Calculate the concentration of an aqueous solution of a non-electrolyte at $300 \ K$ if its osmotic pressure is $12 \ atm$. $\left[R = 0.0821 \ atm \ dm^3 \ K^{-1} \ mol^{-1}\right]$ (in $M$)

$A$ solution contains a non-volatile solute of molecular mass $M_p$. Which of the following can be used to calculate the molecular mass of the solute in terms of osmotic pressure ($m = \text{Mass of solute}$,$V = \text{Volume of solution}$,and $\pi = \text{Osmotic pressure}$)?

The value of osmotic pressure of a $0.2 \ M$ aqueous solution at $293 \ K$ is ........... $atm$.

Which one has the highest osmotic pressure?

Assuming complete ionisation,arrange the following solutions in order of increasing osmotic pressure.
$(a)$ $0.5 \ m \ Li_2SO_4$
$(b)$ $0.5 \ m \ KCl$
$(c)$ $0.5 \ m \ Al_2(SO_4)_3$
$(d)$ $0.1 \ m \ BaCl_2$

$300 \ mL$ of an aqueous solution of a protein contains $2.52 \ g$ of the protein. If the osmotic pressure of such a solution at $300 \ K$ is $5.04 \times 10^{-3} \ bar$,the molar mass of the protein in $g \ mol^{-1}$ is: