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NEET CHEMISTRYSolutionsEasy

Question

The largest freezing point depression among the following 0.10 m solutions is shown by:

A

KCl

B

C₆H₁₂O₆

C

Al₂(SO₄)₃

D

K₂SO₄

Step-by-Step Solution

The depression in freezing point (ΔTf\Delta T_f) is a colligative property proportional to the number of solute particles in the solution. It is calculated using the formula ΔTf=i×Kf×m\Delta T_f = i \times K_f \times m. Since the molality (m=0.10 mm = 0.10 \text{ m}) and the solvent (KfK_f) are the same for all options, the solution with the highest Van't Hoff factor (ii) will show the largest freezing point depression.

  1. KCl: Strong electrolyte, dissociates as K++Cl−K^+ + Cl^-. i=2i = 2.
  2. C₆H₁₂O₆ (Glucose): Non-electrolyte, does not dissociate. i=1i = 1.
  3. Al₂(SO₄)₃: Strong electrolyte, dissociates as 2Al3++3SO42−2Al^{3+} + 3SO_4^{2-}. Total ions = 5, so i=5i = 5.
  4. K₂SO₄: Strong electrolyte, dissociates as 2K++SO42−2K^+ + SO_4^{2-}. Total ions = 3, so i=3i = 3.

Since Al2(SO4)3Al_2(SO_4)_3 produces the maximum number of particles (i=5i=5), it exhibits the largest freezing point depression .

Exam Context & Concepts Covered

This question aligns with the NEET CHEMISTRY syllabus, specifically targeting concepts from Solutions. Mastering this topic is crucial for scoring well in the upcoming medical entrance examinations. Solving conceptually related problems will help you understand the nuances of these concepts and improve your problem-solving speed.

CHEMISTRYSolutionslargestfreezingdepressionfollowingsolutions

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