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 $= 5.5 ^\circ C$)?

The normal freezing point $(f.p.)$ of nitrobenzene is $278.82 \ K$. If a non-volatile solute is dissolved in it and a solution of $0.25 \ molality$ is prepared,the observed freezing point of the solution is $276.82 \ K$. Evaluate the cryoscopic constant $(K_f)$ of nitrobenzene in $K \ kg \ mol^{-1}$.

$CaCl_2$ is preferred over $NaCl$ for clearing ice on roads,particularly in very cold countries. This is because:

$A$ camphor sample melts at $176^{\circ} C$. $K_f$ for camphor is $40 \ K \ kg \ mol^{-1}$. $A$ solution of $0.02 \ g$ of a hydrocarbon in $0.8 \ g$ of camphor melts at $156.77^{\circ} C$. The hydrocarbon is made up of $92.3 \%$ of carbon. What is the molecular formula of the hydrocarbon?

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

Which of the following $0.10 \ m$ aqueous solutions will have the lowest freezing point?