Depression in Freezing Point of the Solvent

Assertion: Camphor is usually used in molecular mass determination.

Reason: Camphor has low cryoscopic constant and therefore, causes greater depression in freezing point.

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

Reason :Sodium chloride depresses the freezing point of water.

Calculate the molal depression constant of a solution, which freezes at $15°\mathrm{C}$. The latent heat of fusion is $180.7{\mathrm{Jg}}^{-1}$

$2 \mathrm{g}$ of a non-electrolyte solute (molar mass is $500 \mathrm{g}{ \mathrm{mol}}^{-1}$ ) was dissolved in$57.3 \mathrm{g}$ of xylene. If the freezing point depression constant ${\mathrm{K}}_{\mathrm{f}}$ of Xylene is $4.3 \mathrm{K} \mathrm{kg}{ \mathrm{mol}}^{-1}$. Then the depression in freezing point of Xylene is

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

Round off your answer to the nearest integer after multiplying with 10.

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 ${\mathrm{gmol}}^{-1}$.(${\mathrm{K}}_{{\mathrm{f}}_{{\mathrm{H}}_2\mathrm{O}}} = 1.86 \mathrm{K} \mathrm{kg} {\mathrm{mol}}^{-1} , {\mathrm{T}}^{\mathrm{o}}{\mathrm{f}}_{{\mathrm{H}}_2\mathrm{O}}= 273\mathrm{K}$)

The depression in freezing point of $0.01 \mathrm{m}$ aqueous solution of urea, sodium chloride and sodium sulphate is in the ratio :

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. $\left(K_f= 1.86 \mathrm{K} \mathrm{Kg} {\mathrm{mol}}^{-1}\right)$.

It is seen that sprinkling of salt helps in clearing the snow covered roads in hills. What is the phenomenon involved in the process?

Same amount of the following complexes $\mathrm{I},\mathrm{ }\mathrm{II},\mathrm{ }\mathrm{III}$ is used to prepare three different solutions by dissolving in water. The correct order of freezing points will be :

$\mathrm{I}.\mathrm{ }\left[\mathrm{Co}{\left({\mathrm{NH}}_3\right)}_3{\left({\mathrm{NO}}_2\right)}_3\right]$

$\mathrm{II}.\left[\mathrm{Co}{\left({\mathrm{NH}}_3\right)}_5\left({\mathrm{NO}}_2\right)\right]{\left[\mathrm{Co}{\left({\mathrm{NH}}_3\right)}_2{\left({\mathrm{NO}}_2\right)}_4\right]}_2$

$\mathrm{III}.\mathrm{ }\left[\mathrm{Co}{\left({\mathrm{NH}}_3\right)}_4{\left({\mathrm{NO}}_2\right)}_2\right]\left[\mathrm{Co}{\left({\mathrm{NH}}_3\right)}_2{\left({\mathrm{NO}}_2\right)}_4\right]$

[Given: ${\mathrm{K}}_{\mathrm{f}}\left({\mathrm{H}}_2\mathrm{O}\right)=1{.86}^{\mathrm{o}}\mathrm{C}/\mathrm{m}$ ]

Find out the amount of water (in g) separated as ice, if a solution containing $62 \mathrm{g}$ ethylene glycol in $250 \mathrm{g}$ water is cooled to $-{10}^{° }\mathrm{C}$ . ${\mathrm{K}}_{\mathrm{f}}$ for water is $1.86 \mathrm{K}\mathrm{ }\mathrm{kg}\mathrm{ }{\mathrm{mol}}^{-1}$ .

Among the following, which solution has lowest freezing point?