Depression in Freezing Point of the Solvent

Assertion: Sodium chloride is used to clear snow on the roads.

Reason :Sodium chloride depresses the freezing point of water.

Give some examples of anti-freezing agents.

What are anti-freezing agents?

Which of the following statements is false?

$31 \mathrm{g}$ of an unknown molecular material is dissolved in $500 \mathrm{g}$ of water. The resulting solution freezes at $271.14 \mathrm{K}$. Calculate molar mass of the material in ${\mathrm{gmol}}^{-1}$.(${\mathrm{K}}_{{\mathrm{f}}_{{\mathrm{H}}_2\mathrm{O}}} = 1.86 \mathrm{K} \mathrm{kg} {\mathrm{mol}}^{-1} , {\mathrm{T}}^{\mathrm{o}}{\mathrm{f}}_{{\mathrm{H}}_2\mathrm{O}}= 273\mathrm{K}$)

Which is the correct relationship between molal depression constant and enthalpy of fusion ?

$1.00 \mathrm{g}$ of a non-electrolyte solute dissolved in $50 \mathrm{g}$ of benzene lowered the freezing point of benzene by $0.40 \mathrm{K}$. The freezing point depression constant of benzene is $5.12 \mathrm{K}$ $\mathrm{kg} {\mathrm{mol}}^{-1}$. Find the molar mass of the solute.

The observed depression in freezing point of water for a particular solution is $0.093 \mathrm{K}$. Calculate the concentration of the solution in molality. Given that molal depression constant for water is $1.86 \mathrm{K} \mathrm{kg} {\mathrm{mol}}^{-1}$. (Write only numerical value and round upto two decimal places)

Define molal depression constant. How is it related to enthalpy of fusion?

Which of the following will have maximum depression in freezing point?

How molar mass of a non-volatile solute is related to the depression in freezing point? Derive an equation.

What causes depression in freezing point?

Calculate the temperature at which the solution (of $54 \mathrm{g}$ glucose in $250 \mathrm{g}$ water) freezes. $\left(K_f= 1.86 \mathrm{K} \mathrm{Kg} {\mathrm{mol}}^{-1}\right)$.

Which of the following solutions contains the maximum freezing point?

If sodium sulphate is considered to be completely dissociated into cations and anions in aqueous solution, the change in freezing point of water $\left(\Delta T_f\right)$ , when $0.01$ mole of sodium sulphate is dissolved in $1 kg$  of water is $(K_f=1.86 K-kg/mol)$

$25 \mathrm{mL}$ of an aqueous solution of $\mathrm{KCl}$ was found to require $20 \mathrm{mL} \mathrm{of} 1.0 \mathrm{M} {\mathrm{AgNO}}_3$ solution when titrated, using a ${\mathrm{K}}_2{\mathrm{CrO}}_4$ as indicator. The depression in freezing point of $\mathrm{KCl}$ solution with $100\%$ ionization will be:

$[{\mathrm{K}}_{\mathrm{f}}=2.0{\mathrm{mol}}^{-1}\mathrm{kg}$and molarity$=$molality$]$