Sorption of uranyl and arsenate on SiO2, Al2O3, TiO2 and FeOOH

Nair, Sreejesh; Karimzadeh, Lotfollah; Merkel, Broder J.

doi:10.1007/s12665-014-3258-x

Cited by 25 publications

(9 citation statements)

References 31 publications

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“…Although numerous studies have investigated the cosorption of uranyl-arsenate onto various mineral surfaces, − only a few studies have focused on their aqueous properties. , Through the time-resolved laser-induced fluorescence spectroscopy (TRLFS) measurements, it has been suggested that UO 2 H 2 AsO 4 + is the major uranyl arsenate species in the pH range of 1.5–3.5 . Their microstructures were further investigated by Gezahegne et al (2012), who proposed that the bidentate-coordinated 1:2 complex (i.e., UO 2 (H 2 AsO 4 ) 2 0 ) rather than UO 2 H 2 AsO 4 + should be dominant at a pH of 2 by combining static density functional theory (DFT) calculation and extended X-ray absorption fine structure (EXAFS) fitting.…”

Section: Introductionmentioning

confidence: 99%

Uranyl Arsenate Complexes in Aqueous Solution: Insights from First-Principles Molecular Dynamics Simulations

Liu

Cheng

et al. 2018

Inorg. Chem.

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In this study, the structures and acidity constants (p K's) of uranyl arsenate complexes in solutions have been revealed by using the first principle molecular dynamics technique. The results show that uranyl and arsenate form stable complexes with the U/As ratios of 1:1 and 1:2, and the bidentate complexation between U and As is highly favored. Speciation-pH distributions are derived based on free energy and p K calculations, which indicate that for the 1:1 species, UO(HAsO)(HO) is the major species at pH < 7, while UO(HAsO)(HO) and UO(AsO)(HO) dominate in acid-to-alkaline and extreme alkaline pH ranges. For the 1:2 species, UO(HAsO)(HO) is dominant under acid-to-neutral pH conditions, while UO(HAsO)(HAsO)(HO), UO(HAsO)(HAsO)(HO), and UO(AsO)(HAsO)(HO) become the major forms in the pH range of 7.2-10.7, 10.7-12.1, and >12.1, respectively.

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Section: Introductionmentioning

confidence: 99%

Uranyl Arsenate Complexes in Aqueous Solution: Insights from First-Principles Molecular Dynamics Simulations

Liu

Cheng

et al. 2018

Inorg. Chem.

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“…[16] Nair et al have used SiO 2 , Al 2 O 3 , TiO 2 and FeOOH to adsorb uranyl and arsenate. [17] Xu et al have synthesized amidoximated chitosangrafted polyacrylonitrile for uranium (VI) adsorption. [18] Gu et al have prepared graphene oxide-carbon nanotubes hybrid aerogels for removal of uranium (VI).…”

Section: Introductionmentioning

confidence: 99%

In situ growth of ZnO nanorod arrays on cotton cloth for the removal of uranium(vi)

Zhang

et al. 2015

RSC Adv.

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In situ growth of ZnO nanorod arrays on cotton cloth (ZnO/CC) was proposed to remove uranium (VI) from aqueous solution. The as-prepared adsorbent is easy separation from the reaction medium after adsorption. The effect factors for uranium adsorption, such as solution pH, initial U (VI) concentration, contact time, and temperature have been systematically investigated. The maximum adsorption capacity of uranium (VI) which was calculated by the Langmuir model at pH=5.0 and T=298 K is 431.03 mg g -1 , exhibiting its excellent uranium adsorption properties. It was observed that the kinetic data fit well to the pseudo-second-order kinetic model indicating that the rate-limiting step of adsorption process is chemical adsorption. Moreover, thermodynamic parameters [ΔH 0 =20.26 kJ mol -1 ΔG 0 =-5.66 kJ mol -1 (298 K) ΔS 0 =86.98 J mol -1 K -1 ] reveal that the uranium adsorption is endothermic and spontaneous. Therefore, the ZnO/CC is a potential adsorbent for recovery of uranium (VI) from aqueous solution.

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“…At the same time, the binding energy and relative strength of Si-O and Al-O are also reduced. This is because in the silicon aluminum oxide, the oxygen atom will have a certain complexation with uranyl ion (Nair et al 2014). However, the binding energy of C=O did not change, indicating that C=O did not participate in the adsorption reaction, similar to the ZHANG study (Zhang et al 2019c).…”

Section: Xps Analysismentioning

confidence: 58%

Preparation of aluminum sludge composite gel spheres and adsorption of U(IV) from aqueous solution

Yang

Lei

Dai

et al. 2020

Environ Sci Pollut Res

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A novel three-dimensional aluminum sludge/polyvinyl alcohol/sodium alginate(AS/PA/SA) gel spheres were designed and prepared for uranium(VI) adsorption, and it overcomes the shortcomings of poor recycling of powdery aluminum sludge adsorbent and poor stability of sodium alginate. Experiments show that the P-S-AS has a good pH range for removal of uranium (4-5). Fitting experimental data with pseudo-first-order kinetic model and pseudo-second-order kinetic model shows that the adsorption of U(VI) by P-S-AS is a chemical action. The fit of the Langmuir isotherm model and Freundlich isotherm model to the experimental data found that the P-S-AS adsorbed U(VI) to a single layer. Thermodynamic analysis shows that the adsorption occurs spontaneously, and an increase in temperature is favorable for the adsorption of uranium by the P-S-AS. Fourier transform infrared (FTIR) and X-ray photoelectron spectroscopy (XPS) analysis of the P-S-AS before and after adsorption showed that the main adsorption mechanism was the complexation reaction between functional groups and U(VI), the bonding reaction between metal oxides and U(VI).

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Sorption of uranyl and arsenate on SiO2, Al2O3, TiO2 and FeOOH

Cited by 25 publications

References 31 publications

Uranyl Arsenate Complexes in Aqueous Solution: Insights from First-Principles Molecular Dynamics Simulations

Uranyl Arsenate Complexes in Aqueous Solution: Insights from First-Principles Molecular Dynamics Simulations

In situ growth of ZnO nanorod arrays on cotton cloth for the removal of uranium(vi)

Preparation of aluminum sludge composite gel spheres and adsorption of U(IV) from aqueous solution

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