What is the minimum concentration of SO_4^{2- | vedclass

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(C) The precipitation of $BaSO_4$ occurs when the ionic product exceeds the solubility product constant $(K_{sp})$.The equilibrium expression is: $BaS

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$4 	imes 10^{-6} \ M$

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(C) The precipitation of $BaSO_4$ occurs when the ionic product exceeds the solubility product constant $(K_{sp})$.The equilibrium expression is: $BaSO_4(s) ightleftharpoons Ba^{2+}(aq) + SO_4^{2-}(aq)$.The solubility product expression is: $K_{sp} = [Ba^{2+}][SO_4^{2-}]$.Given that $[Ba^{2+}] = 1.0 	imes 10^{-4} \ M$ and $K_{sp} = 4 	imes 10^{-10}$.Substituting the values: $4 	imes 10^{-10} = (1.0 	imes 10^{-4}) 	imes [SO_4^{2-}]$.Solving for $[SO_4^{2-}]$: $[SO_4^{2-}] = \frac{4 	imes 10^{-10}}{1.0 	imes 10^{-4}} = 4 	imes 10^{-6} \ M$.

What is the minimum concentration of $SO_4^{2-}$ required to precipitate $BaSO_4$ in a solution containing $1.0 \times 10^{-4} \ M \ Ba^{2+}$ ($K_{sp}$ for $BaSO_4$ is $4 \times 10^{-10}$)?

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