The K_{sp} of Ag_2CrO_4 is 1.1 times 10^{-12} | vedclass

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(B) The dissociation of $Ag_2CrO_4$ is given by: $Ag_2CrO_4(s) \rightleftharpoons 2Ag^{+}(aq) + CrO_4^{2-}(aq)$.In the presence of $0.1 \ M \ AgNO_3$,

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$(B) \ 1.1 	imes 10^{-10}$

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(B) The dissociation of $Ag_2CrO_4$ is given by: $Ag_2CrO_4(s) ightleftharpoons 2Ag^{+}(aq) + CrO_4^{2-}(aq)$.In the presence of $0.1 \ M \ AgNO_3$,the concentration of $Ag^{+}$ ions is dominated by the strong electrolyte $AgNO_3$,so $[Ag^{+}] \approx 0.1 \ M$.Let $s$ be the solubility of $Ag_2CrO_4$ in $mol/L$. Then $[CrO_4^{2-}] = s$.The solubility product expression is $K_{sp} = [Ag^{+}]^2 [CrO_4^{2-}]$.Substituting the values: $1.1 	imes 10^{-12} = (0.1)^2 	imes s$.$1.1 	imes 10^{-12} = 0.01 	imes s$.$s = \frac{1.1 	imes 10^{-12}}{0.01} = 1.1 	imes 10^{-10} \ mol/L$.

The $K_{sp}$ of $Ag_2CrO_4$ is $1.1 \times 10^{-12}$ at $298 \ K$. The solubility (in $mol/L$) of $Ag_2CrO_4$ in a $0.1 \ M \ AgNO_3$ solution is

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