Question

Determine the amount of KMnO4 in given solution by titrating with 0.1N solution of ferrous sulfates.​

Answer 1

Answer:The chemical reaction and the molecular chemical equation is given below.

Reduction half reaction –

2KMnO4 + 3H2SO4 → K2SO4 + 2MnSO4 + 3H2O + 5[O]

Oxidation half reaction –

2FeSO4(NH4)2SO4.6H2O + H2SO4 + 5[O] → Fe2(SO4)3 + 2(NH4)2SO4 + 13H2O x 5

Overall reaction –

2KMnO4 + 10FeSO4(NH4)2SO4.6H2O+8H2O → K2SO4+ 2MnSO4+ 5Fe2(SO4)3+ 10(NH4)2SO4+ 68H2O

The ionic equation involved in the process is given below.

Oxidation half reaction – [Fe2+ → Fe3+ – e–] x 5

Reduction half reaction – MnO4– + 8H+ + 5e– → Mn2+ + 4H2O

Overall ionic equation – MnO4– + 8H+ + 5Fe2+ → Mn2+ + 5Fe3+ + 4H2O

This titration is based upon oxidation-reduction titrations. When ferrous ammonium sulfate solution is titrated against potassium permanganate in the presence of acidic medium by sulfuric acid. Acidic medium is necessary in order to prevent precipitation of manganese oxide. Here KMnO4 acts as a self indicator and this titration is called permanganate titration.

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