Question:
Which of the following solution will have highest freezing point depression?
Which of the following solution will have highest freezing point depression?
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Electrolytes show greater colligative effects due to dissociation into ions.
Updated On: Mar 28, 2026
- 1 M glucose
- 1 M sucrose
- 1 M urea
- 1 M KCl
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The Correct Option is D
Solution and Explanation
Step 1: Understanding freezing point depression.
Freezing point depression is a colligative property and depends on the number of particles present in solution.
Step 2: Role of Van’t Hoff factor.
\[ \Delta T_f = i K_f m \] where \( i \) is the Van’t Hoff factor.
Step 3: Comparing the solutions.
Glucose, sucrose, and urea are non-electrolytes and do not dissociate, so \( i = 1 \).
KCl dissociates into \( \mathrm{K^+} \) and \( \mathrm{Cl^-} \), so \( i = 2 \).
Step 4: Conclusion.
Since KCl produces the maximum number of particles, it shows the highest freezing point depression.
Freezing point depression is a colligative property and depends on the number of particles present in solution.
Step 2: Role of Van’t Hoff factor.
\[ \Delta T_f = i K_f m \] where \( i \) is the Van’t Hoff factor.
Step 3: Comparing the solutions.
Glucose, sucrose, and urea are non-electrolytes and do not dissociate, so \( i = 1 \).
KCl dissociates into \( \mathrm{K^+} \) and \( \mathrm{Cl^-} \), so \( i = 2 \).
Step 4: Conclusion.
Since KCl produces the maximum number of particles, it shows the highest freezing point depression.
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