Kinetic modeling of the decomposition of beudantite in NaOH medium

Patiño, Francisco; Flores, Mizraím U.; Reyes, Iván A.; Ordoñez, Sayra; Méndez, Jonathan; Flores, Víctor Hugo Portilla; Islas, Hernán; Reyes, Martín

doi:10.1007/s11144-016-1065-y

Cited by 8 publications

(2 citation statements)

References 28 publications

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“…Arsenic is an extremely toxic byproduct of the mining and smelting of precious and nonferrous metals [1][2][3][4][5] and a common metalloid element in mineral feedstocks, which could be mobilized/discharged during the metallurgical operation, and it results in a serious environmental problem [6,7].…”

Section: Introductionmentioning

confidence: 99%

Dissolution, Solubility, and Stability of the Basic Ferric Sulfate-Arsenates [Fe(SO4)x(AsO4)y(OH)z·nH2O] at 25–45°C and pH 2–10

Zhu

Yang

Liu

et al. 2021

Journal of Chemistry

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Basic ferric sulfate-arsenates [FeSAsOH, Fe(SO4)x(AsO4)y(OH)z·nH2O] were prepared and characterized to study their potential fixation of arsenic in the oxidizing and acidic environment through a dissolution for 330d. The synthetic solids were well-shaped monoclinic prismatic crystals. For the dissolution of the sample FeSAsOH–1 [Fe(SO4)0.27(AsO4)0.73 (OH)0.27·0.26H2O] at 25–45°C and initial pH 2, all constituents preferred to be dissolved in the order of AsO43− > SO42− > Fe3+ in 1–3 h, in the order of SO42− > AsO43− > Fe3+ from 1–3 h to 12–24 h, and finally in the order of SO42− > Fe3+ > AsO43−. The released iron, sulfate, and arsenate existed dominantly as Fe3+/Fe(OH)2+/FeSO4+, HSO4−/SO42−/FeSO4+, and H3AsO40/H2AsO4−, respectively. The higher initial pHs (6 and 10) could obviously inhibit the release of Fe3+ from solid into solution, and the solid components were released in the order of SO42− > AsO43− > Fe3+. The crystal tops were first dissolved, and the crystal surfaces were gradually smoothed/rounded until all edges and corners disappeared. The dissociations were restricted by the Fe-O(H) breakdown in the FeO6 octahedra and obstructed by the OH− and AsO4 tetrahedra outliers; the lowest concentration of the dissolved arsenic was 0.045 mg/L. Based on the dissolution experiment at 25°C and pH 2, the solubility products (Ksp) for the basic ferric sulfate-arsenate [Fe(SO4)0.27(AsO4)0.73 (OH)0.27·0.26H2O], which are equal to the ion activity products (logˍIAP) at equilibrium, were calculated to be -23.04 ± 0.01 with the resulting Gibbs free energies of formation (ΔGfo) of −914.06 ± 0.03 kJ/mol.

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Section: Introductionmentioning

confidence: 99%

Dissolution, Solubility, and Stability of the Basic Ferric Sulfate-Arsenates [Fe(SO4)x(AsO4)y(OH)z·nH2O] at 25–45°C and pH 2–10

Zhu

Yang

Liu

et al. 2021

Journal of Chemistry

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“…The jarosite process offers the advantage of removing the iron by the high‐efficiency precipitation of the solution with relatively low losses of divalent base metals such as zinc, cadmium and copper . The particularity of these compounds is that they may have different substitutions in the structure of jarosite, working as a means of inertization incorporating elements of environmental importance, such as Tl + , Cr(VI), As(V), ½Pb 2+ , ½Cd 2+ and ½Hg 2+ reducing its impact on the environment . One of the less well studied jarosite‐type compounds is mercury jarosite Hg 0.5 Fe 3 (SO 4 ) 2 (OH) 6 , synthesized by Dutrizac and Kaiman in 1976 making it possible to incorporate 14.62 wt% mercury.…”

Section: Introductionmentioning

confidence: 99%

Kinetic Analysis of the Decomposition Reaction of the Mercury Jarosite in NaOH Medium

Ordoñez

Flores

Patiño

et al. 2017

Int. J. Chem. Kinet.

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This work presents the kinetic study of the decomposition in NaOH medium of mercury jarosite whose approximate formula is [Hg 0.39 (H 3 O) 0.22 ]Fe 2.71 (SO 4 ) 2.17 (OH) 4.79 (H 2 O) 2.09 . The reaction progress takes place on the surface of the compound with diffusion of the hydroxyl ions (OH − ) from the solution to the particle surface moving the reaction front toward the interior of the particle, with the release of ions SO 4 2and Hg 2+ from the core to the reaction medium. The decomposition curve can be described by three kinetics stages: an induction period followed by a progressive conversion period and ending the reaction in the stabilization zone. The results of X−ray diffraction showed that as the decomposition reaction progresses the partially decomposed solids lost its crystallinity ending as amorphous solids. For the induction period, the reaction order (n) was 0.52 for [OH − ] < 0.0187 mol L −1 and when [OH − ] > 0.0187 mol L −1 n = 1.48, whereas the calculated activation energy (E a ) was 81.7 kJ mol −1 . For the progressive conversion period n = 0.99 for [OH − ] > 0.0057 mol L −1 and for lower concentrations n 0, with E a = 56.9 kJ mol −1 , confirming that the decomposition process is controlled by the chemical reaction. Based on the calculated kinetic parameters, the partial

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Analytical solutions for the rate equations of irreversible two-step consecutive processes with mixed second order later steps

Lente

2016

J Math Chem

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Kinetic modeling of the decomposition of beudantite in NaOH medium

Cited by 8 publications

References 28 publications

Dissolution, Solubility, and Stability of the Basic Ferric Sulfate-Arsenates [Fe(SO4)x(AsO4)y(OH)z·nH2O] at 25–45°C and pH 2–10

Dissolution, Solubility, and Stability of the Basic Ferric Sulfate-Arsenates [Fe(SO4)x(AsO4)y(OH)z·nH2O] at 25–45°C and pH 2–10

Kinetic Analysis of the Decomposition Reaction of the Mercury Jarosite in NaOH Medium

Analytical solutions for the rate equations of irreversible two-step consecutive processes with mixed second order later steps

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