Question: Which of the following will exhibit the greatest freezing point depression?
Options:
0.1 M NaCl
0.1 M K2SO4
0.1 M CaCl2
0.1 M urea
Correct Answer: 0.1 M CaCl2
Solution:
0.1 M K2SO4 will exhibit the greatest freezing point depression due to its van \'t Hoff factor of 3.
Which of the following will exhibit the greatest freezing point depression?
Practice Questions
Q1
Which of the following will exhibit the greatest freezing point depression?
0.1 M NaCl
0.1 M K2SO4
0.1 M CaCl2
0.1 M urea
Questions & Step-by-Step Solutions
Which of the following will exhibit the greatest freezing point depression?
Correct Answer: 0.1 M K2SO4
Step 1: Understand what freezing point depression means. It is the lowering of the freezing point of a solvent when a solute is added.
Step 2: Know that the extent of freezing point depression depends on the concentration of the solute and its ability to dissociate into particles in solution.
Step 3: Identify the van 't Hoff factor (i) for each solute. This factor tells us how many particles the solute breaks into when dissolved.
Step 4: For K2SO4, it dissociates into 2 potassium ions (K+) and 1 sulfate ion (SO4^2-), giving a total of 3 particles. So, its van 't Hoff factor is 3.
Step 5: Calculate the freezing point depression using the formula: ΔTf = i * Kf * m, where ΔTf is the freezing point depression, Kf is the freezing point depression constant, and m is the molality of the solution.
Step 6: Since K2SO4 has a higher van 't Hoff factor (3) compared to other solutes, it will cause a greater freezing point depression at the same molarity.
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