The solubility of Ag_2C_2O_4 is 2 times 10^{- | vedclass

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(B) The dissociation of silver oxalate is given by: $Ag_2C_2O_{4(s)} \rightleftharpoons 2Ag^+{(aq)} + C_2O_4^{2-}{(aq)}$
Let the solubility be $S = 2

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$3.2 	imes 10^{-11}$

Vedclass · Answer

(B) The dissociation of silver oxalate is given by: $Ag_2C_2O_{4(s)} ightleftharpoons 2Ag^+{(aq)} + C_2O_4^{2-}{(aq)}$
Let the solubility be $S = 2 	imes 10^{-4} \ mol \ L^{-1}$.
Then,$[Ag^+] = 2S$ and $[C_2O_4^{2-}] = S$.
The solubility product expression is: $K_{sp} = [Ag^+]^2 [C_2O_4^{2-}]$
Substituting the values: $K_{sp} = (2S)^2 	imes (S) = 4S^3$
Calculating the value: $K_{sp} = 4 	imes (2 	imes 10^{-4})^3 = 4 	imes (8 	imes 10^{-12}) = 3.2 	imes 10^{-11}$

The solubility of $Ag_2C_2O_4$ is $2 \times 10^{-4} \ mol \ L^{-1}$ at $298 \ K$. What is its solubility product?

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