Ionic equilibrium acids bases pH common ion effect hydrolysis and buffers - Question Bank
1. 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?
2. When a salt of a weak acid and strong base dissolves in water, the pH of the solution will be:
3. Which of the following is the most acidic?
4. The ionization of a weak acid is favored by:
5. A buffer solution is made from a weak base and its conjugate acid. The Henderson-Hasselbalch equation for this buffer is:
6. If the solubility of AgCl is 's', then its Ksp is:
7. Which of the following will decrease the pH of a solution?
8. The conjugate base of H2O is:
9. The pH of a 0.0001 M solution of NaOH is:
10. Which of the following statements is true for a neutral solution at 25°C?
11. For a polyprotic acid, the first dissociation constant (Ka1) is generally:
12. The common ion effect is an application of:
13. The buffer range of a buffer solution is typically:
14. Which type of hydrolysis occurs when a salt of a weak acid and strong base is dissolved in water?
15. The pKa of a weak acid is 5. What is the Ka?
16. The pH of a 0.01 M solution of a monoprotic strong acid is:
17. Which of the following is a Lewis base?
18. If the solubility of a sparingly soluble salt M(OH)2 is 's', then its solubility product (Ksp) is:
19. The Ostwald's dilution law is applicable to:
20. A buffer solution is prepared by mixing a weak acid with:
21. The hydrolysis of the salt of a strong acid and a strong base results in a solution that is:
22. Which of the following species is NOT a Brønsted-Lowry acid?
23. The pH of a 0.1 M solution of acetic acid (Ka = 1.8 x 10^-5) is approximately:
24. A substance that can act as both an acid and a base is called:
25. What is the relationship between pH and pOH at 25°C?
26. The solubility product (Ksp) of a sparingly soluble salt is the product of the concentrations of its ions, each raised to the power of its stoichiometric coefficient in the equilibrium equation. For CaF2, Ksp = [Ca2+][F-]^2. If [Ca2+] = x and [F-] = y, then Ksp is:
27. Which of the following is NOT a component of an acidic buffer solution?
28. Hydrolysis of a salt of a weak acid and weak base results in a solution that is:
29. For a sparingly soluble salt like AgCl, the common ion effect leads to:
30. The degree of dissociation of a weak electrolyte increases with:
31. Which factor affects the pH of a buffer solution the most?
32. The conjugate base of H2SO4 is:
33. A solution with a pH of 3 is considered:
34. In the autoionization of water, the equilibrium constant Kw is equal to:
35. The buffer capacity of a buffer solution is highest when:
36. Which of the following mixtures can act as a buffer solution?
37. The salt of a weak acid and strong base, when dissolved in water, undergoes:
38. For a weak base, a higher Kb value indicates:
39. The dissociation constant of a weak acid (Ka) is a measure of its:
40. What is the pOH of a 0.001 M solution of NaOH?
41. The pH of pure water at 25°C is:
42. Which of the following is a Lewis acid?
43. The Henderson-Hasselbalch equation for an acidic buffer is:
44. A buffer solution resists changes in pH upon addition of small amounts of:
45. Hydrolysis of a salt of a strong acid and weak base results in a solution that is:
46. The common ion effect describes the decrease in the solubility of a sparingly soluble salt when:
47. Which of the following is an amphoteric substance?
48. The conjugate acid of NH3 is:
49. According to the Brønsted-Lowry theory, a base is a substance that:
50. What is the pH of a 0.01 M solution of HCl?