THE PROBLEM It has been proposed that commercial manganese ferrite (MnFe2O4) production in Ghana is based on manganese oxide ore from the manganese mine at Nsuta in Ghana. A grade of the ore has been cleaned and composition determined as: MnO2 (55%), Fe2O3 (20%), Silica (15%) and water + minor components (10%). In the laboratory, a sample of the milled ore was leached in acidified ferrous sulphate (FeSO4) solution (stoichiometric amount of ferrous sulphate was used). The leaching reaction, assuming that only MnO2 from the ore is dissolved in the acid media used, is given as: MnO2 + FeSO4 + H2SO4 = MnSO4 + Fe2(SO4)3 + H2O Manganese ferrite was then prepared by calcining precursory hydroxides precipitated from the solution prepared. For ferrite preparation, the mole ratio of Fe:Mn in the solution must be 2:1. Solve the following: 1. Write a balanced leach reaction equation. 2. Based on 1 kg ore sample used, how much MnO2 does it contain? 3. How much FeSO4 will be required if all MnO2 dissolves? 4. What is the mole ratio of Fe:Mn in the solution prepared? 5. Using the solution above, what method in materials processing would you suggest to prepare the manganese ferrite (no description required!!). 6. How can you make up to the 2:1 Fe:Mn ratio required, if necessary, for ferrite preparation? 7. What chemical precipitant can be used in the precipitation process? 8. What compounds are precipitated from solution? 9. Write balanced equation for the precipitation reaction. Atomic mass: Mn (54.94); Fe (55.85); S (32.06); H (1)
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