`ClO^(-) + CrO_(2)^(2-) + OH^(-) = Cl^(-) + CrO_(4)^(2-) + H_(2)O`

Explanation

To balance the redox reaction \( \text{ClO}^- + \text{CrO}_2^{2-} + \text{OH}^- = \text{Cl}^- + \text{CrO}_4^{2-} + \text{H}_2\text{O} \), we will follow these steps:

### Step 1: Identify Oxidation States
- In \( \text{ClO}^- \), chlorine (Cl) has an oxidation state of +1.
- In \( \text{Cl}^- \), chlorine has an oxidation state of -1.
- In \( \text{CrO}_2^{2-} \), chromium (Cr) has an oxidation state of +2.
- In \( \text{CrO}_4^{2-} \), chromium has an oxidation state of +6.

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