`K_(sp)` of `PbBr_(2)` is `8 xx 10^(-5)`. If the salt is `80%` dissociated in solution, calculate the solubility of salt in `gL^(-1)`.

Explanation

To solve the problem, we need to calculate the solubility of lead(II) bromide (PbBr₂) given that its solubility product (Ksp) is \(8 \times 10^{-5}\) and that the salt is 80% dissociated in solution.

### Step-by-Step Solution:

1. **Write the dissociation equation**:
\[ \text{PbBr}_2 (s) \rightleftharpoons \text{Pb}^{2+} (aq) + 2 \text{Br}^- (aq) \]
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