The addition of a polar solvent to a solid electrolyte results in:

$A$ $0.001 \ molal$ 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:

Which one of the following electrolytes has the same value of van't Hoff factor $(i)$ as that of $Al_2(SO_4)_3$ (if all are $100 \%$ ionised)?

Which of the following solutions in water possesses the lowest vapour pressure?

$19.5 \ g$ of $CH_2FCOOH$ is dissolved in $500 \ g$ of water. The depression in the freezing point of water observed is $1.0 \ ^\circ C$. Calculate the van't Hoff factor and dissociation constant of fluoroacetic acid.

The $\Delta T_{b}$ value for $0.01 \ m$ $KCl$ solution is $0.01 \ K$. What is the Van't Hoff factor? $(K_{b}$ for water $= 0.52 \ K \ kg \ mol^{-1})$