Complete the explanation of why two solubility products cannot be compared directly.

For a 1:1 salt the solubility product equals s squared, but for an $\mathrm{A_2B}$ salt it equals 4s cubed. Because the two are different functions of the solubility, silver chromate can have the smaller constant while being the more soluble of the two.

For AgCl, $K_{sp} = s^2$; for $\mathrm{Ag_2CrO_4}$, $K_{sp} = 4s^3$. Cubing a small solubility pushes the constant far lower for the same amount dissolved, so only solubilities computed from the constants are comparable, never the constants themselves.