Final answer:
The boiling point of a NaCl solution would be slightly above the normal boiling point of water, which is 100°C, due to boiling point elevation caused by the NaCl's dissociation into ions.
Step-by-step explanation:
The normal boiling point of water is 100°C, however, when a solute like NaCl is added, the boiling point changes due to the phenomenon of boiling point elevation. The boiling point elevation depends on the molality of the solution and the van't Hoff factor (i), which represents the number of particles the solute dissociates into. In the case of NaCl, which dissociates into two ions (Na+ and Cl-), the van't Hoff factor is 2. Thus, the boiling point elevation can be calculated using the formula ΔTb = i * Kb * molality, where ΔTb is the change in boiling point, Kb is the ebullioscopic constant for the solvent, and molality is the number of moles of solute per kilogram of solvent. However, without the ebullioscopic constant for water, we cannot directly calculate the boiling point elevation. Yet, if we assume the student's solution behaves ideally, we can infer that the boiling point increase would be proportional to the freezing point depression. Since the freezing point depression is -0.93°C, assuming that the effects are proportionally similar, the increase in boiling point would be slightly more due to NaCl. Taking into account the ideal solution behavior, we would expect the boiling point of the NaCl solution to be slightly above 100°C.