Name: Class: Date: Multiple Choice Identify the letter of the choice that best completes the statement or answers the question.

Size: px

Start display at page:

Download "Name: Class: Date: Multiple Choice Identify the letter of the choice that best completes the statement or answers the question."

Mildred Blair
7 years ago
Views:

1 Class: Date: Chapter 13 Multiple Choice Identify the letter of the choice that best completes the statement or answers the question. 1. In the Brønsted-Lowry model an acid is a. a proton donor. b. a proton acceptor. c. an electron pair acceptor. d. an electron pair donor. e. any substance which contains hydrogen. 2. Which of the following reactions are acid-base reactions according to the Brønsted-Lowry model? 1. NH 4+ (aq) + H 2 O NH 3 (aq) + H 3 O + (aq) 2. F - (aq) + H 2 O HF(aq) + OH - (aq) 3. H 2 PO 4- (aq) + OH - (aq) HPO 4 2- (aq) + H 2 O a. 1 only b. 2 only c. 3 only d. 1 and 3 e. 1, 2, and 3 3. The species formed when a proton is removed from an acid is called the a. cation. b. conjugate base. c. conjugate acid. d. buffer. e. antacid. 4. A species that can either accept or donate a proton is called a. a Brønsted-Lowry compound. b. a Lewis base. c. an Arrhenius acid. d. amphiprotic. e. a conjugate pair. 5. What is the conjugate base of HBr? a. b. H - c. Br + d. Br e. Br - 6. What is the conjugate acid of ammonia? a. b. H - c. NH + 4 d. NH 3 e. NH - 2 1

2 7. What is the conjugate base of water? a. b. O 2- c. OH - d. H 2 O e. H 3 O + 8. What is the conjugate acid of potassium hydrogen phosphate, K 2 HPO 4? a. H 3 PO 4 b. H 2 PO - 4 c. HPO 2-4 d. K + e. OH - 9. All of the following species are amphiprotic EXCEPT a. H 2 O. b. HSO 4-. c. HPO 2-4. d. H 2 PO 4-. e. H 3 PO Which of the following equilibrium constant expressions represents the ionization of water? a. K W = OH b. K W = OH OH c. K W = d. K W = log e. K W = log OH 11. Which of the following chemical reactions represents the ionization of water? a. 2H 2 O 2H 2 (g) + O 2 (g) b. H 2 O H 2 O - (aq) c. H 2 O H 2 O + (aq) + e - d. H 2 O (aq) + OH - (aq) e. (aq) + OH - (aq) H 2 O 2

3 12. If the concentration in a certain tap-water sample is M, what is the OH - concentration? (K w = ) a M b M c M d M e M 13. If the OH - concentration in a bottle of an ammonia based cleaner is M, what is the concentration? (K w = ) a M b M c M d M e M 14. If the concentration is less than M, the solution is a. basic. b. acidic. c. neutral. d. amphiprotic. e. in equilibrium. 15. What is the correct expression for the calculation of ph? a. ph = log[ ] b. ph = -log([ ][OH - ]) c. ph = log[oh - ] d. ph = -log[oh - ] e. ph = -log[ ] 16. If the ph of a solution is greater than 7, the solution is a. acidic. b. basic. c. amphiprotic. d. neutral. e. in equilibrium. 17. If the ph of vinegar is 3.0, what is the concentration of in vinegar? a M b M c M d M e M 18. The ph of a human blood sample is What is concentration of OH - in blood? a M b M c M d M e M 3

4 19. The hydronium ion concentration in a sample of lemon juice is M. What is the ph of the lemon juice? a b c d e Seawater has a hydroxide ion concentration of M. What is the ph of seawater? a b c d e What is the poh of 0.45 M KOH? a b c d e All of the following species are strong acids EXCEPT a. HClO 4. b. HBr. c. H 2 SO 4. d. HF. e. HI. 23. All of the following species are strong bases EXCEPT a. NaOH. b. KOH. c. Mg(OH) 2. d. Sr(OH) 2. e. RbOH. 24. Which of the following species is a weak base? a. KOH b. NH + 4 c. HF d. H 3 PO 4 e. CH 3 CO What is the ph of a solution prepared by diluting 0.35 mol HCl to a volume of 750 ml? a b c d e

5 26. Which of the following solutions will have a ph of 3.0? a M CH 3 CO 2 H b M NH 3 c M NH + 4 d M HI e. Answers b and c are correct. 27. Which of the following solutions will have a ph of 11.0? a. 11 M Sr(OH) 2 b M NH 3 c M HCl d M NH + 4 e M NaOH 28. Which of the following chemical reactions corresponds to the generic form of the acid dissociation constant (K a )? a. HB(aq) + H 2 O B - (aq) + H 3 O + (aq) b. HB(aq) + OH - (aq) B - (aq) + H 2 O c. 2H 2 O H 3 O + (aq) + OH - (aq) d. HA(aq) + HB(aq) H 2 A(aq) + B - (aq) e. B - (aq) + H 2 O HB(aq) + OH - (aq) 29. Which of the following chemical reactions corresponds to the generic form of the base dissociation constant (K b )? a. HB(aq) + OH - (aq) B - (aq) + H 2 O b. 2H 2 O H 3 O + (aq) + OH - (aq) c. HB(aq) + H 2 O B - (aq) + H 3 O + (aq) d. B - (aq) + H 2 O HB(aq) + OH - (aq) e. B - (aq) + H 3 O + (aq) HB(aq) + H 2 O 30. The acid equilibrium constant (K a ) for ammonium chloride refers to which of the following chemical reactions? a. NH 4+ (aq) + H 3 O + (aq) NH 5 2+ (aq) + H 2 O b. NH 4+ (aq) + H 2 O NH 3 (aq) + H 3 O + (aq) c. NH 4+ (aq) + OH - (aq) NH 3 (aq) + H 2 O d. NH 3 (aq) + H 2 O NH 4+ (aq) + OH - (aq) e. NH 3 (aq) + H 3 O + (aq) NH 4+ (aq) + H 2 O 31. The base equilibrium constant (K b ) for CN - refers to which of the following chemical reactions? a. HCN(aq) + H 2 O CN - (aq) + H 3 O + (aq) b. HCN(aq) + OH - (aq) CN - (aq) + H 2 O c. CN - (aq) + H 2 O HCN(aq) + OH - (aq) d. CN - (aq) + OH - (aq) HOCN(aq) e. CN - (aq) + H 3 O + (aq) HCN(aq) + H 2 O 5

6 32. Which of the following mathematical equations corresponds to the acid dissociation constant (K a )? OH a. K a = [ HB] [ HB] b. K a = B [ HB] B c. K a = d. K a = e. K a = È È B [ HB] È [ HB] B 33. The anions derived from strong acids are a. spectator ions. b. strong bases. c. amphiprotic. d. weak acids. e. strong acids. 34. The conjugate acid of a weak base is a. amphiprotic. b. a weak base. c. a weak acid. d. a strong acid. e. a strong base. 35. A solution of 0.10 M aluminum nitrate has a ph close to 3.0. Which chemical equation explains the acidic ph of the solution? a. Al 3+ (aq) + 3OH - (aq) Al(OH) 3 (s) + 3H 3 O + b. Al(H 2 O) 3+ 6 (aq) + H 2 O Al(H 2 O) 5 (OH) 2+ (aq) + H 3 O + (aq) c. Al(NO 3 ) 3 (s) + 3H 2 O Al(OH) 3 (s) + 3HNO 3 (s) d. HNO 3 (aq) + H 2 O NO 3- (aq) + H 3 O + (aq) e. NO 3- (aq) + H 2 O H 2 O + HNO 3 (aq) 6

7 36. The ph of M ammonium chloride, NH 4 Cl, is What is the value of K a for this acid? a b c d e The ph of M benzoic acid, HC 7 H 5 O 2, is What is the pk a for this acid? a b c d e The ph of M sodium nitrite, NaNO 2, is What is the K b for this base? a b c d e The ph of M sodium hypochlorite, NaClO, is What is the pk b for this base? a b c d e A 1.00 M solution of NH 4 Cl has a ph of What is the percent ionization of this acid? a % b. 0.28% c. 4.6% d. 9.3% e. 36% 41. A solution of 0.25 mol HF diluted to 1.0 L has a hydronium ion concentration of M. What is the percent ionization of HF? a % b. 1.3% c. 4.2% d. 5.2% e. 31% 42. What is the ph of 0.66 M hypochlorous acid? HOCl(aq) + H 2 O OCl - (aq) + H 3 O + (aq) K a = a b c d e

8 43. Ammonia is a weak base (K b = ). What is the ph of 1.2 M ammonia? a b c d e Lactic acid, HC 3 H 5 O 3, is found in sour milk. What is the ph of 0.30 M lactic acid? (K a = ) a b c d e Hydrogen sulfate ion, HSO 4-, has an acid dissociation constant of What is the ph of 0.45 M hydrogen sulfate? a b c d e Which of the following species is the strongest base? a. ClO - b. NH 3 c. CH 3 CO - 2 d. H - e. F Which of the following chemical equations corresponds to K a3 for phosphoric acid, H 3 PO 4? a. H 3 PO 4 (aq) + H 2 O H 2 PO 4- (aq) + H 3 O + (aq) b. H 2 PO 4- (aq) + H 2 O HPO 2-4 (aq) + H 3 O + (aq) c. HPO 2-4 (aq) + H 2 O PO 3-4 (aq) + H 3 O + (aq) d. H 3 PO 4 (aq) + 2H 2 O HPO 2-4 (aq) + 2H 3 O + (aq) e. H 2 PO 4- (aq) + 2H 2 O PO 3-4 (aq) + H 3 O + (aq) 48. Which of the following chemical equations corresponds to K b3 for sodium phosphate, Na 3 PO 4? a. PO 3-4 (aq) + H 3 O + (aq) HPO 2-4 (aq) + H 2 O b. PO 3-4 (aq) + H 2 O HPO 2-4 (aq) + OH - (aq) c. HPO 2-4 (aq) + H 2 O PO 3-4 (aq) + H 3 O + (aq) d. H 2 PO 4- (aq) + H 2 O H 3 PO 4 (aq) + OH - (aq) e. H 2 PO 4- (aq) + H 3 O + (aq) H 3 PO 4 (aq) + H 2 O 49. All of the following statements concerning diprotic acids and bases are incorrect EXCEPT a. K a1 is always large. b. K a1 is larger than K a2. c. K a1 is equal to K b2. d. K a1 + K b2 equals K w. e. K a1 + K a2 equals K w. 8

9 50. What is the ph of 1.0 M sulfurous acid? (K a1 = , K a2 = ) a b c d e The K a for hydrofluoric acid is What is K b for fluoride ion? a b c d e Determine the equilibrium constant for the reaction HF(aq) + NH 3 (aq) F - (aq) + NH 4+ (aq) given the equilibrium constants for the following reactions. HF(aq) + H 2 O(l) F - (aq) + H 3 O + (aq) K a = NH 3 (aq) + H 2 O(l) NH 4+ (aq) + OH - (aq) K b = H 2 O OH - (aq) + H 3 O + (aq) K w = a b c d e A salt solution can be acidic, basic, or neutral. When dissolved in water, which of the following salts will make the solution acidic: NaCl, Al 2 (SO 4 ) 3, LiNO 3, Na 2 CO 3, KF, and NH 4 Br? a. Al 2 (SO 4 ) 3 and NH 4 Br b. Al 2 (SO 4 ) 3, Na 2 CO 3 and NH 4 Br c. Al 2 (SO 4 ) 3 and LiNO 3 d. NaCl, LiNO 3 and NH 4 Br e. Na 2 CO 3, KF, and NH 4 Br 54. A salt solution can be acidic, basic, or neutral. When dissolved in water, which of the following salts will make the solution basic: FeCl 3, NaBr, CaCO 3, Na 3 PO 4, and NH 4 Br? a. CaCO 3 and Na 3 PO 4 b. FeCl 3 and NaBr c. FeCl 3 and CaCO 3 d. Na 3 PO 4 and NH 4 Br e. NH 4 Br 9

10 55. A salt solution can be acidic, basic, or neutral. When dissolved in water, which of the following salts will not affect the ph: KCl, FeCl 3, NaNO 3, CaCO 3, LiF, and NH 4 Br? a. KCl and FeCl 3 b. KCl, FeCl 3 and NaNO 3 c. CaCO 3 and LiF d. KCl and NaNO 3 e. CaCO 3, LiF, and NH 4 Br 10

11 Chapter 13 Answer Section MULTIPLE CHOICE 1. ANS: A 2. ANS: E 3. ANS: B 4. ANS: D 5. ANS: E 6. ANS: C 7. ANS: C 8. ANS: B 9. ANS: E 10. ANS: A 11. ANS: D 12. ANS: C 13. ANS: B 14. ANS: A 15. ANS: E 16. ANS: B 17. ANS: D 18. ANS: B 19. ANS: C 20. ANS: E 21. ANS: B 22. ANS: D 23. ANS: C 24. ANS: E 25. ANS: B 26. ANS: D 27. ANS: E 28. ANS: A 29. ANS: D 30. ANS: B 31. ANS: C 32. ANS: E 33. ANS: A 34. ANS: C 35. ANS: B 36. ANS: B 37. ANS: E 38. ANS: A 39. ANS: C 40. ANS: A 1

12 41. ANS: D 42. ANS: A 43. ANS: E 44. ANS: C 45. ANS: B 46. ANS: D 47. ANS: C 48. ANS: D 49. ANS: B 50. ANS: E 51. ANS: B 52. ANS: B 53. ANS: A 54. ANS: A 55. ANS: D 2

CHAPTERS 15 FAKE TEST QUESTIONS. 1. According to the Brønsted Lowry definition, which species can function both as an acid and as a base?

You might need to know the following K values: CHAPTERS 15 FAKE TEST QUESTIONS CH 3 COOH K a = 1.8 x 10 5 Benzoic Acid K a = 6.5 x 10 5 HNO 2 K a = 4.5 x 10 4 NH 3 K b = 1.8 x 10 5 HF K a = 7.2 x 10 4