The solubility product $({K_{sp}})$ of $BaCO_3$ is $1.5 \times 10^{-9}$. At what concentration of $Ba^{2+}$ ions will precipitation begin when solid $Ba(NO_3)_2$ is added to a $10^{-4} \ M$ solution of $Na_2CO_3$?
- A$1.5 \times 10^{-5} \ M$
- B$5.1 \times 10^{-5} \ M$
- C$1.5 \times 10^{-4} \ M$
- D$1.0 \times 10^{-5} \ M$
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