At 298 , K,the solubility product (K_{sp}) of | vedclass

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(B) The dissociation of $M_2SO_4$ is given by: $M_2SO_4(s) \rightleftharpoons 2M^+(aq) + SO_4^{2-}(aq)$.Let the solubility of $M_2SO_4$ be $s \, mol/L

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$2.89 	imes 10^{-2} \, M$

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(B) The dissociation of $M_2SO_4$ is given by: $M_2SO_4(s) ightleftharpoons 2M^+(aq) + SO_4^{2-}(aq)$.Let the solubility of $M_2SO_4$ be $s \, mol/L$.Then,$[M^+] = 2s$ and $[SO_4^{2-}] = s$.The solubility product expression is $K_{sp} = [M^+]^2 [SO_4^{2-}] = (2s)^2(s) = 4s^3$.Given $K_{sp} = 1.2 	imes 10^{-5}$,we have $4s^3 = 1.2 	imes 10^{-5}$.$s^3 = 0.3 	imes 10^{-5} = 3.0 	imes 10^{-6}$.$s = (3.0 	imes 10^{-6})^{1/3} \approx 1.442 	imes 10^{-2} \, M$.The concentration of $M^+$ is $[M^+] = 2s = 2 	imes 1.442 	imes 10^{-2} = 2.884 	imes 10^{-2} \, M \approx 2.89 	imes 10^{-2} \, M$.

At $298 \, K$,the solubility product $(K_{sp})$ of $M_2SO_4$ (where $M^+$ is a monovalent metal ion) is $1.2 \times 10^{-5}$. What is the maximum concentration of $M^+$ ions in a saturated solution of this salt at $298 \, K$?

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