In the disproportionation reaction (unbalanced), $Br_{2} + OH^{-} \rightarrow Br^{-} + BrO_{3}^{-} +

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In the disproportionation reaction (unbalanced), $Br_{2} + OH^{-} \rightarrow Br^{-} + BrO_{3}^{-} + H_{2}O$The ratio of Br2 molecules undergoing oxidation and reduction is

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Oxidation:$Br_{2} + 12OH^{-} ightarrow 2BrO_{3}^{-} + 6H_{2}O + 10e^{-}$Reduction:$Br_{2} + 2e^{-} ightarrow 2Br^{-}1 	imes 5$Net reaction: $6Br_{2} + 12OH^{-} ightarrow 2BrO_{3}^{-} + 10Br^{-} + 6H_{2}O$

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