## Chemistry and Chemical Reactivity (9th Edition)

a) $Ksp=[Ag^+][CN^-]=s^2$ $s=\sqrt{6\dot{}10^{-17}}=7.75\dot{}10^{-9}\ M$ b) $K=Ksp\dot{}Kf\rightarrow K=7.8\dot{}10^4$ Since the equilibrium constant is very large, the reaction is product favored, AgCN would dissolve in enough KCN. c) $K=Ksp(AgCN)\dot{}Kf(Ag(S_2O_3)_2^{3-})$ $K=1.74\dot{}10^{-3}$ Assuming constant $[S_2O_3^{2-}]$: $K=[Ag(S_2O_3)^{3-}][CN^-]/[S_2O_3^{2-}]^2$ $1.74\dot{}10^{-3}=s^2/0.10^2$ $s=4.18\dot{}10^{-3}\ M$