Calculate the molality of a solution if its depression in freezing point is $0.18 \ K$. $[K_f = 1.6 \ K \ kg \ mol^{-1}]$ (in $m$)

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 $180.75 \, J/g$.

The freezing point of a $4 \%$ by weight aqueous solution of $A$ is equal to the freezing point of a $10 \%$ by weight aqueous solution of $B$. If the molecular weight of $A$ is $60$,then the molecular weight of $B$ is:

The freezing point of a solution containing $4.8 \ g$ of a compound in $60 \ g$ of benzene is $4.48 ^\circ C$. What is the molar mass of the compound $(K_f = 5.1 \ K \ kg \ mol^{-1})$,(freezing point of benzene $= 5.5 ^\circ C$)?

Which of the following aqueous molal solutions has the highest freezing point?

How much amount of $NaCl$ should be added to $600 \ g$ of water $(\rho=1.00 \ g / mL)$ to decrease the freezing point of water to $-0.2^{\circ} C ?$ ............. $gm$
(The freezing point depression constant for water $=2 \ K \ kg \ mol^{-1}$ )