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

If the freezing point of a $0.01 \ m$ aqueous solution of a cobalt $(III)$ chloride-ammonia complex (which behaves as a strong electrolyte) is $-0.0558^{\circ} C$,the number of chloride $(Cl^-)$ ions in the coordination sphere of the complex is.
$\left[ K_{f} \text{ of water } = 1.86 \ K \ kg \ mol^{-1} \right]$

We have three aqueous solutions of $NaCl$ labelled as '$A$','$B$' and '$C$' with concentrations $0.1 \ M$,$0.01 \ M$,and $0.001 \ M$ respectively. The value of the Van't Hoff factor for these solutions will be in the order . . . . . . .

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

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:

An aqueous solution is prepared by dissolving $0.1 \ mol$ of an ionic salt in $1.8 \ kg$ of water at $35^{\circ} C$. The salt remains $90 \%$ dissociated in the solution. The vapour pressure of the solution is $59.724 \ mm \ Hg$. Vapor pressure of water at $35^{\circ} C$ is $60.000 \ mm \ Hg$. The number of ions present per formula unit of the ionic salt is . . . . . .