Published by:
CGP EDU Academic Team
Published on: August 14, 2026
A 0.01 molal solution of ammonia freezes at –0.02ºC. Calculate the van’t Hoff factor, i and the percentage dissociation of ammonia in water. 
= 1.86 deg molal –1 .
Text Solution
Verified by ExpertsThe correct answer is:
1
1.075, 7.5.
Experimental Δ T = 0.02º
Theoretical Δ T = 1.86 × 0.01 = 0.0186º
i = van’t Hoff factor = 
= 1.075
Degree of dissociation, α = 
(v = no. of species formed on dissociation)
= 
= 0.075
% dissociation = 7.5.
Prepare Smarter with CGP Edu
Get practice questions, solutions, and test series in one place.
Write a Review
Share your experience with this question and solution.
Commentary
Send your comment, doubt, correction, or feedback to admin.
Similar Questions
Explore conceptually related problems
The latent heat of vapourisation of water is and if the b.p. is , ebullioscopic constant of water…
The molal elevation constant of water . The boiling point of 1.0 molal aqueous solution (assuming…
The rise in the boiling point of a solution containing 1.8 gram of glucose in of a solvent in . T…
If of a solute dissolved in of solvent is boiled at a temperature higher by than that of the pur…
Pressure cooker reduces cooking time for food because
Which of the following statements is correct for the boiling point of solvent containing a dissolve…