In an aqueous solution of potassium ferrocyanide,the degree of dissociation of the salt is $80\%$. The value of the van't Hoff factor is:

If $1$ mole of a solute dissociates to give $n$ number of ions,then the degree of dissociation $\alpha$ in terms of the van't Hoff factor $i$ is given by:

Calculate the amount of $KCl$ $(M_w = 74.5 \ g \ mol^{-1})$ in grams required to depress the freezing point of $1000 \ g$ of water by $2 \ K$. (Given: $K_f = 1.86 \ K \ kg \ mol^{-1}$) (in $.0$)

$A$ $0.001 \ molal$ solution of $[Pt(NH_3)_4Cl_4]$ in water has a freezing point depression of $0.0054 \ ^oC$. If $K_f$ for water is $1.80 \ K \ kg \ mol^{-1}$,the correct formulation for the above complex is:

$2.0 \, m \, CH_3COOH$ undergoes $100 \%$ dimerization in benzene. It will be isotonic with which of the following?

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?