.

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The effect of some operating variables on the adsorption of lead and cadmium ions on kaolinite clay

Cited by 214 publications

References 54 publications

Competitive adsorption of metal ions onto goethite–humic acid-modified kaolinite clay

Competitive adsorption of metal ions onto goethite–humic acid-modified kaolinite clay

Use of Surfactant-Modified Zeolites and Clays for the Removal of Heavy Metals from Water

Sorption of Heavy Metals by Ferralic-Arenosol and Vertic-Luvisol: A Comparative Isothermal Study

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