Calculate the osmotic pressure of a $0.2 \ M$ aqueous $KCl$ solution at $0^{\circ} C$ if the van't Hoff factor for $KCl$ is $1.83$. $[R = 0.082 \ dm^3 \ atm \ mol^{-1} \ K^{-1}]$ (in $atm$)

Calculate the molar mass of a non-electrolyte solute when $6 \text{ g}$ of it is dissolved in $1 \text{ dm}^3$ of water, having an osmotic pressure of $2.4 \text{ atm}$ at $300 \text{ K}$ $(R = 0.0821 \text{ atm dm}^3 \text{ K}^{-1} \text{ mol}^{-1})$.

$A$ solution containing $8.6 \ g$ of urea per liter is isotonic with a $0.5 \ \%$ (weight/volume) solution of a non-volatile organic solute. What is the molecular weight of the organic solute?

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?

If a $6.84 \% (wt./vol.)$ solution of cane sugar $(mol. wt. 342)$ is isotonic with a $1.52 \% (wt./vol.)$ solution of thiocarbamide,then the molecular weight of thiocarbamide is:

At $300 \ K$,$6 \ g$ of urea was dissolved in $500 \ mL$ of water. What is the osmotic pressure (in $atm$) of the resultant solution? $(R=0.082 \ L \ atm \ K^{-1} \ mol^{-1})$ $(C=12; N=14; O=16; H=1)$