If the $K_f$ value of $H_2O$ is $1.86 \ K \ kg \ mol^{-1}$,the value of $\Delta T_f$ for a $0.1 \ m$ solution of a non-volatile solute is:

$31 \ g$ of ethylene glycol $(C_2H_6O_2)$ is dissolved in $600 \ g$ of water. The freezing point depression of the solution is ($K_f$ for water is $1.86 \ K \ kg \ mol^{-1}$) (in $K$)

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 should be the freezing point of an aqueous solution containing $17 \ g$ of $C_2H_5OH$ in $1000 \ g$ of water? (Given: $K_f$ of water = $1.86 \ K \ kg \ mol^{-1}$)

$1.00 \ g$ 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 .......... $K$.

Calculate the molar mass of a nonvolatile solute when $1.5 \ g$ of it is dissolved in $90 \ g$ of solvent,decreasing its freezing point by $0.25 \ K$. Given: $K_{f} = 1.2 \ K \ kg \ mol^{-1}$.