$\mathrm{MY} \mathrm{and} {\mathrm{NY}}_3$, two nearly insoluble salts, have the same ${\mathrm{K}}_{\mathrm{sp}}$ values of $6.2\times {10}^{-13}$ at room temperature. Which statement would be true in regard to $\mathrm{MY} \mathrm{and} {\mathrm{NY}}_3$ ?

For MY:${\mathrm{K}}_{\mathrm{sp}}={\mathrm{s}}_1^2$

$\Rightarrow {\mathrm{s}}_1=\sqrt{{\mathrm{K}}_{\mathrm{sp}}}=\sqrt{6.2\times {10}^{-13}}=7.87\times {10}^{-7} \mathrm{mol}{ \mathrm{L}}^{-1}$

For ${\mathrm{NY}}_3$:${\mathrm{K}}_{\mathrm{sp}}=27{\mathrm{s}}_2^4\Rightarrow {\mathrm{s}}_2=\sqrt[4]{\frac{6.2\times {10}^{-13}}{27}}$

$\Rightarrow {\mathrm{s}}_2=3.89\times {10}^{-4} \mathrm{mol}{ \mathrm{L}}^{-1}$

$\mathrm{Hence}, \mathrm{molar} \mathrm{solubility} \mathrm{of} \mathrm{MY} \mathrm{in} \mathrm{water} \mathrm{is} \mathrm{less} \mathrm{than} \mathrm{that} \mathrm{of} {\mathrm{NY}}_3$.