Which of the following pairs of solutions is expected to be isotonic at the same temperature?

$A$ solution containing $4 \ g$ of polymer in $4.0 \ L$ solution at $27^{\circ} C$ shows an osmotic pressure of $3.0 \times 10^{-4} \ atm$. The molar mass of the polymer in $g \ mol^{-1}$ is

The osmotic pressure of a solution containing $3 \ g$ of glucose (molar mass = $180 \ g/mol$) in $60 \ g$ of water at $15^\circ C$ (density = $1 \ g/mL$) is ....... $atm$.

$A$ $0.6\%$ solution of urea (molecular weight $= 60$) would be isotonic with

Calculate the mass of a non-volatile solute dissolved in $0.3 \text{ dm}^3$ of water, which has an osmotic pressure of $0.1 \text{ atm}$ at $300 \text{ K}$. [Molar mass of solute = $328 \text{ g mol}^{-1}$, $R = 0.082 \text{ dm}^3 \text{atm K}^{-1} \text{mol}^{-1}$] (in $\text{ g}$)

Arrange the following solutions according to decreasing order of osmotic pressure under similar conditions of temperature,assuming complete dissociation:
$A. 0.2 \ m \ KCl$
$B. 0.3 \ m \ MgSO_4$
$C. 0.1 \ m \ BaCl_2$
$D. 0.5 \ m \ Al_2(SO_4)_3$