When a solute is dissolved in a solvent,the freezing point decreases by $0.184 \ ^oC$. What will be the molality of the solution? (Given $K_f = 18.4 \ K \ kg \ mol^{-1}$)

What will be the freezing point of a $1\%$ aqueous solution of $Ca(NO_3)_2$?

Find the freezing point depression of a solution having molality $0.25 \ mol \ kg^{-1}$. $(K_{f} = 4.0 \ K \ kg \ mol^{-1})$ (in $K$)

Calculate the molal freezing point depression constant $(K_f)$ of a solvent which has a freezing point of $16.6 \, ^\circ C$ and a latent heat of fusion of $180.75 \, J/g$.

Which of the following solutions has the maximum freezing point?

$A$ solution containing $7.5 \ g$ of urea (molar mass $= 60 \ g \ mol^{-1}$) in $1 \ kg$ of water freezes at the same temperature as another solution containing $15 \ g$ of solute $X$,in the same amount of water. The molar mass of $X \ (g \ mol^{-1})$ is