Which among the following colligative properties is useful to determine molar masses of very expensive solutes?

At $298 \, K$,the ratio of osmotic pressures of two solutions of a substance with concentrations of $0.01 \, M$ and $0.001 \, M$ respectively,is

When the pure solvent diffuses out of the solution through the semi-permeable membrane,then the process is called:

The following solutions were prepared by dissolving $10 \ g$ of glucose $(C_{6}H_{12}O_{6})$ in $250 \ mL$ of water $(P_{1})$,$10 \ g$ of urea $(CH_{4}N_{2}O)$ in $250 \ mL$ of water $(P_{2})$,and $10 \ g$ of sucrose $(C_{12}H_{22}O_{11})$ in $250 \ mL$ of water $(P_{3})$. The right option for the decreasing order of osmotic pressure of these solutions is:

$50 \ mL$ of $0.2$ molal urea solution (density $= 1.012 \ g \ mL^{-1}$ at $300 \ K$) is mixed with $250 \ mL$ of a solution containing $0.06 \ g$ of urea. Both the solutions were prepared in the same solvent. The osmotic pressure (in Torr) of the resulting solution at $300 \ K$ is . . . . . $[\Delta_{mix} V = 0]$

Determine the osmotic pressure of a solution prepared by dissolving $25 \, mg$ of $K_{2}SO_{4}$ in $2 \, L$ of water at $25^{\circ} C$,assuming that it is completely dissociated.