Chemical equilibrium, equilibrium constants Kp and Kc, Le Chatelier's principle, ionic equilibrium, acids and bases concepts, pH scale, buffers and solubility products - One Line Questions

1. The equilibrium constant Kc for the reaction aA + bB <=> cC + dD is given by: — ([C]^c [D]^d) / ([A]^a [B]^b)
2. The solubility product (Ksp) of a sparingly soluble salt like AgCl is: — [Ag+][Cl-]
3. The pH of a neutral solution at 25°C is: — 7
4. The pH of a 0.01 M HCl solution is: — 2
5. 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]? — 1:1
6. What is the concentration of H+ ions in a solution with pH = 5? — 10^-5 M
7. The Ksp of Mg(OH)2 is 1.8 x 10^-11. The solubility of Mg(OH)2 in pure water is: — 1.3 x 10^-4 M
8. The pH of a 0.001 M NaOH solution is: — 11
9. What is the pOH of a solution with a pH of 10? — 4
10. The solubility of CaF2 is 's' mol/L. Its solubility product Ksp is: — 4s^3
11. The common ion effect states that the solubility of a sparingly soluble salt is decreased by the presence of: — A common ion
12. The Lewis acid-base reaction involves the transfer of: — An electron pair
13. A buffer solution is typically made from a mixture of: — A weak acid and its conjugate base
14. A Brønsted-Lowry base is defined as a species that: — Accepts a proton
15. A solution with a pH of 3 is considered: — Acidic
16. A solution with a pOH of 2 is: — Acidic
17. Which of the following will decrease the solubility of AgCl in water? — Adding NaCl solution
18. Which of the following is an example of a Lewis acid? — BF3
19. In an ionic equilibrium, the degree of dissociation of a weak electrolyte is: — Directly proportional to the square root of dilution
20. According to Arrhenius theory, an acid is a substance that: — Dissociates in water to produce H+ ions
21. The autoionization of water produces: — H3O+ and OH- ions
22. Which of the following is a conjugate acid-base pair? — All of the above
23. Which of the following species can act as both a Brønsted-Lowry acid and a Brønsted-Lowry base? — HCO3-
24. Which of the following is an amphoteric substance? — H2O
25. The conjugate base of H2SO4 is: — HSO4-
26. Which of the following is a characteristic of ionic equilibrium? — It involves reactions between ions in solution.
27. The relationship between Kp and Kc for the reaction N2(g) + 3H2(g) <=> 2NH3(g) is: — Kp = Kc(RT)^-2
28. Which of the following is a unit of Kc for the reaction H2(g) + I2(g) <=> 2HI(g)? — Unitless
29. The equilibrium constant Kp is defined in terms of: — Partial pressures
30. Which of the following is a strong base? — NaOH
31. For a strong acid like HCl, its dissociation in water is: —
32. A buffer solution prepared from a weak base and its conjugate acid will have its pH calculated using: — pOH = pKb + log([conjugate acid]/[base])
33. The Henderson-Hasselbalch equation for a weak acid buffer is: — pH = pKa + log([conjugate base]/[acid])
34. If the ionic product of a solution is greater than its Ksp, then: — Precipitation will occur
35. For the reaction PCl5(g) <=> PCl3(g) + Cl2(g), if the volume of the container is decreased, the equilibrium will: — Shift to the right
36. For an endothermic reaction at equilibrium, if the temperature is increased, the equilibrium will: — Shift to the right
37. For the equilibrium CO(g) + H2O(g) <=> CO2(g) + H2(g), if the concentration of CO is increased, the equilibrium will: — Shift to the right
38. For the reaction 2SO2(g) + O2(g) <=> 2SO3(g) (exothermic), if temperature is decreased, equilibrium will: — Shift to the right
39. For the reaction SO2Cl2(g) <=> SO2(g) + Cl2(g), if the pressure is increased by doubling the volume, the equilibrium will: — Shift to the right
40. For the equilibrium CaCO3(s) <=> CaO(s) + CO2(g), if the pressure of CO2 is increased, the equilibrium will: — Shift to the left
41. In the equilibrium N2(g) + 3H2(g) <=> 2NH3(g), if the partial pressure of N2 is increased, what will happen to the equilibrium? — Shift to the right (towards products)
42. Adding a catalyst to a reversible reaction at equilibrium: — Increases the rate of both forward and reverse reactions equally, reaching equilibrium faster.
43. A buffer solution resists changes in pH upon addition of small amounts of: — Strong acid or strong base
44. Le Chatelier's principle applies to: — Systems at equilibrium
45. Which factor does NOT affect the equilibrium position of a gaseous reaction? — Addition of an inert gas at constant volume
46. The ionization constant of a weak acid (Ka) is: — The equilibrium constant for its dissociation
47. The solubility of a salt is defined as: — The maximum amount of solute that can dissolve in a given amount of solvent at a specific temperature.
48. For a reversible reaction, which statement is always true at equilibrium? — The rate of the forward reaction is equal to the rate of the reverse reaction.
49. If the ionic product of a solution is less than its Ksp, the solution is: — Unsaturated
50. If Kp > Kc for a reversible reaction, it implies that: — Δn > 0 (change in moles of gas is positive)
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E-Book Chemical equilibrium, equilibrium constants Kp and Kc, Le Chatelier's principle, ionic equilibrium, acids and bases concepts, pH scale, buffers and solubility products Audio Book Chemical equilibrium, equilibrium constants Kp and Kc, Le Chatelier's principle, ionic equilibrium, acids and bases concepts, pH scale, buffers and solubility products Online Test 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 Chemical equilibrium, equilibrium constants Kp and Kc, Le Chatelier's principle, ionic equilibrium, acids and bases concepts, pH scale, buffers and solubility products