What is the boiling point of the antifreeze 17.9m Ethylene Glycol?

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.

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