What is the minimum concentration of `Ba^(+2)` ions required in order to initiate the precipitation of `BaSO_(4)` from a solution containing 0.002 mole `L^(-1)` of ` So_(4)^(-2)` ions?
(Given `K_(sp)` for ` BaSO_(4)=1.4xx10^(-10))`

Explanation

To find the minimum concentration of \( \text{Ba}^{2+} \) ions required to initiate the precipitation of \( \text{BaSO}_4 \) from a solution containing \( 0.002 \, \text{mol L}^{-1} \) of \( \text{SO}_4^{2-} \) ions, we can use the solubility product constant \( K_{sp} \) of \( \text{BaSO}_4 \).

### Step-by-step Solution:

1. **Write the expression for the solubility product \( K_{sp} \)**:
\[ K_{sp} = [\text{Ba}^{2+}][\text{SO}_4^{2-}] \]
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