What is the molar solubility of Ag_2CO_3 (K_{ | vedclass

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(A) The dissociation of $Ag_2CO_3$ is given by: $Ag_2CO_{3(s)} \rightleftharpoons 2Ag^+{(aq)} + CO_3^{2-}{(aq)}$
In $0.1 \ M \ Na_2CO_3$ solution,the

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$10^{-6}$

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(A) The dissociation of $Ag_2CO_3$ is given by: $Ag_2CO_{3(s)} ightleftharpoons 2Ag^+{(aq)} + CO_3^{2-}{(aq)}$
In $0.1 \ M \ Na_2CO_3$ solution,the concentration of $CO_3^{2-}$ ions is $0.1 \ M$ due to the common ion effect.
Let $s$ be the molar solubility of $Ag_2CO_3$. Then $[Ag^+] = 2s$ and $[CO_3^{2-}] = (s + 0.1) \approx 0.1 \ M$ (since $s$ is very small).
The solubility product expression is: $K_{sp} = [Ag^+]^2 [CO_3^{2-}]$
Substituting the values: $4 	imes 10^{-13} = (2s)^2 	imes (0.1)$
$4 	imes 10^{-13} = 4s^2 	imes 0.1$
$s^2 = \frac{4 	imes 10^{-13}}{4 	imes 10^{-1}} = 10^{-12}$
$s = 10^{-6} \ M$

What is the molar solubility of $Ag_2CO_3$ $(K_{sp} = 4 \times 10^{-13})$ in $0.1 \ M \ Na_2CO_3$ solution?

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