Chemical equilibrium, equilibrium constants Kp and Kc, Le Chatelier's principle, ionic equilibrium, acids and bases concepts, pH scale, buffers and solubility products - Question Bank
1. If the ionic product of a solution is less than its Ksp, the solution is:
2. The pH of a 0.001 M NaOH solution is:
3. For the equilibrium CaCO3(s) <=> CaO(s) + CO2(g), if the pressure of CO2 is increased, the equilibrium will:
4. Which of the following species can act as both a Brønsted-Lowry acid and a Brønsted-Lowry base?
5. The solubility of a salt is defined as:
6. A buffer solution prepared from a weak base and its conjugate acid will have its pH calculated using:
7. If Kp > Kc for a reversible reaction, it implies that:
8. The Ksp of Mg(OH)2 is 1.8 x 10^-11. The solubility of Mg(OH)2 in pure water is:
9. Which of the following is an amphoteric substance?
10. In an ionic equilibrium, the degree of dissociation of a weak electrolyte is:
11. For the reaction SO2Cl2(g) <=> SO2(g) + Cl2(g), if the pressure is increased by doubling the volume, the equilibrium will:
12. What is the concentration of H+ ions in a solution with pH = 5?
13. The Lewis acid-base reaction involves the transfer of:
14. Which of the following will decrease the solubility of AgCl in water?
15. The solubility of CaF2 is 's' mol/L. Its solubility product Ksp is:
16. A buffer solution of acetic acid and sodium acetate has a pH of 4.75. If Ka for acetic acid is 1.8 x 10^-5, what is the ratio of [CH3COO-]/[CH3COOH]?
17. The pH of a 0.01 M HCl solution is:
18. Which of the following is a strong base?
19. The ionization constant of a weak acid (Ka) is:
20. For the reaction 2SO2(g) + O2(g) <=> 2SO3(g) (exothermic), if temperature is decreased, equilibrium will:
21. The equilibrium constant Kp is defined in terms of:
22. Which factor does NOT affect the equilibrium position of a gaseous reaction?
23. A solution with a pOH of 2 is:
24. For the equilibrium CO(g) + H2O(g) <=> CO2(g) + H2(g), if the concentration of CO is increased, the equilibrium will:
25. The conjugate base of H2SO4 is:
26. Which of the following is an example of a Lewis acid?
27. The autoionization of water produces:
28. The common ion effect states that the solubility of a sparingly soluble salt is decreased by the presence of:
29. If the ionic product of a solution is greater than its Ksp, then:
30. The solubility product (Ksp) of a sparingly soluble salt like AgCl is:
31. The Henderson-Hasselbalch equation for a weak acid buffer is:
32. A buffer solution is typically made from a mixture of:
33. A buffer solution resists changes in pH upon addition of small amounts of:
34. Which of the following is a conjugate acid-base pair?
35. For a strong acid like HCl, its dissociation in water is:
36. What is the pOH of a solution with a pH of 10?
37. A solution with a pH of 3 is considered:
38. The pH of a neutral solution at 25°C is:
39. A Brønsted-Lowry base is defined as a species that:
40. According to Arrhenius theory, an acid is a substance that:
41. Which of the following is a characteristic of ionic equilibrium?
42. Adding a catalyst to a reversible reaction at equilibrium:
43. The relationship between Kp and Kc for the reaction N2(g) + 3H2(g) <=> 2NH3(g) is:
44. For an endothermic reaction at equilibrium, if the temperature is increased, the equilibrium will:
45. Le Chatelier's principle applies to:
46. Which of the following is a unit of Kc for the reaction H2(g) + I2(g) <=> 2HI(g)?
47. For the reaction PCl5(g) <=> PCl3(g) + Cl2(g), if the volume of the container is decreased, the equilibrium will:
48. The equilibrium constant Kc for the reaction aA + bB <=> cC + dD is given by:
49. In the equilibrium N2(g) + 3H2(g) <=> 2NH3(g), if the partial pressure of N2 is increased, what will happen to the equilibrium?
50. For a reversible reaction, which statement is always true at equilibrium?