The solubility product of `BaSO_4 ` at 298 K is ` 1.08 xx 10^(-10) ` . What is the minimum concentration of ` SO_4^(2-)` ions required to precipitate `BaSO_4` from a 0.01 M solution of `BaCl_2`

Explanation

To solve the problem, we need to determine the minimum concentration of sulfate ions (SO₄²⁻) required to precipitate barium sulfate (BaSO₄) from a 0.01 M solution of barium chloride (BaCl₂). We will use the solubility product constant (Ksp) of BaSO₄, which is given as 1.08 × 10⁻¹⁰.

### Step-by-step Solution:

1. **Write the dissociation equation for BaSO₄:**
\[ \text{BaSO}_4 (s) \rightleftharpoons \text{Ba}^{2+} (aq) + \text{SO}_4^{2-} (aq) \]
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