$A$ solution is made by dissolving $20 \ g$ of a substance in $500 \ mL$ of water. Its osmotic pressure was found to be $600 \ mm$ of $Hg$ at $15 \ ^oC$. The molecular weight of the substance is

$20 \text{ g}$ 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 blood at $300 \ K$ is $8.21 \ atm$. What is the concentration of an aqueous glucose solution that is isotonic with this blood in $g \ L^{-1}$?

The osmotic pressure of a decinormal solution of $BaCl_2$ in water is

What is the concentration (in $g/L$) of a sugar solution $(mol. wt. = 342 \, g/mol)$ that is isotonic with a $6 \, g/L$ urea solution $(mol. wt. = 60 \, g/mol)$?

Calculate the osmotic pressure of a $0.1 \ M$ aqueous solution of an electrolyte at $300 \ K$ if the van't Hoff factor is $1.125$. $[R = 0.0821 \ atm \ dm^3 \ K^{-1} \ mol^{-1}]$ (in $atm$)