The first ionization constant of `H_(2)S` is `9.1xx10^(-8)`. Calculate the concentration of `HS^(Θ)` ion in its `0.1 M` solution. How will this concentration be affected if the solution is `0.1 M` in `HCl` also? If the second dissociation constant if `H_(2)S` is `1.2xx10^(-13)`, calculate the concentration of `S^(2-)` under both conditions.

Explanation

To solve the problem, we will follow these steps:

### Step 1: Calculate the concentration of `HS⁻` in a `0.1 M` solution of `H₂S`.

The first dissociation of `H₂S` can be represented as:
\[ H_2S \rightleftharpoons H^+ + HS^- \]

Let the initial concentration of `H₂S` be `0.1 M`. If we let `x` be the concentration of `H^+` and `HS⁻` produced, we can set up the following equilibrium expression based on the first ionization constant \( K_{a1} \):
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