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 $atm$)

Which of the following $0.1 \ M$ solutions has the maximum osmotic pressure at $25^o \ C$?

If $3 \ g$ of glucose (molar mass $= 180 \ g \ mol^{-1}$) is dissolved in $60 \ g$ of water at $15^{\circ} C$,the osmotic pressure of the solution will be (in $atm$)

$200 \ mL$ 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 ......... $g \ mol^{-1}$.
$(R = 0.083 \ L \ bar \ mol^{-1} \ K^{-1})$

. . . . . . solution is hypertonic with reference to fluid inside the blood cell.

To have an osmotic pressure equal to a solution containing $9.2 \ g$ of glucose per liter,how many grams of glucose must be dissolved in $0.5 \ L$ of solution?