Comparative Kinetics of Iron Ore Dissolution in Aqueous HCl-HNO3 System

DOI: 10.4236/jmmce.2013.14026   PDF   HTML     3,470 Downloads   4,684 Views   Citations


The dissolution kinetics of the dissolution of iron ore in aqueous HCl/HNO3solution was studied. The elemental composition of the ore was carried out using the inductively coupled plasma-optical emission spectrophotometer (ICP-OES). The result showed that the iron ore contain; Fe (62.1%), O (21.7%), Cu (11.1%), Mg (2.39%), Na (1.51%), Mn (1.47%), K (0.78%), Ca (0.58%) and Zn (0.01%). It was determined that the dissolution rate increased with increased solution concentration, temperature, time and decreased particle size of the ore. The optimum conditions for effective dissolution of 88% of the iron ore were found to be 8 Mof the solution, 353 K, 100 min and ore particle size of less than 75 μm. The kinetic evaluation of the dissolution process was studied using three different shrinking core models (SCM); Film diffusion: kft =XB; interfacial chemical reaction krt = 1-(1-XB)1/3 and ash/product layer diffusion :  for spherical materials was performed. The results obtained showed that the rate determining step for the dissolution process was the product layer diffusion and therefore, the reaction followed this mechanism. The apparent activation energy (Ea) and the order of reaction were found to be 20.48 kJ/mol and 0.7 respectively.

Share and Cite:

O. Gerald, N. Christopher, O. Ayebatonworio and O. Martin, "Comparative Kinetics of Iron Ore Dissolution in Aqueous HCl-HNO3 System," Journal of Minerals and Materials Characterization and Engineering, Vol. 1 No. 4, 2013, pp. 153-159. doi: 10.4236/jmmce.2013.14026.

Conflicts of Interest

The authors declare no conflicts of interest.


[1] A. A. Baba, F. A. Adekola and A. J. Lawal, “Investigation of Chemical and Microbial Leaching of Iron Ore in Sulphuric Acid,” Journal of Applied Sciences and Environmental Management, Vol. 11, No. 1, 2007, pp. 39-44.
[2] A. A. Baba, F. A. Adekola, and A. O. Folashade, “Quatitative Leaching of a Nigerian Iron ore in Hydrochloric acid,” Journal of Applied Sciences and Environmental Management, Vol. 9, No. 3, 2005, pp. 15-20.
[3] A. A. Baba, A. A. Folahan, A. A. Olayide, I. Lateef, B. B. Rafiu, K. G. Malay and R. S. Abdul, “Simultaneous Recovery of Total Iron and Titanium from Ilmenite Ore by Hydrometallurgical Processing,” Metallurgical and Materials Engineering, Vol. 18, No. 1, 2012, pp. 67-78.
[4] G. Gülfen, M. Gülfen and A. O. Aydam, “Dissolution Kinetics of Iron from Diasporic Bauxite in Hydrochloric Acid Solution,” Indian Journal of Chemical Technology, Vol. 13, No. 4, 2006, pp. 386-390.
[5] A. Martinez-Luévanos, M. G. Rodriguez-Delgado, A. Uribe-Salas, F. R. Carrillo-Pedroza and J. G. Osuna-Alarcon, “Leaching Kinetic of Iron from Low-Grade Kaolin by Oxalic Acid Solutions,” Applied Clay Science, Vol. 51, No. 4, 2011, pp. 473-477. doi:10.1016/j.clay.2011.01.011
[6] O. Levenspiel, “Chemical Reaction Engineering,” 3rd Edition, John Wiley and Sons Inc., New York, 1999, pp. 566-582.
[7] S. Yagi and D. Kunnii, 5th Symposium (International) on Combustion, In: O. Levenspiel, Ed., Chemical Reaction Engineering, 3rd Edition, John Wiley & Sons, New York, p. 231.
[8] S. Yagi, D. Kunnii, Chemical Engineering Science, Vol. 16, In: O. Levenspiel, Ed., Chemical Reaction Engineering, 3rd Edition, John Wiley & Sons, New York, pp. 364-380.
[9] H. Su, H. Liu, F. Wang, X. Lu and Y. Wen, “Kinetics of Reductive Leaching of Low-Grade Pyrolusite with Molasses Alcohol Wastewater in H2SO4,” Chinese Journal of Chemical Engineering, Vol. 18, No. 5, 2010, pp. 730-735.

comments powered by Disqus

Copyright © 2020 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.