Boiling Point Elevation
Boiling point elevation is the phenomenon in which the boiling point of a solution is higher than that of the pure solvent. This is due to the presence of a non-volatile solute in the solution, which reduces the vapor pressure of the solvent.

Formula for Boiling Point Elevation
ΔTb = Kb × msolute
where ΔTb is the boiling point elevation, Kb is the molal boiling point elevation constant, and msolute is the molality of the solute.

Calculation of Boiling Point Elevation
Given, freezing point depression = -0.465°C
We know that, ΔTf = Kf × msolute
where ΔTf is the freezing point depression, Kf is the molal freezing point depression constant, and msolute is the molality of the solute.

Kf for water is 1.86 °C/m

-0.465 = 1.86 × msolute
msolute = -0.25 mol/kg

Now, we need to calculate the boiling point elevation using the formula ΔTb = Kb × msolute
Kb for water is 0.512°C/m

ΔTb = 0.512 × -0.25
ΔTb = -0.128°C

Therefore, the boiling point of the solution is 100°C - 0.128°C = 99.872°C.

Explanation
The presence of a non-volatile solute in a solution reduces the vapor pressure of the solvent, which results in a higher boiling point than that of the pure solvent. The amount of boiling point elevation is directly proportional to the molality of the solute in the solution. The molal boiling point elevation constant is a characteristic property of the solvent and is used to calculate the boiling point elevation of a solution.