## Chemistry and Chemical Reactivity (9th Edition)

a) $1.34\dot{}10^{-5}\ M$ b) $4.45\dot{}10^{-2}\ M$
a) $Ksp=[Ag^+][Cl^-]=s^2$ $s=\sqrt{1.8\dot{}10^{-10}}=1.34\dot{}10^{-5}\ M$ b) $Knet=Kf\dot{}Ksp=[Ag(NH_3)_2^+][Cl^-]/[NH_3]^2$ Assuming constant [NH3]: $1.98\dot{}10^{-3}=s^2/1.0^2$ $s=4.45\dot{}10^{-2}\ M$