Seema Saini Solutions for Chapter: Solutions, Exercise 4: DPP 2.4

In which case, depression freezing point is equal to cryoscopic constant for water?

The amount of urea to be dissolved in $500 \mathrm{cc}$ of water $\left({\mathrm{K}}_{\mathrm{f}}\right.$$=1.86$ $)$ to produce a depression of $0.186°\mathrm{C}$ in the freezing point is:

Freezing point of an aqueous solution is $-0.186°\mathrm{C}$.  Elevation of boiling point of same solution would be $\left({\mathrm{K}}_{\mathrm{b}}=0.512\text{ and }{\mathrm{K}}_{\mathrm{f}}=1.86\mathrm{K}{\text{ molality }}^{-1}\right)$

The amount of ice that will separate on cooling a solution containing $50 \mathrm{g}$ of ethylene glycol in $200 \mathrm{g}$ water to $-9.3°\mathrm{C}$ is: $\left({\mathrm{K}}_{\mathrm{f}}=1.86 \mathrm{K}{\text{ molality }}^{-1}\right)$ is

What should be the freezing point of aqueous solution containing $17 \mathrm{g}$ of ${\mathrm{C}}_2{\mathrm{H}}_5\mathrm{OH}$ in $1000 \mathrm{g}$ of water $({\mathrm{K}}_{\mathrm{f}}$$=1.86 \mathrm{K} {\mathrm{m}}^{-1}$$)$?

The phase diagrams for a pure solvent (represented by the solid line) and a corresponding solution (containing a non-volatile solute and represented by the dashed lines) are shown below.

Choose the correct option.

Where ${\mathrm{T}}_{\mathrm{f}}, {\mathrm{T}}_{\mathrm{b}}$ and $\mathrm{m}$ stand for freezing point temperature, boiling point temperature and molality.

A solution of urea (mol mass $60 \mathrm{g} {\mathrm{mol}}^{-1}$) boils at $100.18°\mathrm{C}$ at atmospheric pressure. If ${\mathrm{K}}_{\mathrm{f}}$ and ${\mathrm{K}}_{\mathrm{b}}$ for water are $1.86 \mathrm{K} \mathrm{kg} {\mathrm{mol}}^{-1}$and $0.512 \mathrm{K} \mathrm{kg} {\mathrm{mol}}^{-1}$ respectively, the above solution will not freeze at:

Which of the following is/are not linked to the lowering of vapor pressure by a non-volatile solute?