Question

At ${30}^0$C, the solubility of $A{g}_{2}C{O}_3(K_{sp}=8\times {10}^{-12}$ would be maximum in $1$ litre of:

• A. $0.05MN{a}_{2}C{O}_3$
• B. $0.05MAgN{O}_3$
• C. pure water
• D. $0.05MN{H}_3$

Answer 1

The correct option is D $0.05MN{H}_3$

In water the reaction will be $A{g}_{2}C{O}_3\rightleftharpoons 2A{g}^{+}+C{O}_3^{2-}$

In $N{H}_3$ the reaction will be $A{g}_{2}C{O}_3\rightleftharpoons 2A{g}^{+}+C{O}_3^{-2}$

$2A{g}^{+}+4N{H}_3\rightleftharpoons 2Ag(N{H}_3{)}_2$

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$A{g}_{2}C{O}_3+4N{H}_3⟶2Ag(N{H}_3{)}_2+C{O}_3^{2-}$

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Here a complex reaction is taking place due to this the formation of complex shifts the solubility equilibria in forward direction, which increases the solubility.

$\Rightarrow AgN{O}_3,N{a}_{2}C{O}_3$ causes common ion effect decreases the solubility.