Ignoring ion pairing, which aqueous solution has the highest normal boiling point?

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To compare boiling points, we apply the boiling point elevation formula ΔTb = i · Kb · m, where i is the van't Hoff factor (number of particles the solute yields in solution) and m is the molality. The solution with the largest product i·m will have the highest normal boiling point.
Option 1: 0.15 m Ca(NO3)2. This electrolyte dissociates into three particles (Ca2+ and two NO3−), so i ≈ 3. The product i·m = 3 × 0.15 = 0.45, which is relatively large among the given options.
Option 2: 0.20 m C3H7OH. Ethanol is a nonelectrolyte, so it does not dissociate; i ≈ 1. The product i·m = 1 × 0.20 = 0.20, considerably smaller than 0.45, so its boiling point elevation would be less.
Option 3: 0.15 m NaCl. Sodium chloride dissociates into Na+ and Cl−, giving i ≈ 2. The product i·m = 2 × 0.15 = 0.30, which is smaller than 0.45, so the boiling point rise would be less than that of the Ca(NO3)2 solution.
Option 4: 0.20 m KBr. Potassium bromide also yields two ions (K+ and Br−), so i ≈ 2. The product i·m = 2 × 0.20 = 0.40, still below 0.45, indicating a smaller boiling point elevation than Ca(NO3)2.
Overall, the largest i·m among these options is 0.45 for 0.15 m Ca(NO3)2, due to its three particles upon dissociation, which drives the greatest boiling point elevation among the choices.

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Ignoring ion pairing, which aqueous solution has the highest normal boiling point?

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