Osmotic pressure is $0.0821 \ atm$ at a temperature of $300 \ K$. Find the concentration in $mol/L$.

$A$ $1.17 \%$ solution of solute $A$ is isotonic with a $7.2 \%$ solution of glucose. If the molecular weight of solute $A$ is $58.5$, the value of the van't Hoff factor,'$i$',is:

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 $atm$)? $[R=0.082 \ dm^3 \ atm \ mol^{-1} \ K^{-1}]$

Find out the osmotic pressure of a $0.2 \, M$ solution of glucose at $300 \, K$. (in $, \text{atm}$)

$A$ solution containing $6.0 \ g$ of urea is isotonic with a solution containing $10 \ g$ of a non-electrolytic solute $X$. The molar mass of $X$ (in $g \ mol^{-1}$) is

At $27^{\circ} C$,the osmotic pressure of a solution containing $4 \ g$ of a non-electrolyte solute in $1.0 \ L$ of solution is $0.4 \ bar$. The molar mass of the solute in $g \ mol^{-1}$ is :
$(R=0.083 \ L \ bar \ K^{-1} \ mol^{-1})$