Solutions - Abnormal Molar Mass, Van't Hoff Factor

Grade 12 Chemistry — Solutions - Abnormal Molar Mass, Van't Hoff Factor: 25 practice questions with instant scoring and explanations.

1. The van't Hoff factor (i) accounts for:
2. For acetic acid in water, i < 1 due to:
3. The observed molar mass is related to theoretical molar mass by:
4. For NaCl, the van't Hoff factor is approximately:
5. The degree of dissociation (α) is related to van't Hoff factor by:
6. For a binary electrolyte dissociating into n ions, i = 1 + α(n-1) where α is:
7. If a solute forms dimers in solution, the van't Hoff factor (i) is:
8. For weak electrolytes like acetic acid, i is:
9. For strong electrolytes like HCl, i is:
10. The freezing point depression is ΔTf = i × Kf × m. For 0.1 m NaCl (i≈2) and Kf=1.86:
11. An abnormal molar mass is observed for:
12. The experimental molar mass of acetic acid in water is about 60, while theoretical is 60. This indicates:
13. If observed molar mass < theoretical molar mass, the solute is likely:
14. For CaCl₂, which dissociates as CaCl₂ → Ca²⁺ + 2Cl⁻, the ideal i value is:
15. The actual van't Hoff factor for CaCl₂ in dilute solution is approximately:
16. Abnormal behavior is most common in:
17. The degree of ionization (α) can be calculated from colligative property by:
18. If a weak acid shows i = 1.5 and dissociates as HA ↔ H⁺ + A⁻ (n=2), then α is:
19. For benzoic acid in benzene, i < 1 because:
20. The deviation from ideal behavior increases with:
21. For a solution where observed M is 45 g/mol and theoretical M is 90 g/mol, i =:
22. Which of the following shows maximum deviation from ideal behavior?
23. The van't Hoff factor corrects for:
24. For a non-electrolyte solute, the observed molar mass:
25. In concentrated NaCl solutions, i is less than 2 due to: