Calculate the density of an aqueous solution of KI if its molarity and molality are $1.44M$ and $1.5molK{g}^{-1}$ respectively

We know,

$m=\frac{1000.M}{1000.d-M.M_B}$

$\Rightarrow d=\frac{1000.M+m.M.M_B}{1000.m}$

$=\frac{1000\times 1.44+1.5\times 1.44\times 166}{1000\times 1.5}$

$=1.1990=1.20g{L}^{-1}$

$m=molality=1.5molk{g}^{-1}$

$M=molarity=1.44mol{L}^{-1}$

$M_B=$ molar mass of KI

$=166gmo{l}^{-1}$

d = density of solution