The osmotic pressure of a solution at $327\,^oC$ and concentration $C$ is $P$. If the osmotic pressure of the same solution at concentration $C/2$ and temperature $427\,^oC$ is $2\, atm$,then the value of $P$ is:

$200 \ mL$ of an aqueous solution of a protein contains its $1.26 \ g$. The osmotic pressure of this solution at $300 \ K$ is found to be $2.57 \times 10^{-3} \ bar$. The molar mass of protein will be ......... $g \ mol^{-1}$.
$(R = 0.083 \ L \ bar \ mol^{-1} \ K^{-1})$

$A$ $5\%(w/v)$ solution of sucrose is isotonic with a $1\%(w/v)$ solution of substance '$A$'. What is the molar mass of substance '$A$'?

Which of the following pairs of solutions is isotonic?

Assuming complete ionisation,arrange the following solutions in order of increasing osmotic pressure.
$(a)$ $0.5 \ m \ Li_2SO_4$
$(b)$ $0.5 \ m \ KCl$
$(c)$ $0.5 \ m \ Al_2(SO_4)_3$
$(d)$ $0.1 \ m \ BaCl_2$

When $10 \ g$ of glucose (osmotic pressure $P_1$),$10 \ g$ of urea (osmotic pressure $P_2$),and $10 \ g$ of sucrose (osmotic pressure $P_3$) are dissolved in $250 \ mL$ of water,the correct relationship between the osmotic pressures of these solutions is: