Share This Article:

Kinetics of Manganese Oxides Dissolution in Sulphuric Acid Solutions Containing Oxalic Acid

Abstract Full-Text HTML Download Download as PDF (Size:641KB) PP. 714-719
DOI: 10.4236/eng.2013.59085    4,449 Downloads   6,668 Views   Citations

ABSTRACT

The kinetics of the interaction of MnO2, Mn2O3, and Mn3O4, with sulphuric acid solutions and the effect of oxalic acid on this process are studied. As the sulphuric acid concentration is increased from 0.1 to 5 N, the dissolution rate of Mn2O3, Mn3O4 to MnO2 and Mn2+ ions decreases, whereas it increases with the concentration of Mn2+ ions. Upon the addition of H2Ox, the complete dissolution of Mn3O4 occurs more quickly. The reaction order with respect to the H+ and O x2- ions is +0.5 ± 0.1. A mechanism of MnO2 dissolution promotion by O x2- is proposed. The dissolution rate was found to depend on the concentrations of MnHOx - ions and was highest at pH 1.6 ± 0.2. A rate law and mechanism are suggested for manganese oxides dissolution.

Conflicts of Interest

The authors declare no conflicts of interest.

Cite this paper

I. Artamonova, I. Gorichev and E. Godunov, "Kinetics of Manganese Oxides Dissolution in Sulphuric Acid Solutions Containing Oxalic Acid," Engineering, Vol. 5 No. 9, 2013, pp. 714-719. doi: 10.4236/eng.2013.59085.

References

[1] M. A. Blesa, I. M. Perdo and A. E. Regazzoni, “Chemical Dissolution of Metal Oxides,” CRC Press, Boca Ration, 1994.
[2] S. O. Lee, T. Tran, Y. Y. Park, S. J. Kim and M. J. Kim, “Study on the Kinetics of Iron Leaching by Oxalic Acid,” International Journal of Mineral Processing, Vol. 80, No. 2-4, 2006, pp. 144-152.
[3] S. K. Mindal and P. C. Banerjee, “Iron Leaching with Oxalic Acid: Effects of Different Physico-Chemical Pa rameters,” International Journal of Mineral Processing, Vol. 74, No. 1-4, 2004, pp. 263-270.
[4] С. I. Nwoye, “Model for Computational Analysis of Dis solved Haematite and Heat Absorbed by Oxalic Acid So lution during Leaching of Iron Oxide Ore,” Journal of Engineering and Applied Science, Vol. 4, 2008, pp. 22-25.
[5] D. Panias, M. Taxiarchou, I. Paspaliaris and A. Konto poulos, “Mechanisms of Dissolution of Iron Oxides in Aqueous Oxalic Acid Solutions,” Hydrometallurgy, Vol. 42, No. 2, 1996, pp. 257-265.
doi:10.1016/0304-386X(95)00104-O
[6] D. Panias, M. Taxiarchou, I. Paspaliaris and A. Konto poulos, “Termodynamic Analysis of the Reactions of Iron Oxides: Dissolution in Oxalic Acid,” Canadian Metallur gical Quarterly, Vol. 35, No. 4, 1996, pp. 363-373. doi:10.1016/S0008-4433(96)00018-3
[7] Y. Wang and A. T. Stone, “Reaction of Mn(III,IV)(hydr) Oxades with Oxalic Acid, Glioxylic Acid, Phosphono formic Acid, Compounds,” Geochimica et Cosmochimica Acta, Vol. 70, 2006, pp. 4477-4490.
doi:10.1016/j.gca.2006.06.1548
[8] Y. Wang Y. and A. T. Stone, “The Citric Acid-Mn(III,IV) O2(s,birnessite) Reaction. Electron Transfer, Complex Formation,” Geochimica et Cosmochimica Acta, Vol. 70, 2006, pp. 4463-4476.
doi:10.1016/j.gca.2006.06.1551
[9] A. T. Stone, “Reductive Dissolution of Manganese(III)/ (IV) Oxide by Subsituted Phenols,” Environmental Sci ence & Technology, Vol. 21, No. 4, 1987, pp. 979-988. doi:10.1021/es50001a011
[10] A. T. Stone, “Reduction and Dissolution of Manganese (III) and Manganese(IV) Oxides by Organics,” Environmental Science & Technology, Vol. 18, No. 2, 1984, pp. 450-456. doi:10.1021/es00124a011
[11] A. T. Stone and I. I. Morgan, “Reductive Dissolution of Metal Oxides, in Aquatic Surface Chemistry,” Wiley, New York, 1987.
[12] A. T. Stone and H. J. Urion, “Kinetics and Reaction Sto ichiometry in the Reductive Dissolution of Manganese(IV) Dioxide and Co(III) Oxide by Hydrocarbons,” Journal of Colloid and Interface Science, Vol. 132, No. 2, 1989, pp. 509-522. doi:10.1016/0021-9797(89)90265-8
[13] A. K. Lavrukhina and L. V. Yutkina, “Analiticheskaya Khimiya Margantsa (Analytical Chemistry of Manga nese),” Nauka, Moscow, 1974.
[14] K. Vetter and N. Jaeger, “The Mechanism of Occurrence of Potential of an Electrode from Manganese Dioxide,” In: A. I. Frumkin, Ed., The Basic Questions of Modern Theoretical Electrochemistry, Mir, Moscow, 1965, pp. 253-262.
[15] B. Delmon, “Introduction a la Cinetique Heterogene, Paris: Technip,” Mir, Moscow, 1972.
[16] W. F. Tan, S. J. Lu, F. Liu, X. H. Feng, J. Z. He and L. K. Koopal, “Determination of the Point-Of-Zero Charge of Manganese Oxides with Different Methods Including an Improved Salt Titration Method,” Soil Science, Vol. 173, No. 4, 2008, pp. 277-286. doi:10.1097/SS.0b013e31816d1f12
[17] V. V. Batrakov, I. G. Gorichev and N. A. Kipriyanov, “Influence of a Double Electric Layer on the Kinetics Dissolution Oxides Metals,” Elektrokhim, Vol. 30, No. 4, 1994, pp. 444-458.
[18] R. Schmidt and V. N. Sapunov, “Neformalnaya kinetika,” Mir, Moscow, 1985.
[19] A. A. Bezdenezhnykh, “Inzhenernye Metody Sostavle niya Uravnenii Skorostei Reaktsii i Rascheta Kinetiche skikh Konstant (Engeneering Techniques of Formulation of Equations for Reaction Rates and Calculation of Kinetic Constants),” Khimiya, Leningrad, 1974.

  
comments powered by Disqus

Copyright © 2019 by authors and Scientific Research Publishing Inc.

Creative Commons License

This work and the related PDF file are licensed under a Creative Commons Attribution 4.0 International License.