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MnO(4)^(-) + SO(2)^(2-) + H(2)O = MnO(2)...

`MnO_(4)^(-) + SO_(2)^(2-) + H_(2)O = MnO_(2) + SO_(4)^(2-) + OH^(-)`

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To balance the redox reaction given, we will follow the half-reaction method. The reaction is: \[ \text{MnO}_4^{-} + \text{SO}_2^{2-} + \text{H}_2\text{O} \rightarrow \text{MnO}_2 + \text{SO}_4^{2-} + \text{OH}^{-} \] ### Step 1: Assign Oxidation States First, we need to assign oxidation states to identify the species being oxidized and reduced. - In \(\text{MnO}_4^{-}\), Mn has an oxidation state of +7. ...
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