At a temperature of $27\,^oC$,$0.6\,g$ of a solute is dissolved in $0.1\,L$ of solvent,resulting in an osmotic pressure of $1.23\,atm$. The molar mass of the solute is .......... $g\,mol^{-1}$.

$A$ solution has an osmotic pressure of $x \ kPa$ at $300 \ K$ having $1 \ mole$ of solute in $10.5 \ m^{3}$ of solution. If its osmotic pressure is reduced to $(\frac{1}{10})$th of its initial value,what is the new volume of solution (in $m^{3}$)?

Which of the following colligative properties is most suitable for determining the molar mass of polymers?

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 $\text{ g}$)

Equal masses of glucose,sucrose,and urea are dissolved in $V \ L$ of water to prepare separate solutions. The order of osmotic pressures $\pi_1, \pi_2$,and $\pi_3$ for glucose,sucrose,and urea respectively will be...........

The osmotic pressure of a solution containing $34.2 \ g$ of cane sugar (molar mass = $342 \ g \ mol^{-1}$) in $1 \ L$ of solution at $20^{\circ} C$ is
(Given,$R = 0.082 \ L \ atm \ K^{-1} \ mol^{-1}$) (in $atm$)