Calculate the osmotic pressure of a $0.2 \ M$ aqueous solution of an electrolyte at $300 \ K$. If the van't Hoff factor is $1.6$,find the osmotic pressure. $\left[R=0.0821 \ atm \ dm^3 \ K^{-1} \ mol^{-1}\right]$ (in $atm$)

Consider separate solutions of $0.500 \, M \, C_2H_5OH \, (aq)$,$0.100 \, M \, Mg_3(PO_4)_2 \, (aq)$,$0.250 \, M \, KBr \, (aq)$ and $0.125 \, M \, Na_3PO_4 \, (aq)$ at $25 ^\circ C$. Which statement is true about these solutions,assuming all salts to be strong electrolytes?

$A$ 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 $atm$)

Calculate the osmotic pressure of a $0.2 \ M$ aqueous $KCl$ solution at $0^{\circ} C$ if the van't Hoff factor for $KCl$ is $1.83$. $[R = 0.082 \ dm^3 \ atm \ mol^{-1} \ K^{-1}]$ (in $atm$)

The osmotic pressure of a solution at $327^o C$ and concentration $C$ is $P$. The osmotic pressure of the same solution at $427^o C$ and concentration $C/2$ is $2$ bar. Then $P = ......$ bar.

$A$ solution is prepared by dissolving $0.6 \ g$ of urea (molar mass $= 60 \ g \ mol^{-1}$) and $1.8 \ g$ of glucose (molar mass $= 180 \ g \ mol^{-1}$) in $100 \ mL$ of water at $27 \ ^oC$. The osmotic pressure of the solution is : ............. $atm$ $(R = 0.08206 \ L \ atm \ K^{-1} \ mol^{-1})$