$0.440 \ g$ of a substance dissolved in $22.2 \ g$ of benzene lowered the freezing point of benzene by $0.567 \ ^oC$. Calculate the molecular mass of the substance. (Given: $K_f = 5.12 \ ^oC \ kg \ mol^{-1}$)

What happens to the freezing point of benzene when a small quantity of naphthalene is added to it?

$1.00 \ g$ of a non-electrolyte solute (molar mass $250 \ g \ mol^{-1}$) was dissolved in $51.2 \ g$ of benzene. If the freezing point depression constant,$K_f$ of benzene is $5.12 \ K \ kg \ mol^{-1},$ the freezing point of benzene will be lowered by .......... $K$.

Ethylene glycol is used as an antifreeze in cold climates. The mass of ethylene glycol $(C_2H_6O_2)$ that should be added to $4 \ kg$ of water to prevent it from freezing at $-6 \ ^oC$ is ......... $g$.
($K_f$ for water $= 1.86 \ K \ kg \ mol^{-1}$,and molar mass of ethylene glycol $= 62 \ g \ mol^{-1}$)

$K_f$ for water is $1.86 \, K \, kg \, mol^{-1}$. If your automobile radiator holds $1.0 \, kg$ of water,how many $gm$ of ethylene glycol $(C_2H_6O_2)$ must you add to lower the freezing point of the solution to $-2.8 \, ^oC$?

At the freezing point of a solution containing a nonvolatile solute,which of the following are in equilibrium?