Final answer:
The boiling point of the solution would be above the lower boiling point of component A (46.0°C) and below the higher boiling point of component B (116.0°C), due to boiling point elevation. An exact boiling point cannot be determined without additional information, but it's clear that it will be between these two temperatures.
Step-by-step explanation:
The boiling point of a liquid solution containing components A and B, with boiling point elevation taken into consideration, will always be higher than the boiling point of the pure solvent with the lower boiling point. Since the solution behaves as an ideal solution, and using the mole fraction of component A (0.69) and the boiling points of pure A (46.0°C) and pure B (116.0°C), the boiling point of the solution will lie somewhere between these two temperatures. Applying this logic and the principles of boiling point elevation, the solution's boiling point will be higher than 46.0°C but less than 116°C. The elevation effect increases the boiling point due to the presence of the solute decreasing the vapor pressure of the liquid solvent. Although we don't have enough information to calculate the exact boiling point here, it's certain that the answer is A) It is somewhere between 46 and 116 degrees C.