Organic ligand induced release of vanadium from the dissolution of stone coal oxide ore
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The effects of low-molecular-weight dissolved organic matters (LMWDOMs) on the release of vanadium (V) under environmental conditions are part of a broader study on the environmental geochemistry behavior of V. Eight typical naturally occurring LMWDOMs with carboxyl, hydroxyl, and amidogen groups were chosen: citric acid, oxalic acid, EDTA, salicylic acid, catechol, glycine, cysteine, and glucose. The results showed that the release of V was largely promoted by LMWDOMs with carboxyl functional groups under acidic conditions and with catechol under basic conditions. In the presence of citric acid, oxalic acid, or EDTA at pH 4.0, the initial release rates of V were approximately 25–39 times greater than the rates in the control experiments; the steady release rates were 164, 95, and 49 times than the rates in the control experiments, respectively. For catechol, the release rate at pH 8.0 was approximately 20 times the rate at pH 4.0. Amino acids and alcohols had a minimal effect on the release of V. Ligand-promoted release rates of V were found primarily due to the faster detachment of surface complexes, the protonated sites from the mineral surface and the reduction of dissolved V (V) in the presence of citric acid, oxalic acid, EDTA, and catechol. This study helps understand the pollution risk of V in some mine areas and the fate of V in the environment.
KeywordsVanadium Stone coal Dissolved organic matters Kinetics Dissolution Complexation
This work was supported by the National Natural Science Foundation of China [grant numbers 41641034, 21607166, and 41473113] and the National Water Pollution Control and Treatment Science and Technology Major Project [grant number 2015ZX07205-003].
- Baroch F (2000) Vanadium and vanadium alloys. In: Kirk-Othmer Encyclopedia of Chemical Technology. John Wiley & Sons, Inc, pp 1–18Google Scholar
- Bin Z (2006) Progress of the research on extraction of vanadium pentoxide from stone coal and the market of the V2O5. Hunan Nonferrous Metals 22(1):16–20 (in Chinese)Google Scholar
- Brantley SL (2008) Kinetics of Mineral Dissolution. Springer Publishing, New York, pp 151–210Google Scholar
- Evans HT, White JD (1987) The colorful vanadium minerals: a brief review and a new classification. Mineralogical Theatr Rec 18:333–340Google Scholar
- Lide DR (2008) CRC Handbook of Chemistry and Physics, 88th edn. CRC Press, Boca Raton, pp 4–40Google Scholar
- Małuszynski MJ (2007) Vanadium in Environment. Ochrona Srodowiska i Zasobów Naturalnych, Ochr’ Sr Zasobów Nat 31:475–478Google Scholar
- Polyak DE (2011) U.S. Geological Survey 2009. Minerals Yearbook, VanadiumGoogle Scholar
- Sposito G (2004) The Surface Chemistry of Natural Particles. Oxford University Press, Oxford/New YorkGoogle Scholar
- Sposito G (2008) The Chemistry of Soils. Oxford University Press, Oxford/New YorkGoogle Scholar
- Tracey AS, Gresser MJ, Parkinson KM (1987) Vanadium (V) oxyanions. Interactions of vanadate with oxalate, lactate and g1ycerate. Inorg Chem 26:629–638. https://doi.org/10.1002/chin.198730076
- Waples JS, Nagy KL, Aiken GR, Ryan JN (2005) Dissolution of cinnabar (HgS) in the presence of natural organic matter. Geochim Cosmochim Acta 69(6):1575–1588. https://doi.org/10.1016/j.gca.2004.09.029