Final 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.
Step-by-step explanation:
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.