Final answer:
To solve for the boiling point of a solution, the molality must be calculated and used along with the van't Hoff factor and the boiling point elevation constant. However, the student's question lacks crucial information, such as the molar mass of AIF3, and includes incorrect data. Hence, the problem is unsolvable as stated.
Step-by-step explanation:
The subject question pertains to the boiling point elevation of a solution and requires knowledge of colligative properties, specifically the calculation of boiling point elevation using the molality of the solution. The given salt is assumed to have a 100% dissociation in water, and the molal boiling point elevation constant (Kb) for water is provided. The boiling point elevation can be calculated using the formula ΔTb = i * Kb * m, where ΔTb is the change in boiling point, i is the van't Hoff factor, Kb is the boiling point elevation constant, and m is the molality of the solution.
First, we need to calculate the molality of the AIF3 solution by finding the number of moles of AIF3 and dividing by the kilograms of solvent (water). Next, we use the molality with the provided Kb and the van't Hoff factor (for AIF3 it would be 4 because it dissociates into 4 ions: Al3+ and 3 F-) to find the boiling point elevation, and then add this to the normal boiling point of water to find the final boiling point of the solution.
However, since the student has made a mistake in their question by providing the wrong formula or a cryptic message AHfus × m = 3341 instead of correct data to calculate the molality of the solution, we are unable to solve the problem. The question also fails to specify the molar mass of AIF3, which is crucial for finding its molality. Therefore, none of the answer choices provided (A, B, C, or D) can be selected with confidence based on the information given. The student should clarify the molar mass of AIF3 and provide correct data to proceed with the calculation.