Final answer:
The question addresses the calculation of the boiling point elevation of a barium nitrate solution using the van't Hoff factor. To predict the boiling point, the boiling point elevation formula and the molal boiling point elevation constant, Kb, are needed, which are not provided.
Step-by-step explanation:
The question pertains to the boiling point elevation of aqueous solutions, which is a colligative property influenced by the van't Hoff factor (i). Boiling point elevation is 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 molal boiling point elevation constant, and m is the molality of the solution. Barium nitrate, Ba(NO3)2, is a salt that dissociates into three ions (Ba2+ and two NO3-), giving it an ideal van't Hoff factor of 3. The boiling point of pure water is 100°C, and thus, the boiling point of the 1.80 m solution can be elevated. However, to accurately predict the boiling point from provided options, the complete formula and Kb value for water are needed, which are not given in the provided information.