Chemistry · 2020
JEE Main · 6 September 2020, Shift 2 · Q47
If the solubility product of AB_2 is 3.20 × 10^-11 M^3, then the solubility of A B_2 in pure water is \ \ \ \ × 10^-4 mol L^-1. [Assuming that…
If the solubility product of $\displaystyle \mathrm{AB}_2$ is $\displaystyle 3.20 \times 10^{-11} \mathrm{M}^3$, then the solubility of $\displaystyle A B_2$ in pure water is \_\_\_\_ $\displaystyle \times 10^{-4} \mathrm{~mol} \mathrm{~L}^{-1}$. [Assuming that neither kind of ion reacts with water]
Official answer
2
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