Which of the following is a colligative property?

Which of the following sets of solutions of urea (mol. mass $60 \ g \ mol^{-1}$) and sucrose (mol. mass $342 \ g \ mol^{-1}$) is isotonic?

At a certain temperature,a $1.6 \%$ solution of an unknown substance is isotonic with a $2.4 \%$ solution of Urea. If both solutions have the same solvent and the same density of $1 \ g/cm^3$,what is the molecular mass of the unknown substance in $g/mol$? [Molecular mass of urea $= 60 \ g/mol$]

Which of the following pairs of solutions is isotonic? (Molar mass: urea $= 60 \ g \ mol^{-1}$,sucrose $= 342 \ g \ mol^{-1}$)

$20 \text{ g}$ hemoglobin in a $1 \text{ L}$ aqueous solution $(A)$ at $300 \text{ K}$ is separated from pure water by a semi-permeable membrane. At equilibrium, the height of the solution in a tube dipped in solution $(A)$ is found to be $80.0 \text{ mm}$ higher than the tube dipped in water. The molar mass of hemoglobin is . . . . . . $\text{kg mol}^{-1}$. (Nearest integer) (Given: $g = 10 \text{ m s}^{-2}$, $R = 8.3 \text{ kPa dm}^3 \text{ K}^{-1} \text{mol}^{-1}$, density of solution = $1000 \text{ kg m}^{-3}$)

The osmotic pressure of a urea solution at $10\,^oC$ is $500\, mm\, of\, Hg$. The solution is diluted such that the temperature increases to $25\,^oC$ and the osmotic pressure becomes $131.6\, mm\, of\, Hg$. By what factor has the solution been diluted?