The osmotic pressure of $2.22\ \%\ (w/v)$ $CaCl_2$ solution at $27\ ^oC$ is $(R = 0.08\ L\ atm\ K^{-1}\ mol^{-1})$

Which of the following would have the highest osmotic pressure? (Assume that all salts are $90\%$ dissociated.)

Determine the osmotic pressure of a solution prepared by dissolving $25 \, mg$ of $K_{2}SO_{4}$ in $2 \, L$ of water at $25^{\circ} C$,assuming that it is completely dissociated.

Due to osmosis,the volume of the more dilute solution ...

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:

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