Normal Boiling Point of Ethylene Glycol Solution
What is the normal boiling point of ethylene glycol [C₂H₆O₂] for the 34% solution and Kf =1.86 (C\m)?
Without the molality of the 34% ethylene glycol solution, we cannot calculate the normal boiling point from the provided options. The equation for boiling point elevation requires both the ebullioscopic constant and the solution's molality.
Answer:
Without the molality of the 34% ethylene glycol solution, we cannot calculate the normal boiling point from the provided options. The equation for boiling point elevation requires both the ebullioscopic constant and the solution's molality.
To find the normal boiling point of a 34% solution of ethylene glycol [C₂H₆O₂], one must consider the colligative properties of the solution. Specifically, the boiling point elevation phenomenon which states that the presence of a solute elevates the boiling point of a solvent. The normal boiling point can be calculated by using the equation ΔTb = Kb * m, where ΔTb is the boiling point elevation, Kb is the ebullioscopic constant (given as 1.86 °C/m), and m is the molality of the solution. Unfortunately, to proceed with this calculation, we would need additional information such as the molality (m) of the 34% solution, which is not provided. Given that we do not have all the necessary information, we cannot definitively determine the normal boiling point of the 34% ethylene glycol solution from the choices provided.