Write the disproportionation reaction of `ClO^(-) ` to `Cl^(-) and ClO_(3)^(-)`

Explanation

To write the disproportionation reaction of \( \text{ClO}^- \) to \( \text{Cl}^- \) and \( \text{ClO}_3^- \), we need to follow these steps:

### Step 1: Identify the oxidation states
In the ion \( \text{ClO}^- \):
- Chlorine (Cl) has an oxidation state of +1.
- Oxygen (O) has an oxidation state of -2.

In the products:
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