Concentration of the Ag^{+} ions in a saturat | vedclass

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(C) The dissociation of $Ag_2C_2O_4$ is given by: $Ag_2C_2O_4(s) ightleftharpoons 2Ag^{+}(aq) + C_2O_4^{2-}(aq)$.Given $[Ag^{+}] = 2.2 	imes 10^{-4

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$5.3 	imes 10^{-12}$

Vedclass · Answer

(C) The dissociation of $Ag_2C_2O_4$ is given by: $Ag_2C_2O_4(s) ightleftharpoons 2Ag^{+}(aq) + C_2O_4^{2-}(aq)$.Given $[Ag^{+}] = 2.2 	imes 10^{-4} \ mol \ L^{-1}$.From the stoichiometry,$[C_2O_4^{2-}] = \frac{1}{2} [Ag^{+}] = \frac{2.2 	imes 10^{-4}}{2} = 1.1 	imes 10^{-4} \ mol \ L^{-1}$.The solubility product $K_{sp}$ is defined as: $K_{sp} = [Ag^{+}]^2 [C_2O_4^{2-}]$.Substituting the values: $K_{sp} = (2.2 	imes 10^{-4})^2 	imes (1.1 	imes 10^{-4})$.$K_{sp} = (4.84 	imes 10^{-8}) 	imes (1.1 	imes 10^{-4}) = 5.324 	imes 10^{-12} \approx 5.3 	imes 10^{-12}$.

Concentration of the $Ag^{+}$ ions in a saturated solution of $Ag_2C_2O_4$ is $2.2 \times 10^{-4} \ mol \ L^{-1}.$ Solubility product of $Ag_2C_2O_4$ is

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