$A$ $0.0020 \ m$ aqueous solution of an ionic compound $[Co(NH_3)_5(NO_2)]Cl$ freezes at $-0.00732 \ ^oC.$ Number of moles of ions which $1 \ mol$ of ionic compound produces on being dissolved in water will be
$(K_f = 1.86 \ ^oC/m)$

$0.2 \ molal$ aqueous solution of an electrolyte $A_3B$ is $90\%$ ionised. The boiling point of the solution at $1 \ atm$ is ........ $K.$ ($K_b$ for $H_2O = 0.52 \ K \ Kg \ mol^{-1}$ and $B.pt.$ of $H_2O = 373 \ K$)

$17.4\%\, (w/v)$ $K_2SO_4$ $(Mw=174\, g/mol)$ solution at $27\, ^\circ C$ is isotonic to $4\%\, (w/v)\, NaOH$ solution at the same temperature. If $NaOH$ is $100\%$ ionized,what is the $\%$ ionization of $K_2SO_4$ in aqueous solution .......... $\%$.

For a $0.01 \ m$ aqueous solution of $K_4[Fe(CN)_6]$,if $K_b = 0.52 \ K \ kg \ mol^{-1}$ for the solvent,then its boiling point will be ..... $^\circ C$.

Which of the following has the lowest freezing point?

The interionic attraction depends on the interaction of: