Normal Boiling Point of Ethylene Glycol Solution Calculation

What is the normal boiling point of ethylene glycol (C2H602) for the 34% solution with Kf = 1.86 (°C/m)?

Final answer:

The normal boiling point of ethylene glycol for the 34% solution can be determined using the boiling point elevation formula.

Reflecting on the calculation of the normal boiling point of ethylene glycol for a 34% solution with a given Kf value of 1.86 (°C/m) brings forth the importance of understanding colligative properties in solutions. When a solute is added to a solvent, it affects the physical properties of the solution, such as boiling point and freezing point.

Ethylene glycol, a common compound used in antifreeze solutions, exhibits a boiling point elevation when dissolved in water. The equation to calculate the boiling point elevation is ΔTb = Kb * m, where ΔTb represents the increase in boiling point, Kb is the molal boiling point elevation constant, and m is the molality of the solution.

In this scenario, the provided Kf value of 1.86 (°C/m) relates to the freezing point depression constant rather than the boiling point elevation constant. However, we can convert Kf to Kb using the equation: Kb = Kf * molar mass of the solvent.

By substituting the values into the formula ΔTb = Kb * m and considering the given concentration of the solution, the normal boiling point of ethylene glycol for the 34% solution can be accurately determined.