What is the osmotic pressure of a solution prepared by dissolving $3 \ g$ of solute in $2 \ dm^3$ of water at $300 \ K$ (in $atm$)? (Molar mass of solute $= 60 \ g \ mol^{-1}$,$R = 0.0821 \ dm^3 \ atm \ K^{-1} \ mol^{-1}$)

Isotonic solutions have

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

$15 \%$ aqueous solution of glucose (molecular weight $= 180 \ g/mol$) is isotonic with $8 \%$ aqueous solution containing an unknown non-dissociable solute. What is the molecular weight of the unknown solute?

$20 \text{ g}$ 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 = $1000 \text{ kg m}^{-3}$)

Arrange the following equimolar solutions according to increasing order of osmotic pressure [Assume complete ionisation]:
$A$. $KCl$
$B$. $BaCl_2$
$C$. $AlCl_3$
$D$. $Al_2(SO_4)_3$