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8.21. The Mn3+ ion is unstable in solution and undergoes disproportionation to give Mn2+, MnO2 and H+ ion. Write a balanced ionic equation for the reaction.

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    Answered by

    Vishal Baghel | Contributor-Level 10

    4 months ago

    The unbalanced chemical reaction is:
    Mn3+ (aq) → Mn2+ (aq) + MnO2? (s) + H+ (aq)
    The oxidation half reaction is,  
    Mn3+ (aq) → MnO2? (s).
    To balance oxidation number, one electron is added on R.H.S.
    Mn3+ (aq) → MnO2? (s) + e−
    4 protons are added to balance the charge.
    Mn3+ (aq) → MnO2? (s) + 4H+ (aq) + e−
    2 water molecules are added to balance O atoms.
    The reduction half reaction is Mn3+ (aq) → Mn2+ (aq).
    An electron is added to balance oxidation number.
    Mn3+ (aq) + e− → Mn2+ (aq)
    Two half-cell reactions are added to obtain balanced chemical equation.
    2Mn3+ (aq) + 2H2? O (l) → Mn2+ (aq)

    ...more

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