At T(K),K_{sp} of two ionic salts MX_2 and MX | vedclass

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Question

(A) For salt $MX_2$: $MX_2 ightleftharpoons M^{2+} + 2X^-$. Let solubility be $S_1$. Then $K_{sp} = (S_1)(2S_1)^2 = 4S_1^3$. Given $4S_1^3 = 5 	ime

Vedclass · Accepted Answer

$12.5$

Vedclass · Answer

(A) For salt $MX_2$: $MX_2 ightleftharpoons M^{2+} + 2X^-$. Let solubility be $S_1$. Then $K_{sp} = (S_1)(2S_1)^2 = 4S_1^3$. Given $4S_1^3 = 5 	imes 10^{-13}$,so $S_1^3 = 1.25 	imes 10^{-13} = 125 	imes 10^{-15}$. Thus,$S_1 = 5 	imes 10^{-5} \ M$.For salt $MX$: $MX ightleftharpoons M^+ + X^-$. Let solubility be $S_2$. Then $K_{sp} = S_2^2$. Given $S_2^2 = 1.6 	imes 10^{-11} = 16 	imes 10^{-12}$. Thus,$S_2 = 4 	imes 10^{-6} \ M$.The ratio of molar solubility is $\frac{S_1}{S_2} = \frac{5 	imes 10^{-5}}{4 	imes 10^{-6}} = \frac{50}{4} = 12.5$.

At $T(K)$,$K_{sp}$ of two ionic salts $MX_2$ and $MX$ is $5 \times 10^{-13}$ and $1.6 \times 10^{-11}$ respectively. The ratio of molar solubility of $MX_2$ and $MX$ is

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