An aqueous solution has an osmotic pressure of $4.92 \text{ atm}$ at $300 \text{ K}$. Calculate the molarity of the solution. $(R = 0.082 \text{ L atm mol}^{-1} \text{ K}^{-1})$ (in $\text{ M}$)

What is the osmotic pressure of a solution of $1.7 \ g$ of $CaCl_2$ in $1.25 \ dm^3$ of water at $300 \ K$,if the van't Hoff factor and molar mass of $CaCl_2$ are $2.47$ and $111 \ g \ mol^{-1}$ respectively (in $atm$)? $[R=0.082 \ dm^3 \ atm \ mol^{-1} \ K^{-1}]$

The osmotic pressure of blood at $300 \ K$ is $8.21 \ atm$. What is the concentration of an aqueous glucose solution that is isotonic with this blood in $g \ L^{-1}$?

Arrange the following equimolar solutions according to increasing order of osmotic pressure [Assume complete ionisation]:
$A$. $KCl$
$B$. $BaCl_2$
$C$. $AlCl_3$
$D$. $Al_2(SO_4)_3$

What mass of solute (molar mass $58 \ g \ mol^{-1}$) is to be dissolved in $2.5 \ dm^3$ $H_2O$ to generate osmotic pressure of $0.245 \ atm$ at $300 \ K$ (in $g$)? $(R = 0.0821 \ dm^3 \ atm \ K^{-1} \ mol^{-1})$.

Find out the osmotic pressure of a $12 \% \ w/V$ $KCl$ solution at $27 \ ^oC$. (in $atm$)