Final answer:
The 0.1 M CaCl₂ solution has the highest boiling point because it produces 3 ions per formula unit upon dissociation, which is more than the other salts and the non-electrolyte glucose, leading to a greater boiling point elevation.
Step-by-step explanation:
The question asks which aqueous solution among 0.1 M NaCl, 0.1 M CaCl₂, 0.1 M KCl, and 0.1 M glucose has the highest boiling point. According to colligative properties, boiling point elevation is directly related to the number of dissolved particles in the solution. For a given concentration, salt solutions that dissociate into more ions will typically have a higher boiling point due to the greater number of solute particles.
Considering the options presented, NaCl dissociates into 2 ions (Na^+ and Cl^-), KCl also dissociates into 2 ions (K^+ and Cl^-), but CaCl₂ dissociates into 3 ions (Ca^2+ and 2Cl^-). Glucose, being a non-electrolyte, does not dissociate into ions. So given the same molar concentration (0.1 M), the 0.1 M CaCl₂ solution will have the highest boiling point since it will produce the most ions upon dissociation, which are 3 ions per formula unit.