Solutions having the same osmotic pressure under a given set of conditions are known as

$A$ solution is prepared by dissolving $0.3 \ g$ of a non-volatile non-electrolyte solute '$A$' of molar mass $60 \ g \ mol^{-1}$ and $0.9 \ g$ of a non-volatile non-electrolyte solute '$B$' of molar mass $180 \ g \ mol^{-1}$ in $100 \ mL$ $H_2O$ at $27^{\circ}C$. Osmotic pressure of the solution will be
[Given: $R=0.082 \ L \ atm \ K^{-1} \ mol^{-1}$] (in $atm$)

$A$ solution of polystyrene in benzene contains $10 \, g/L$. The equilibrium height of the column of solution having density $0.9 \, g/mL$ in the osmometer is $11 \, cm$ at $27 \, ^\circ C$. What is the average molar mass of polystyrene? (Assume the solution is ideal)

$18 \ g$ glucose (Molar mass $= 180 \ g/mol$) is dissolved in $100 \ mL$ of water at $300 \ K$. If $R = 0.0821 \ L \ atm \ K^{-1} \ mol^{-1}$,what is the osmotic pressure of the solution (in $atm$)?

An aqueous solution has an osmotic pressure of $4.92 \text{ atm}$ at $300 \text{ K}$. Calculate the molarity of the solution. $(R = 0.082 \text{ L atm mol}^{-1} \text{ K}^{-1})$ (in $\text{ M}$)

The plot of osmotic pressure $(\Pi)$ vs concentration $\left(mol \ L^{-1}\right)$ for a solution gives a straight line with slope $25.73 \ L \ bar \ mol^{-1}$. The temperature at which the osmotic pressure measurement is done is
(Use $R=0.083 \ L \ bar \ mol^{-1} \ K^{-1}$) (in $^{\circ} C$)