JEE PYQ: Ionic Equilibrium Question 16
Question 16 - 2020 (06 Sep Shift 2)
Type: Numerical
If the solubility product of $\text{AB}_2$ is $3.20 \times 10^{-11}\text{M}^3$, then the solubility of $\text{AB}_2$ in pure water is ____ $\times 10^{-4}$ mol $\text{L}^{-1}$.
[Assuming that neither kind of ion reacts with water]
Show Answer
Answer: 2
Solution
$\text{AB}_2 \rightleftharpoons \text{A}^{2+}(aq) + 2\text{B}^-(aq)$
$K_{sp} = 4s^3 = 3.2 \times 10^{-11}$
$s^3 = 8 \times 10^{-12}$
$s = 2 \times 10^{-4}$ mol $\text{L}^{-1}$
BETA
