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Why manganate ion (MnO(4)^(2-)) undergo ...

Why manganate ion `(MnO_(4)^(2-))` undergo disproportionation in acidic solutions.

Text Solution

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In acidic solutions manganese (VI) becomes unstable relative to manganese (VII) and manganese (IV). Thus in acidic solution manganate ion undergo disproportionation to permanganate ion and manganese dioxide.
`3MnO_(4)^(2-)+4H^(+)rarr2MnO_(2)+2H_(2)O`
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Knowledge Check

  • The ion that cannot undergo disproportionation is

    A
    `ClO_4^-`
    B
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    C
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    D
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  • Identify the oxidation states of Mn when MnO_3^(3-) ion undergoes disproportionation reaction under acidic medium

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    B
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    C
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    D
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  • On dissolution of Xenates [HXeO_4]^- in alkaline solution perxenate and Xe are obtained (R) Xenates show disproportionation in alkaline solution

    A
    Both (A) and (R) are true and (R) is the correct explanation of (A)
    B
    Both (A) and (R) are true and (R) is not the correct explanation of (A)
    C
    (A) is true but (R) is false
    D
    Both (A) and (R) are false

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    The Mn^(3+) ion is unstable solution and undergoes disproportionation to give Mn^(2+),MnO_(2)andH^(+) ion. Write balanced ionic equation for the reaction.

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    Which of the following ions will not undergo disproportionation?

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