Calculate the osmotic pressure of a $20\%$ (w/v) anhydrous $CaCl_2$ solution at $0^\circ C$. Assume $100\%$ ionization. (in $\text{atm}$)

The osmotic pressure of solutions of $PVC$ in cyclohexanone at $300 \ K$ are plotted on the graph. The molar mass of $PVC$ is $........ \ g \ mol^{-1}$ (Nearest integer) (Given : $R = 0.083 \ L \ atm \ K^{-1} \ mol^{-1}$ )

Which of the following pairs of aqueous solutions exhibits the same osmotic pressure at the same temperature? $\left[ \text{Molar mass of urea} = 60 \ g \ mol^{-1}, \text{sucrose} = 342 \ g \ mol^{-1} \right]$

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

One mole each of urea,glucose,and sodium chloride were dissolved in one litre of water. Equal osmotic pressure will be produced by solutions of

If $5\%$ sugar solution is isotonic with $1\%$ solution of unknown substance,then find out the molecular mass of the unknown substance. (in $g/mol$)