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

For MY,
$\underset{0}{\mathrm{MY}}\iff \underset{s}{M^{+}}+\underset{s}{Y^{-}}$
where, s = solubility and $K_{sp}$ = solubility product.
$\therefore K_{sp}=\left[M^{+}\right]\left[Y^{-}\right]$
$K_{sp}=s^2$
$s=\sqrt{K_{sp}}=\sqrt{6.2\times {10}^{-13}}=7.874\times {10}^{-7}$
Similarly, for $N{Y}_3$,
$\underset{0}{N{Y}_3}\iff \underset{s}{N^{+}}+\underset{3s}{3Y^{-}}$
$\therefore K_{sp}=\left[N^{+}\right]{\left[Y^{-}\right]}^3=s\times {\left(3s\right)}^3$
$K_{sp}=27s^4$
$\therefore s=\sqrt[4]{\frac{K_{sp}}{27}}=\sqrt[4]{\frac{6.2\times {10}^{-13}}{27}}=3.89\times {10}^{-4}$
Therefore, molar solubility of MY in water is less than that of $N{Y}_3$.