A 1 molar aqueous solution of magnesium nitrate is $40 \%$ dissociated at 298 K . Calculate the osmotic pressure of the solution. $\left(R=0.0821 \mathrm{~L} \mathrm{~atm} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}\right)$

0.1 m of urea and 0.05 m of $\mathrm{CaCl}_2$ are dissolved separately in equal volumes of water. Which solution will have higher elevation in boiling point?

A dimolar solution potassium ferrocyanide is $ 50 \% $ dissociated at 300 K . The osmotic pressure of solution is $ \left(R=8.314 \mathrm{JK}^{-1} \mathrm{~mol}^{-1}\right) $

58.5 g of NaCl and 180 g of glucose were separately dissolved in 1000 mL of water. Identify the correct statement regarding the elevation of boiling point of the resulting solution.