Calculate the minimum concentration of sulpha | vedclass

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(A) The precipitation of $BaSO_4$ occurs when the ionic product exceeds the solubility product constant $(K_{sp})$.For precipitation to start,the ioni

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$4 	imes 10^{-6} \ mol/L$

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(A) The precipitation of $BaSO_4$ occurs when the ionic product exceeds the solubility product constant $(K_{sp})$.For precipitation to start,the ionic product must be equal to $K_{sp}$.$K_{sp} = [Ba^{2+}][SO_4^{2-}]$Given: $K_{sp} = 4 	imes 10^{-10}$ and $[Ba^{2+}] = 10^{-4} \ mol/L$.Substituting the values: $4 	imes 10^{-10} = (10^{-4}) 	imes [SO_4^{2-}]$$[SO_4^{2-}] = \frac{4 	imes 10^{-10}}{10^{-4}} = 4 	imes 10^{-6} \ mol/L$.Therefore,the minimum concentration of sulphate ion required is $4 	imes 10^{-6} \ mol/L$.

Calculate the minimum concentration of sulphate ion required to precipitate $BaSO_4$ in a solution containing $10^{-4} \ mol/L$ of $Ba^{2+}$. $(K_{sp} \ BaSO_4 = 4 \times 10^{-10})$

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