Final answer:
The aqueous solution with 0.75 M sucrose will have the highest freezing point as it is a non-electrolyte which contributes fewer solute particles compared to ionic solutions, resulting in the smallest freezing point depression.
Step-by-step explanation:
The question asks us to select the aqueous solution from a given list that has the highest freezing point. From the provided information, the solutions to arrange in order of increasing freezing points are 0.2 m NaCl, 0.3 m acetic acid, 0.1 m CaCl₂, and 0.2 m sucrose. Understanding colligative properties, we know that the freezing point of a substance is lowered when a solute is dissolved in it, and this effect depends on the number of particles in solution, not their identity.
To answer the question, we must consider the freezing point depression and the fact that ionic compounds like NaCl and CaCl₂ ionize and release more particles into the solution compared to non-electrolytes like sucrose, which doesn't ionize. Since 0.2 m sucrose remains as whole molecules, it will contribute fewer particles to the solution, thus having the least impact on freezing point depression.
The solution with 0.75 M C₁₂H₂₂O₁₁ (sucrose) will have the highest freezing point among the given examples because it is a non-electrolyte and will have the smallest effect on the freezing point depression, as compared to ionic compounds of the same concentration.