An aqueous solution of a metal bromide `MBr_(2)(0.05M)` is saturated with `H_(2)S`. What is the minimum pH at which MS will precipitate ? `K_(SP)` for `M S= 6.0xx10^(-21)` . Concentration of saturqated `H_(2)S=0.1M, K_(1)=10^(-7)and K_(2)=1.3xx10^(-13)` for `H_(2)S` .

Explanation

To solve the problem, we need to determine the minimum pH at which the metal sulfide (MS) will precipitate from the solution of the metal bromide (MBr₂) when saturated with H₂S. We will use the given solubility product constant (Ksp) for MS and the dissociation constants for H₂S.

### Step-by-Step Solution:

1. **Identify the relevant equations:**
The precipitation of metal sulfide (MS) can be expressed in terms of its solubility product (Ksp):
\[
K_{sp} = [M^{2+}][S^{2-}]
...