Balance the equation in acidic medium
`H_(2)S + Fe^(3+) to Fe^(3+) + S + H^(+)`

Explanation

To balance the redox reaction \( H_2S + Fe^{3+} \rightarrow Fe^{2+} + S + H^+ \) in acidic medium, we will follow these steps:

### Step 1: Identify Oxidation and Reduction
- **Oxidation**: In \( H_2S \), sulfur (S) has an oxidation state of -2. In elemental sulfur (S), the oxidation state is 0. Therefore, sulfur is oxidized from -2 to 0, which involves the loss of 2 electrons.
- **Reduction**: Iron (Fe) is reduced from +3 in \( Fe^{3+} \) to +2 in \( Fe^{2+} \), which involves the gain of 1 electron.

### Step 2: Write Half-Reactions
- **Oxidation Half-Reaction**:
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