What is the molar solubility of Ag_{2}CO_{3} | vedclass

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(A) The dissociation of $Ag_{2}CO_{3}$ is given by: $Ag_{2}CO_{3(s)} \longleftrightarrow 2Ag^{+}_{(aq)} + C{O_{3}}^{2-}_{(aq)}$In the presence of $0.1

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$10^{-6}$

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(A) The dissociation of $Ag_{2}CO_{3}$ is given by: $Ag_{2}CO_{3(s)} \longleftrightarrow 2Ag^{+}_{(aq)} + C{O_{3}}^{2-}_{(aq)}$In the presence of $0.1 \ M \ Na_{2}CO_{3}$,the concentration of $CO_{3}^{2-}$ is dominated by the salt,so $[CO_{3}^{2-}] \approx 0.1 \ M$.Let $s$ be the molar solubility of $Ag_{2}CO_{3}$. Then $[Ag^{+}] = 2s$.The solubility product expression is $K_{sp} = [Ag^{+}]^{2} [CO_{3}^{2-}]$.Substituting the values: $4 	imes 10^{-13} = (2s)^{2} 	imes (0.1)$.$4 	imes 10^{-13} = 4s^{2} 	imes 0.1$.$10^{-13} = s^{2} 	imes 10^{-1}$.$s^{2} = 10^{-12}$.$s = 10^{-6} \ M$.

What is the molar solubility of $Ag_{2}CO_{3}$ $(K_{sp} = 4 \times 10^{-13})$ in $0.1 \ M \ Na_{2}CO_{3}$ solution?

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