Solubility product constants () of salts of types and at temperature are and , respectively. Solubil — Ionic Equilibrium Chemistry Question
Question
Solubility product constants ($K_{sp}$) of salts of types $MX, MX_2$ and $M_3X$ at temperature $T$ are $4.0 \times 10^{-8}, 3.2 \times 10^{-14}$ and $2.7 \times 10^{-15}$, respectively. Solubilities (in $\text{mol dm}^{-3}$) of the salts at temperature $T$ are in the order:
Answer: D
💡 Solution & Explanation
Calculate molar solubility ($S$) for each. For $MX$: $S^2 = 4 \times 10^{-8} \Rightarrow S = 2 \times 10^{-4} \text{ M}$. For $MX_2$: $4S^3 = 3.2 \times 10^{-14} \Rightarrow S^3 = 8 \times 10^{-15} \Rightarrow S = 2 \times 10^{-5} \text{ M}$. For $M_3X$: $27S^4 = 2.7 \times 10^{-15} \Rightarrow S^4 = 10^{-16} \Rightarrow S = 10^{-4} \text{ M}$. Comparing the values: $2 \times 10^{-4} > 10^{-4} > 2 \times 10^{-5}$. The order is $MX > M_3X > MX_2$.
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