Calculate the mass of a non-volatile solute dissolved in $0.3 \text{ dm}^3$ of water, which has an osmotic pressure of $0.1 \text{ atm}$ at $300 \text{ K}$. [Molar mass of solute = $328 \text{ g mol}^{-1}$, $R = 0.082 \text{ dm}^3 \text{atm K}^{-1} \text{mol}^{-1}$] (in $\text{ g}$)

The osmotic pressure in atmospheres of a $10\%$ solution of cane sugar at $69\,^oC$ is:

The osmotic pressure of blood is $7.47 \, bar$ at $300 \, K$. To inject glucose to a patient intravenously,it has to be isotonic with blood. The concentration of glucose solution in $g \, L^{-1}$ is $......$ (Molar mass of glucose $= 180 \, g \, mol^{-1}$,$R = 0.083 \, L \, bar \, K^{-1} \, mol^{-1}$) (Nearest integer)

At a certain temperature,the osmotic pressure of a $0.25 \, M$ solution of a non-electrolyte is $\pi \, bar$. What will be the osmotic pressure of a $0.125 \, M \, Ba(NO_3)_2$ solution at the same temperature?

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

The osmotic pressure of equimolar solutions of $BaCl_2$,$NaCl$,and glucose follows the order: