What will be the osmotic pressure in $atm$ of a $0.2 \ M$ $K_4[Fe(CN)_6]$ solution at $27 \ ^oC$?

Which of the following solutions has the lowest freezing point?

The freezing point of an equimolal aqueous solution will be highest for:

The osmotic pressure $(O.P.)$ of equimolar solutions of $Urea$,$BaCl_2$,and $AlCl_3$ will be in the order:

$A^{2+}$,$B^{2+}$ and $C^{-}$ form an ionic complex like $A_{x-2}[B(C)_x]_2$. If the complex is $75 \%$ dissociated in a solvent with $i=4$,the coordination number of $B$ is:

At a constant temperature,the vapor pressures of aqueous solutions of $Na_2SO_4$,urea,$AlCl_3$,and $1.2 \, m \, KCl$ are approximately equal. The molalities of the aqueous solutions of $Na_2SO_4$,urea,and $AlCl_3$ are,respectively: (Assume $100 \%$ dissociation of the solute)