A solution contains 0.1 M `H_2 S` and 0.3 M HCl. Calculate the concentration of S2- and HS ions in the solution. For `H_2S K_(a_1) = 1 xx 10^(-7) , K_(a_2) = 1.3 xx 10^(-13)`

Explanation

To solve the problem of calculating the concentrations of \( S^{2-} \) and \( HS^- \) ions in a solution containing 0.1 M \( H_2S \) and 0.3 M \( HCl \), we can follow these steps:

### Step 1: Understand the dissociation of \( H_2S \)
The dissociation of \( H_2S \) can be represented as:
1. \( H_2S \rightleftharpoons H^+ + HS^- \) (with \( K_{a1} = 1 \times 10^{-7} \))
2. \( HS^- \rightleftharpoons H^+ + S^{2-} \) (with \( K_{a2} = 1.3 \times 10^{-13} \))

### Step 2: Set up the equilibrium expressions
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