Reflecting on the Boiling Point of Ethylene Glycol in a 34% Solution

What is the normal boiling point of ethylene glycol [C2H6O2] for the 34% solution and Kf =1.86 ( oC\\m)?

O Tb=79.5C O Tb=88.60 OTb=64.30 O DOES NOT EXIST Tb=77.5C O Tb=72.5C O Tb=84.5C O Tb=48.10

Answer:

The normal boiling point of a 34% solution of ethylene glycol is 198.13 oC. Ethylene glycol in a 34% solution has a standard boiling point of 198.13 oC.

The boiling point of a solution depends on the concentration of solute particles. In this case, ethylene glycol [C2H6O2] is the solute and it forms a 34% solution. The boiling point elevation depends on the molality of the solution and the molal boiling point constant, Kf.

The equation to calculate the boiling point elevation is ΔTb = Kf * m, where ΔTb is the boiling point elevation, Kf is the molal boiling point constant, and m is the molality of the solution.

Given that Kf = 1.86 (oC/m) and a 34% solution, we can calculate the boiling point elevation by multiplying the molality of the solution by the molal boiling point constant: ΔTb = 1.86 * 0.34 = 0.6316 (oC).

To find the boiling point of the solution, we add the boiling point elevation to the normal boiling point of the pure solvent. The normal boiling point of ethylene glycol is 197.5 (oC), so the boiling point of the 34% solution would be approximately 197.5 + 0.6316 = 198.13 (oC).