Solid Ba(NO_3)_2 is gradually added to a 1.0 | vedclass

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(D) For the precipitation of $BaCO_3$ to occur,the ionic product must exceed the solubility product constant $(K_{sp})$.The condition for the start of

Vedclass · Accepted Answer

$5.1 	imes 10^{-5} \, M$

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(D) For the precipitation of $BaCO_3$ to occur,the ionic product must exceed the solubility product constant $(K_{sp})$.The condition for the start of precipitation is: $[Ba^{2+}][CO_3^{2-}] = K_{sp}$.Given that $[CO_3^{2-}] = 1.0 	imes 10^{-4} \, M$ and $K_{sp} = 5.1 	imes 10^{-9}$.Substituting the values: $[Ba^{2+}] 	imes (1.0 	imes 10^{-4}) = 5.1 	imes 10^{-9}$.Therefore,$[Ba^{2+}] = \frac{5.1 	imes 10^{-9}}{1.0 	imes 10^{-4}} = 5.1 	imes 10^{-5} \, M$.

Solid $Ba(NO_3)_2$ is gradually added to a $1.0 \times 10^{-4} \, M \, Na_2CO_3$ solution. At what concentration of $Ba^{2+}$ will precipitation start? (Given $K_{sp}$ for $BaCO_3 = 5.1 \times 10^{-9}$)

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