The freezing point depression of a $0.01 \ m$ aqueous solution of $[Pt(NH_3)_4Cl_4]$ is $0.0054^\circ C$. If $K_f$ for water is $1.80 \ K \ kg \ mol^{-1}$,what is the correct formula for the complex?

Which of the following has the highest boiling point at $1 \, atm$ pressure?

If $0.004 \ M \ Na_2SO_4$ and $0.01 \ M$ glucose aqueous solutions are isotonic,then the degree of dissociation of $Na_2SO_4$ is ........ $\%$.

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: $K_f = 1.86 \ K \ kg \ mol^{-1}$)

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 ............. $mol$?

For a $0.1 \, molal$ aqueous solution of $2-$iodopropanoic acid,the degree of dissociation is $5 \%$. The freezing point of the solution will be ............ $^o C$.