As a result of osmosis,what happens to the volume of the solution?

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.

What is the osmotic pressure (in $atm$) of $0.02 \ M$ aqueous glucose solution at $300 \ K$?
$(R=0.082 \ L \ atm \ mol^{-1} \ K^{-1})$

What will be the osmotic pressure of a $0.03 \ N$ solution of Aluminium sulphate at $27 \ ^\circ C$? If the salt dissociation in the solution is $90 \ \%$,the osmotic pressure is . . . . . . $atm$.

If $250 \ cm^3$ of an aqueous solution containing $0.73 \ g$ of a protein $A$ is isotonic with one litre of another aqueous solution containing $1.65 \ g$ of a protein $B,$ at $298 \ K,$ the ratio of the molecular masses of $A$ and $B$ is..........$\times 10^{-2}$ (to the nearest integer).

$A$ $5\% \, w/v$ solution of cane sugar is isotonic with a $1\% \, w/v$ solution of substance $X$. The molecular weight of $X$ is: