91Ó°ÊÓ

At standard atmospheric pressure, the boiling may be defined as the temperature at which the liquid is converted into vapours.

\({\bf{\Delta }}{{\bf{T}}_{\bf{b}}}{\bf{ = }}{{\bf{K}}_{\bf{b}}}{\bf{m}}\)

where,

\({{\bf{K}}_{\bf{b}}}\)= Base Dissociation Constant

m = Molality of the solute

\(\)

The molality of Ethylene Glycol = 17.9m

Calculate the change in boiling point:

\({\rm{\Delta }}{{\rm{T}}_{\rm{b}}}{\rm{ = }}{{\rm{K}}_{\rm{b}}}{\rm{m = 0}}{\rm{.52 \times 17}}{\rm{.9 = 9}}{\rm{.}}{{\rm{2}}^{\rm{o}}}{\rm{C}}\) \(\)

This adds a boiling point elevation to the boiling point of a pure solvent.

\({\rm{Boiling point temperature = 10}}{{\rm{0}}^{\rm{o}}}{\rm{C + 9}}{\rm{.}}{{\rm{2}}^{\rm{o}}}{\rm{C = 109}}{\rm{.}}{{\rm{2}}^{\rm{o}}}{\rm{C}}\)