The osmotic pressure of a solution increases,if:

$A$ solution containing $4 \ g$ of a non-volatile organic solute per $100 \ mL$ has an osmotic pressure of $500 \ cm$ of mercury at $27^\circ C$. What is the molar mass of the solute?

$A$ $1.17 \%$ 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:

Given below are two statements:
Statement $I$: $H_2O$ molecules move from the chamber $1$ to chamber $2$.
Statement $II$: The osmotic pressure of a solution prepared by dissolving $50 \text{ mg}$ of potassium sulphate (molar mass = $174 \text{ g/mol}$) in $2 \text{ L}$ of water (at $27^{\circ}C$) is $0.0107 \text{ bar}$. (Given: $R = 0.083 \text{ dm}^3 \text{ bar K}^{-1} \text{ mol}^{-1}$ and assume complete dissociation of electrolyte).
In the light of the above statements, choose the correct answer from the options given below:

Which method is most suitable to determine the molecular mass of a polymer?

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