If the solubility product of $\mathrm{AB}_2$ is $3.20 \times 10^{-11} \mathrm{M}^3$, then the solubility of $A B_2$ in pure water is $\_\_\_\_$ x $10^{-4} \mathrm{~mol} \mathrm{~L}^{-1}$. [Assuming that neither kind of ion reacts with water]
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