Blood cells will remain as such in

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 $atm$)

$90 \, g$ of $CH_3COOH$ $(i = 0.5)$ is dissolved in $110 \, g$ of benzene. What will be its osmotic pressure at $300 \, K$ if the density of the solution is $1.2 \, g/mL$? (Answer in $atm$)

At $300 \, K$,$36 \, g$ of glucose present in a litre of its solution has an osmotic pressure of $4.98 \, bar$. If the osmotic pressure of the solution is $1.52 \, bar$ at the same temperature,what would be its concentration?

The osmotic pressure of a solution at $327^o C$ and concentration $C$ is $P$. The osmotic pressure of the same solution at $427^o C$ and concentration $C/2$ is $2$ bar. Then $P = ......$ bar.

Identify the correct statement regarding $0.2 \text{ M}$ urea and $0.2 \text{ M}$ sucrose solutions.