For a sparingly soluble salt $AB_2$,the equilibrium concentrations of $A^{2+}$ ions and $B^{-}$ ions are $1.2 \times 10^{-4} \ M$ and $0.24 \times 10^{-3} \ M$,respectively. The solubility product of $AB_2$ is :
- A$0.069 \times 10^{-12}$
- B$6.91 \times 10^{-12}$
- C$0.276 \times 10^{-12}$
- D$27.65 \times 10^{-12}$
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