In the following reaction
`overset(ɵ)(O)H+S_(2)O_(3)^(2-)+Br_(2)toSO_(4)^(2-)+Br^(ɵ)`
Starting with 0.15 " mol of "`Br_(2)` 0.01 " mol of "`S_(2)O_(3)^(2-)` and 0.4 " mol of "`overset(ɵ)(O)H` ions. How many moles of `overset(ɵ)(O)H` ions are left in the solution after the reaction is complete.

Explanation

To solve the problem step by step, we will follow these procedures:

### Step 1: Write the balanced chemical equation
The reaction is given as:
\[ \text{OH}^- + \text{S}_2\text{O}_3^{2-} + \text{Br}_2 \rightarrow \text{SO}_4^{2-} + \text{Br}^- \]

### Step 2: Determine oxidation states
- For sulfur in \(\text{S}_2\text{O}_3^{2-}\):
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