$A$ $0.001 \ molal$ 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:

$K_2HgI_4$ is $40 \%$ ionized in aqueous solution. The value of its van't Hoff factor $(i)$ is:

Which of the following solutions exhibits the minimum boiling point elevation under identical conditions? (Assume complete dissociation)

$2 \ m$ aqueous solution of an electrolyte $X_3Y_2$ is $25\%$ ionized. The boiling point of the solution is .......... $K.$ ($K_b$ for $H_2O = 0.52 \ K \ kg/mol$)

Which of the following solutions will have the highest boiling point?

If sodium sulfate $(Na_2SO_4)$ undergoes complete dissociation into its constituent ions in an aqueous solution,what will be the depression in freezing point $(\Delta T_f)$ when $0.01 \ mol$ of sodium sulfate is dissolved in $1 \ kg$ of water (in $K$)? (Given: $K_f = 1.86 \ K \ kg \ mol^{-1}$)