Final answer:
Calcium chloride (CaCl₂) will have the highest boiling point among the given solutes, due to its dissociation into three ions, leading to a boiling point elevation of 1.53°C over the pure solvent.
Step-by-step explanation:
According to the properties of colligative properties and the molal boiling point elevation constant, we can determine that calcium chloride (CaCl₂) will have the highest boiling point among the solutes listed, due to the number of ions it produces in solution. When calcium chloride dissolves in water, it breaks into three ions (one Ca²⁺ and two Cl⁻), thus for a 1.00 m solution, the boiling point elevation would be 1.53°C (3 x 0.51°C/m), resulting in a boiling point of approximately 101.53°C. The boiling point order from lowest to highest is for the pure solvent (water), sucrose, sodium chloride (NaCl), and then calcium chloride (CaCl₂), assuming ideal behavior and a constant boiling point elevation factor for water (0.51°C/m).