Answer : The boiling point of the solution is [tex]101.4^oC[/tex]
Explanation :
Formula used for Elevation in boiling point :
[tex]\Delta T_b=i\times k_b\times m[/tex]
or,
[tex]T_b-T^o_b=i\times k_b\times \frac{n_2}{w_1}[/tex]
where,
[tex]T_b[/tex] = boiling point of solution = ?
[tex]T^o_b[/tex] = boiling point of water = [tex]100^oC[/tex]
[tex]k_b[/tex] = boiling point constant  of water = [tex]1.86^oC/m[/tex]
m = molality
i = Van't Hoff factor = 1 (for non-electrolyte)
[tex]n_2[/tex] = moles of solute (ethylene glycol) = 0.75 mole
[tex]w_1[/tex] = mass of solvent (water) = 1 kg
Now put all the given values in the above formula, we get:
[tex](T_b-100)^oC=1\times (1.86^oC/m)\times \frac{0.75mole}{1kg}[/tex]
[tex]T_b=101.4^oC[/tex]
Therefore, the boiling point of the solution is [tex]101.4^oC[/tex]
