Multiple Choice
Which of the following best represents the freezing point of fluorine (F_2) under standard atmospheric pressure?
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14. Solutions
Freezing Point Depression
Multiple Choice
Which aqueous solution has the lowest freezing point, assuming each solute behaves as a nonelectrolyte and all solutions have the same concentration?
A
0.10 m sucrose
B
0.10 m glucose
C
0.10 m ethylene glycol
D
All have the same freezing point
Verified step by step guidance1
Understand that the freezing point depression depends on the molality of the solution and the number of particles the solute produces in solution, according to the formula: \(\Delta T_f = i K_f m\), where \(\Delta T_f\) is the freezing point depression, \(i\) is the van't Hoff factor, \(K_f\) is the freezing point depression constant of the solvent, and \(m\) is the molality of the solution.
Since the problem states that each solute behaves as a nonelectrolyte, the van't Hoff factor \(i\) for all solutes is 1, meaning they do not dissociate into ions and each solute particle remains intact in solution.
All solutions have the same molality (0.10 m), so the number of solute particles per kilogram of solvent is the same for each solution.
Because \(i\) and \(m\) are the same for all solutions, and \(K_f\) depends only on the solvent (water, in this case), the freezing point depression \(\Delta T_f\) will be the same for all three solutions.
Therefore, all three aqueous solutions will have the same freezing point, as the freezing point depression depends only on the number of solute particles, which is equal in all cases here.
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