Van't Hoff Factor
A 0.1 m aqueous solution of BaCl₂ shows a depression of freezing point of 0.480 K. If Kf for water is 1.86 K kg mol⁻¹, the van't Hoff factor (i) for BaCl₂ in this solution is:
Select the correct option:
🔒 Solution Hidden from View
Submit your answer to unlock the detailed step-by-step solution.
More solutions Practice Questions
Which solute has van't Hoff factor i ≈ 3 in dilute aqueous solution?
Which solute has van't Hoff factor i ≈ 3 in dilute aqueous solution?
The Van't Hoff factor (i) for NaCl in dilute aqueous solution is approximately:
The Van't Hoff factor (i) for NaCl in dilute aqueous solution is approximately:
For an ideal solution formed by mixing two liquids at constant temperature, which of the following s...
For an ideal solution formed by mixing two liquids at constant temperature, which of the following s...
For a solid solute dissolving in a liquid solvent, which of the following statements correctly descr...
For a solid solute dissolving in a liquid solvent, which of the following statements correctly descr...
What is the boiling point of a solution containing 6 g of a non-volatile, non-electrolyte solute dis...
What is the boiling point of a solution containing 6 g of a non-volatile, non-electrolyte solute dis...
Benzoic acid dissolved in benzene shows an abnormally high molar mass when measured by colligative p...
Benzoic acid dissolved in benzene shows an abnormally high molar mass when measured by colligative p...
An aqueous solution of an unknown non-electrolyte solute has a freezing point of −0.744°C. Given K_f...
An aqueous solution of an unknown non-electrolyte solute has a freezing point of −0.744°C. Given K_f...
A mixture of two miscible liquids that boils at a constant composition and temperature, lower than e...
A mixture of two miscible liquids that boils at a constant composition and temperature, lower than e...
A mixture contains 36 g of water and 92 g of ethanol (molar mass 46 g/mol). What is the mole fractio...
A mixture contains 36 g of water and 92 g of ethanol (molar mass 46 g/mol). What is the mole fractio...
The osmotic pressure of a 0.02 M solution of a non-electrolyte at 300 K is closest to which value? (...
The osmotic pressure of a 0.02 M solution of a non-electrolyte at 300 K is closest to which value? (...
Which of the following pairs of liquids is expected to show a positive deviation from Raoult's law a...
Which of the following pairs of liquids is expected to show a positive deviation from Raoult's law a...
A 0.01 M aqueous solution of AlCl₃ has an osmotic pressure of 0.0984 atm at 300 K. If complete disso...
A 0.01 M aqueous solution of AlCl₃ has an osmotic pressure of 0.0984 atm at 300 K. If complete disso...
About This Question
- Subject
- chemistry
- Chapter
- solutions
- Topic
- van't hoff factor
- Difficulty
- Medium
- Year
- 2025
Solution
Correct Answer:
2.58
The observed freezing point depression is ΔTf = i × Kf × m. Substituting: 0.480 = i × 1.86 × 0.1 = i × 0.186. Therefore, i = 0.480 / 0.186 = 2.58. For complete dissociation of BaCl₂ → Ba²⁺ + 2Cl⁻, the theoretical van't Hoff factor would be 3 (one formula unit yields 3 ions). The observed value of 2.58 is less than 3, indicating incomplete dissociation or ion-pair formation in the solution. This is typical behaviour for strong electrolytes at moderate concentrations where interionic attractions reduce the effective number of particles.
This medium difficulty chemistry question is from the chapter solutions, covering the topic of van't hoff factor. It appeared in the 2025 exam.
Looking for more practice? Explore all chemistry questions or browse solutions questions on RankGuru.