JEE Main - Ionic equilibrium acids bases pH common ion effect hydrolysis and buffers One Line Questions & Answers

1. Which of the following statements is true for a neutral solution at 25°C? — [H+] = [OH-]

2. In the autoionization of water, the equilibrium constant Kw is equal to: — [H+][OH-]

3. When a salt of a weak acid and strong base dissolves in water, the pH of the solution will be: — > 7

4. The pH of pure water at 25°C is: — 7

5. What is the pH of a 0.01 M solution of HCl? — 2

6. What is the pOH of a 0.001 M solution of NaOH? — 1

7. The pH of a 0.01 M solution of a monoprotic strong acid is: — 2

8. The pH of a 0.0001 M solution of NaOH is: — 10

9. The pH of a 0.1 M solution of acetic acid (Ka = 1.8 x 10^-5) is approximately: — 3.42

10. If the solubility of a sparingly soluble salt M(OH)2 is 's', then its solubility product (Ksp) is: — 4s3

11. The pKa of a weak acid is 5. What is the Ka? — 10^-5

12. The dissociation constant of water (Kw) at 37°C is approximately 2.4 x 10^-14. What is the pH of neutral water at this temperature? — 6.6

13. The common ion effect describes the decrease in the solubility of a sparingly soluble salt when: — A common ion is added to the solution.

14. Which of the following is NOT a component of an acidic buffer solution? — A strong acid

15. According to the Brønsted-Lowry theory, a base is a substance that: — Accepts a proton

16. Hydrolysis of a salt of a strong acid and weak base results in a solution that is: — Basic

17. A solution with a pH of 3 is considered: — Acidic

18. Hydrolysis of a salt of a weak acid and weak base results in a solution that is: — Depends on the relative strengths of the acid and base

19. The hydrolysis of the salt of a strong acid and a strong base results in a solution that is: — Neutral

20. Which of the following will decrease the pH of a solution? — Adding HCl

21. A substance that can act as both an acid and a base is called: — Amphoteric

22. Which of the following is a Lewis base? — NH3

23. The salt of a weak acid and strong base, when dissolved in water, undergoes: — Anionic hydrolysis

24. Which type of hydrolysis occurs when a salt of a weak acid and strong base is dissolved in water? — Anionic hydrolysis

25. Which of the following mixtures can act as a buffer solution? — CH3COOH and CH3COONa

26. Which factor affects the pH of a buffer solution the most? — Dilution

27. For a polyprotic acid, the first dissociation constant (Ka1) is generally: — Greater than Ka2

28. Which of the following species is NOT a Brønsted-Lowry acid? — Cl-

29. The conjugate base of H2O is: — OH-

30. Which of the following is an amphoteric substance? — H2O

31. The conjugate base of H2SO4 is: — HSO4-

32. The degree of dissociation of a weak electrolyte increases with: — Decrease in concentration

33. For a sparingly soluble salt like AgCl, the common ion effect leads to: — Decreased solubility

34. Which of the following is a characteristic of a strong acid? — It completely dissociates in water.

35. A buffer solution is prepared by mixing a weak acid with: — Its conjugate base

36. The common ion effect is an application of: — Le Chatelier's principle

37. The ionization of a weak acid is favored by: — Low concentration

38. The conjugate acid of NH3 is: — NH4+

39. Which of the following is a Lewis acid? — BF3

40. What is the relationship between pH and pOH at 25°C? — pH + pOH = 14

41. Which of the following is the most acidic? — pH = 2

42. The buffer capacity of a buffer solution is highest when: — pH = pKa

43. The Henderson-Hasselbalch equation for an acidic buffer is: — pH = pKa + log([conjugate base]/[acid])

44. The buffer range of a buffer solution is typically: — pKa ± 1

45. A buffer solution is made from a weak base and its conjugate acid. The Henderson-Hasselbalch equation for this buffer is: — pOH = pKb + log([conjugate acid]/[base])

46. If the solubility of AgCl is 's', then its Ksp is: — s^2

47. The dissociation constant of a weak acid (Ka) is a measure of its: — Strength

48. A buffer solution resists changes in pH upon addition of small amounts of: — Strong acid or strong base

49. The Ostwald's dilution law is applicable to: — Weak electrolytes

50. For a weak base, a higher Kb value indicates: — Stronger base

Ionic equilibrium acids bases pH common ion effect hydrolysis and buffers - One Line Questions