## Chemistry and Chemical Reactivity (9th Edition)

a) $AgCl$ b) $Ca(OH)_2$ c) $Ca(OH)_2$
a) $Ksp=[Ag^+][Cl^-]=s^2$, $Ksp=[Ag^+][CN^-]=s^2$ AgCl is more soluble in water because it has a higher Ksp b) $Ksp=[Mg^{2+}][OH^-]^2=s\dot{}(2s)^2=4s^3$, $Ksp=[Ca^{2+}][OH^-]^2=s\dot{}(2s)^2=4s^3$ $Ca(OH)_2$ is more soluble in water because it has a higher Ksp c) $Ksp=[Ca^{2+}][OH^-]^2=s\dot{}(2s)^2=4s^3\rightarrow s=0.024\ M$, $Ksp=[Ca^{2+}][SO_4^{2-}]=s^2\rightarrow s=0.007\ M$ $Ca(OH)_2$ has a higher solubility in water.