Dissolution of Magnetite and Hematite in Mixtures of Oxalic and Nitric Acid: Mechanisms and Kinetics

Abstract

Dissolution mechanisms and kinetics have a key role in better understanding of processes. In this work, magnetite and hematite powder were dissolved in oxalic and nitric acid mixtures at different temperatures. Higher temperature and higher amounts of oxalic acid in the system accelerated the dissolution kinetics but did not result in higher solubility levels. Oxalic acid had also drawbacks in the process since higher amounts in the system promoted formation of a solid product, humboldtine (Fe(II)C2O4∙2H2O), which, in turn, inhibited the dissolution. This problem may be overcome by adding even a small amount of nitric acid to the system. Kinetic analysis showed, in the variable-rate-controlling step, that two linear fits of the Kabai model described the dissolution better in an oxalic acid and acid mixture of 70/30. Thermodynamic data and special cubic models showed that the nitric acid concentration had a significant role in the solubility, whereas the concentration of oxalic acid had only minor effects on solubility. The results also showed that measuring the oxalate and nitrate concentrations did not provide additional information about the dissolution mechanism itself. The pH, however, might be a tool for following the extent of dissolution, even though it is not a direct indicator of the dissolution mechanism.

Demulsification of Pickering Emulsions by Chemical Dissolution of Stabilizers

“…These iron(III) ions further get reduced to form ferrous oxalate. After the complete dissolution process, a solid precipitate gets accumulated at bottom of vial, which in line with literature reports 25,26 is found to be humboldtine precipitate Fe(II)C 2 O 4 •2(H 2 O). The overall reaction can be written as 24…”

“…These iron(III) ions further get reduced to form ferrous oxalate. After the complete dissolution process, a solid precipitate gets accumulated at bottom of vial, which in line with literature reports , is found to be humboldtine precipitate Fe(II)C 2 O 4 ·2(H 2 O). The overall reaction can be written as Fe 2 normalO 3 + normalH + + 5 normalH 2 normalC 2 normalO 4 − ⇒ 2 false( FeC 2 normalO 4 false) 2 2 − + 3 normalH 2 normalO + 2 normalC normalO 2 false↑ Fe 2 normalO 3 + 6 normalH 2 normalC 2 normalO 4 ⇒ Fe ( II ) normalC 2 normalO 4 · 2 ( H 2 O ) In the case of the reaction between hydrochloric acid and hematite, it follows a simple reaction of metal oxide and acid giving metal salts and water …”

“…These iron­(III) ions further get reduced to form ferrous oxalate. After the complete dissolution process, a solid precipitate gets accumulated at bottom of vial, which in line with literature reports , is found to be humboldtine precipitate Fe­(II)­C 2 O 4 ·2­(H 2 O). The overall reaction can be written as In the case of the reaction between hydrochloric acid and hematite, it follows a simple reaction of metal oxide and acid giving metal salts and water …”