The solubility of `TI_(2)S` in pure `CO_(2)` -free water is `6.3 xx 10^(-6)M`. Assume that the dissolved `S^(2-)` ion hydrolyses almost completely to `HS^(Θ)` and that the further hydrolysis to `H_(2)S` is neglected. What is the `K_(sp).(K_(2)(H_(2)S) = 10^(-14))`.

Explanation

To solve the problem, we need to calculate the solubility product constant \( K_{sp} \) for \( Tl_2S \) given its solubility in water and the hydrolysis of the sulfide ion \( S^{2-} \).

### Step-by-Step Solution:

1. **Identify the solubility of \( Tl_2S \)**:
The solubility of \( Tl_2S \) in pure carbon dioxide-free water is given as \( 6.3 \times 10^{-6} \, M \). Let's denote this solubility as \( S \).

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