For a $0.25 \ m$ solution of $SrCl_2$,the van't Hoff factor is found to be $2.5$. What will be the effective molality of the solution in $m$?

The depression in freezing point of a $NaCl$ solution is $6 \ K$. If $K_f = 1.86 \ K \ kg \ mol^{-1}$ for water,then the amount of $NaCl$ dissolved in $1 \ kg$ of water is ............. $mol$?

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

When $0.01 \ mol$ of sodium sulphate $(Na_2SO_4)$ is dissolved in $1 \ kg$ of water,complete ionization of the solution is observed. Calculate the decrease in the freezing point of the solution. $(K_f = 1.86 \ K \ kg \ mol^{-1})$

For very dilute solutions of $BaCl_2$ $(t_1)$ and $KCl$ $(t_2)$ having the same molarity,what is the correct relationship between their boiling points?

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)