Permanganate ion reacts with bromide ion in basic medium to give magnesium dioxide and bromate ion.Write the balanced ionic equation for the reaction.

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Solution

1) $2 M n O_{4}^{-} (a q) + B r - (a q) + H_{2} O (l) ⟶ 2 M n O_{2} (s) + B r O_{3} (a q) + 2 O H^{-} (a q)$
Here, instead of solving the overall reaction we solve as half reactions.
The two half reactions occurring here are written as:
$B r^{-} + 3 H_{2} O ⟶ B r O_{3}^{-} + 6 H^{+} + 6 e^{-}$ -----(Oxidation)
$M n O_{4}^{-} + 4 H^{+} + 3 e^{-} \to M n O_{2} + 2 H_{2} O$ ----- (Reduction)
As in the reduction reaction no. of e- involved is half that of the one in the oxidation we will multiply the reaction by 2 so it becomes
$2 M n O_{4}^{-} + 8 H^{+} + 6 e^{-} ⟶ 2 M n O_{2} + 4 H_{2} O$
Thus, reaction can be balanced.

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