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

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1 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 H 2 S K a = 5.7 x 10 8 HSO 4 K a = 1.2 x 10 2 HS K a = 1.2 x HCOOH K a = 1.8 x 10 4 HOCl K a = 3.0 x 10 8 SIMPLE ACIDS AND BASES 1. According to the Brønsted Lowry definition, which species can function both as an acid and as a base? (A) Cl (B) SO 4 2 (C) NH 4 + (D) HCO 3 (E) H 3 O + 2. Which of the following species can function as both a BrønstedLowry acid and a BrønstedLowry base in water? (A) HCl (B) HPO 4 2 (C) NH 2 (D) H 3 O + (E) NaOH 3. In this reaction, CH 3 COOH + H2O H3O + + CH 3 COO, which substances are bases according to the Brønsted Lowry definition? (A) CH 3 COOH and H 2 O (B) CH 3 COOH and CH 3 COO (C) H 2 O and CH 3 COO (D) H 3 O + and CH 3 COO 4. In the reaction CN + H2O HCN + OH, which is an acid base conjugate pair? (A) H 2 O and HCN (C) CN and H 2 O (B) H 2 O and OH (D) HCN and OH 5. Which species is not either an Arrhenius acid or base? (A) HCO 3 (B) NaOH (C) HIO 4 (D) NH 3 6. When we say an ion or a molecule is a base, we mean that it has a tendency to (A) combine with protons. (B) combine with electrons. (C) liberate hydroxide ions as the only anions. (D) liberate hydronium ions as the only cations. (E) Form only weakly dissociated salts. 7. Select the pair of substances in which an acid is listed followed by its conjugate base: (A) NH 3, NH 4 + (B) HPO 2 4, H 2 PO 4 (D) + CH 3 COOH, CH 3 COOH 2 (E) H 2 O, H 3 O + (C) HCO 3, CO 3 2 1

2 8. The conjugate acid of HPO 4 2 is: (A) P 2 O 5 (B) PO 4 3 Acid/Base Strengths (C) H 2 PO 4 (D) H 3 O + (E) H 3 PO 4 9. Given that HX is a stronger Brønsted acid than HY in aqueous solution, which is true of a 1 M solution of NaX? (A) It is less basic than a 1 M solution of NaY. (B) It is more basic than a 1 M solution of NaY. (C) It yields a neutral solution. (D) It is more concentrated than a l M solution of NaY. 10. Which series is the correct order of decreasing acid strength for each group of acids? (A) H 2 S > H 2 Te > H 2 Se > H 2 O (B) HClO 3 > HClO 4 > H 2 SO4 > HNO 3 (C) HClO 4 > HClO 3 > HClO 2 > HClO (D) HF > HCl > HBr > HI 11. In which pair is the first member a stronger proton donating acid than the second? (A) HClO 4, HClO 3 (B) H 2 SO 3, H 2 SO 4 (C) HIO, HBrO (D) H 2 O, H 2 S 12. In which pair of acids is the first member stronger than the second? (A) HClO > HIO (B) H3PO4 > HNO3 (C) H 2 SO3 > H 2 SO4 (D) HBrO > HBrO Which of the following is the strongest acid: (A) H 3 PO 4 (B) H 3 PO 3 (C) H 3 AsO 4 (D) H 3 AsO 3 (E) H 3 PO Given the data in the Table on the first page, select the strongest base. (A) Cl (B) F (C) ClO (D) HCOO (E) CH 3 COO 15. In each of the pairs below, predict which acid is stronger. (i) H 2 S and H 2 Se (ii) HNO 2 and HNO 3 (iii) H 2 SO 3 and HClO 3 (A) i) H 2 S (ii) HNO 3 (iii) H 2 SO 3 (B) i) H 2 Se (ii) HNO 3 (iii) HClO 3 (C) i) H 2 S (ii) HNO 3 (iii) HClO 3 (D) i) H 2 Se (ii) HNO 2 (iii) H 2 SO 3 (E) i) H 2 S (ii) HNO 2 (iii) H 2 SO Which of the following groups of acids is/are in the correct order of DECREASING acid strength? i) HI > HBr > HCl > HF ii) HBrO > HBrO 2 > HBrO 3 > HBrO 4 iii) HClO 4 > H 2 SO 4 > H 3 PO 4 (A) i and iii (B) i only (C) ii only (D) iii only (E) i and ii 2

3 17. The amide ion, NH 2, is a stronger base than the hydroxide ion, OH. Which reaction will occur if sodium amide is dissolved in water? (A) NH 2 + H 2 O H 3 O + + NH 2 (B) NH 2 + H 2 O NH 2 OH + H (C) NH 2 + H 2 O OH + NH 3 (D) NH 2 + H 2 O no reaction 18. The H 3 O + concentration in a 0.1 M solution of CH 3 COOH will be more than in (A) 0.1 M HF (B) 0.1 M NaHS (C) 0.1 M HNO 2 (D) 0.2 M CH 3 COOH (E) 0.1 M NaHSO 4 Simple ph Calculations 19. A solution that has ph of 8 is (A) very acidic. (B) slightly basic. (C) very basic. (D) exactly neutral. (E) slightly acidic. 20. The poh of an aqueous solution is 6.0. What is the [H + ]? (A) 1 x 10 8 M (B) 1 x 10 6 M (C) 1 x 10 7 M (D) 8 M 21. At 25 C the concentration of OH in moles per liter in a solution that has a ph of 8 is (A) 10 3 (B) 10 6 (C) 10 7 (D) 10 8 (E) The ph of a solution is 5. If the ph of this solution is decreased to 2, by what factor is the concentration of hydrogen ion increased? (A) 2 1/2 (B) 3 (C) 10 (D) 100 (E) HCl is a strong acid. What is the ph of 200 ml of M HCl? (A) 2.0 (B) 2.7 (C) 3.4 (D) What is the ph of a 0.01 M NaOH solution? (A) (B) 12 (C) 12 (D) 2 (E) The ph of a 1.0 x 10 3 M Ba(OH) 2 solution at 25 C is (A) 2.7 (B) 3.0 (C) 11.0 (D) When 50 ml of 0.1 M HCl is mixed with 50 ml of 0.2 M NaOH, the [H 3 O + ] is? (A) 0.05 M (B) l x 10 7 M. (C) 0.1 M. (D) 2 x (E) 0.2 M. 3

4 27. Which has the smallest concentration of OH ions? (A) 1 M NaOH (B) M NaOH (C) 1 M HCl (D) water (E) 1 M NH The [OH ] and ph of a M KOH solution are respectively: (A) M and 1.46 (B) M and 1.46 (C) 2.9 x M and (D) M and (E) 2.9 x M and What is the ph of a 1.0 x 10 8 M NaOH solution? (A) 8 (B) 6 (C) 7 (D) a bit less than 7 (E) a bit more than What is the ph of a solution made by mixing 50.0 ml of M KOH with 50.0 ml of M HCl. (A) 6.3 (B) 7.0 (C) 8.1 (D) 5.8 (E) 1.8 More Complex Equilibrium Calculations 31. What is the correct equation for the ion product constant of water? (A) [H 3 O + ] + [OH ] = (B) [H 3 O ] x [OH ] = 10 7 (C) [H 3 O + ] = (D) [H 3 O ] x [OH ] = [OH ] (E) [H 3 O + ] x [OH ] = [H 2 O] At 90 C pure water has a [H 3 O + ] = 1 x What is the value of K w at 90 C? (A) 1 x 10 6 (B) 7 x (C) 1 x (D) 1 x (E) 7 x At 75 C, K w = 5 x What is the ph of neutral water at 75 C? (A) 7 (B) 14 (C) 6.65 (D) 7.35 (E) 2.23 x A 0.20 M solution of the hypothetical weak acid HZ was found to have a ph of exactly 3.0. The ionization constant, K a, of the acid is (A) 0.6 (B) 2.0 x 10 4 (C) 1.0 x 10 3 (D) 5.0 x A 0.10 M C 4 H 9 COOH solution has a ph of What is the K a of this acid? (A) 6.6 x 10 6 (B) 2.6 x 10 3 (C) 6.6 x 10 5 (D) 2.6 x The ph of a 0.55 M solution of HBrO is What is the value of K a for HBrO? (A) 2.0 x 10 9 (B) 1.1 x 10 9 (C) 6.0 x 10 5 (D) 3.3 x 10 5 (E)

5 37. What is the ph of a M solution of HOCl? (A) 2.45 (B) 2.45 (C) 9.22 (D) 9.22 (E) What is the ph of a solution which is 0.10 M in a monoprotic acid, HA, with K a = 1.0 x 10 6? (A) 1.6 (B) 3.5 (C) 5.0 (D) The ionization constant of a weak acid HA is 1 x If 0.1 mol of the acid is dissolved in water and diluted to exactly one liter, what is the ph of the solution? (A) 1 (B) 3 (C) 5 (D) Enough water is added to 0.35 g of benzoic acid (C 6 H 5 COOH) to make 1000 ml of solution. What is the ph? (A) 1.9 (B) 2.6 (C) 3.4 (D) The dissociation constant for monoprotic acid HX in water is 1.34 x What is the concentration of X ion in a 0.20 M solution of HX? (A) 5.2 x 10 3 (B) 4.5 x 10 4 (C) 2.0 x 10 4 (D) 6.4 x The dissociation constant for a weak base B in water was found to be 1.25 x What is the concentration of H + in a 3.2 M solution of B? (A) 2.0 x 10 3 M (B) 1.6 x M (C) 4.0 x 10 6 M (D) 5.0 x M 43. What is the [OH ] in a 0.50 M solution of NH 3 (aq)? (A) 5 x 10 1 M (B) 1.8 x 10 5 M (C) 6 x 10 3 M (D) 9 x 10 6 M (E) 3 x 10 3 M 44. Arsenic acid (H 3 AsO 4 ) has K a values of 2.5 x 10 4, 5.6 x 10 8, and 3 x What is the concentration of the HAsO 4 2 dianion in a solution whose initial arsenic acid concentration was 0.35 M? (A) 9.4 x 10 3 M (B) 2.5 x 10 4 M (C) 8.8 x 10 5 M (D) 5.6 x 10 8 M (E) 3 x HCN has a K a of 2.9 x What is the [CN ] in M HCN? (A) 2.9 x 10 8 M (B) 4.24 M (C) 4.24 x 10 5 M (D) 4.24 x 10 8 M (E) 5.8 x 10 5 M 5

6 Ion Hydrolysis 46. What is the set of products expected from the hydrolysis of CN ion? (A) HCN and OH (B) CN and H 2 O (C) HCN and H + (D) HCN and H 2 O 47. Which substance dissolves in water to form an acidic solution? (A) KCl (B) Na 3 PO 4 (C) NH 4 Cl (D) Na 2 CO Which salt reacts with water (hydrolyzes) to produce a basic solution? (A) NaCH 3 COO (B) NaNO 3 (C) NH 4 Cl (D) Ba(ClO 4 ) Which solution has a ph less than 7.0? (A) 1 M CH 3 NH 3 Cl (B) 1 M NaOCl (C) 1 M K 2 CO 3 (D) 1 M NaOH 50. What is the ph of a 0.30 M sodium acetate, Na CH 3 COO solution? (A) 2.6 (B) 4.9 (C) 9.1 (D) Of the four following substances, which would form basic solutions: NH 4 Cl, NaNO 3, K 2 CO 3, NaF (A) NH 4 Cl and NaNO 3 (B) K 2 CO 3 and NH 4 Cl (C) NaF only (D) NaF and K 2 CO 3 (E) K 2 CO 3 only 52. Calculate the value of K b for F [K a for HF is 7.2 x 10 4 ]. (A) 2.0 x 10 8 (B) 1.4 x (C) 7.2 x (D) 7.2 x 10 4 (E) 1.4 x What is the ph of a 0.15 M solution of KF [K a for HF is 7.2 x 10 4 ]. (A) (B) 5.84 (C) 8.16 (D) 2.33 (E) Sodium hypochlorite (NaClO) is an active ingredient in some household laundry bleach. Given that the K a of HClO is 2.9 x 10 8, what is the ph of a M solution of sodium hypochlorite? (A) 9.4 (B) 10.4 (C) 8.9 (D) 9.9 (E) What answer best describes the ph of the following 0.1 M salt solutions? (a) NaF, (b) KBr, (c) KHCOO and (d) NH 4 Cl? (A) (a) ph < 7 (b) ph > 7 (c) ph > 7 (d) ph > 7 (B) (a) ph > 7 (b) ph = 7 (c) ph > 7 (d) ph < 7 (C) (a) ph < 7 (b) ph = 7 (c) ph < 7 (d) ph > 7 (D) (a) ph = 7 (b) ph = 7 (c) ph > 7 (d) ph < 7 (E) (a) ph < 7 (b) ph < 7 (c) ph < 7 (d) ph < 7 6

7 Buffers 56. Which pair constitutes a buffer in aqueous solution? (A) HCl and NaCl (B) HBr and KBr (C) NH 3 and NH 4 Cl (D) HNO 3 and NH 4 NO The addition of a small amount of acid or base will have very little effect on the ph value of a solution containing equal molar concentrations of (A) NH 4 Cl and NaCl (B) NaOH and NaCl (C) NaOH and HCl (D) NH 3 and NaCl (E) CH 3 COOH and NaCH 3 COO 58. Which of the following pairs could be used to make a buffer solution? (A) NH 3 + NaCH 3 COO (B) NaNO 3 + NH 4 Cl (C) CH 3 COOH + HCl (D) NaOH + NaCl (E) HNO 2 + NaNO Which of the following can form buffer systems? (a) HF/KF (b) HClO 4 /KClO 4 (c) Na 2 SO 3 /NaHSO 3 (A) (b) and (c) (B) (a) and (c) (C) all three (D) (b) (E) (a) and (b) 60. What is the ph of a buffer system consisting of 0.15 M CH 3 COONa and 0.10 M CH 3 COOH? (A) 2.78 (B) 2.87 (C) 5.56 (D) 7.00 (E) K b for ammonia is 1.8 x What is the ph of a solution prepared by combining 50.0 ml of 1.00 M NH 3 and 50.0 ml of 1.00 M NH 4 Cl? (A) 4.63 (B) 9.26 (C) 4.74 (D) 9.37 (E) What is the [OH ] of a solution which is 0.18 M in ammonium ion and 0.10 M in ammonia? (A) 1.3 x 10 3 (B) 1.3 x 10 5 (C) 1.0 x 10 3 (D) 1.0 x The acid HX has an ionization constant of 1 x A solution is 0.1 M in HX and 1.0 M in the salt Na + X. What is a close approximation of the hydrogen ion concentration? (A) 1 x 10 3 M (B) 1 x 10 5 M (C) 2 x 10 5 M (D) 1 x 10 8 M 64. A solution is M in acetic acid and M in NaCH 3 COO. What is the [H + ]? (A) 1.36 x 10 3 M (B) M (C) 1.80 x 10 5 M (D) M 65. What is the [H + ] of a solution which is 0.2 M in NaCH 3 COO and 0.1 M in CH 3 COOH? (A) 9.0 x 10 7 (B) 3.6 x 10 6 (C) 1.8 x 10 6 (D) 9.0 x

8 66. What is the ph of a buffer solution containing 0.10 M KNO 2 and 0.20 M HNO 2? (A) 3.66 (B) 3.05 (C) 3.35 (D) 2.02 LEWIS ACIDS AND BASES 67. SnCl 4 accepts two electron pairs and acts as (A) a Brønsted acid. (B) an Arrhenius base. (C) a Lewis acid. (D) a Lewis base. 68. Which of these species is most likely to be a Lewis acid and is also least likely to be a Brønsted acid? (A) NH 4 + (B) BF 3 (C) H 2 O (D) OH 69. Which compound functions as a Lewis acid but not as a Brønsted acid? (A) BCl 3 (B) NI 3 (C) HCl (D) H 2 O 70. According to the Lewis definition, an acid is a species (A) having a hydrogen ion. (B) donating a pair of electrons. (C) accepting a pair of electrons. (D) accepting a hydrogen ion. 71. In the reaction, BF 3 + F BF 4, BF 3 is acting as what type of acid? (A) Arrhenius only (B) BrønstedLowry only (C) Lewis only (D) All three (E) Arrhenius and BrønstedLowry Titrations 72. In titrating NH 3 (aq) with 0.1 M HCl, the equivalence point in ph units will be + (A) lower than 7 due to hydrolysis of NH 4 (B) lower than 7 due to hydrolysis of Cl + (C) higher than 7 due to hydrolysis of NH 4 (D) higher than 7 due to hydrolysis of Cl 73. When titrating 25 ml of 1.0 M HNO 2 with 2.0 M NaOH, which of the following statements is correct? (A) The ph at the start of the titration will be greater than 7. (B) The ph at the equivalence point will be equal to 7. (C) The equivalence point will occur after addition of 25 ml of NaOH (D) The ph at the equivalence point will be greater than 7. (E) HNO 2 is a strong acid 74. A 25.0mL sample of M HCl is mixed with 15.0 ml of M of NaOH. The ph of the resulting solution will be nearest (A) 2.1 (B) 7 (C) 11.9 (D)

9 75. In the titration of 50.0 ml of M benzoic acid (a monoprotic acid) with 50.0 ml of M Na0H, the properties of the solution at the equivalence point will correspond exactly to the properties of (A) a M sodium solution. (B) a M sodium hydroxide solution. (C) a M benzoic acid solution. (D) a M sodium benzoate solution. 76. Which equation best represents the net reaction that occurs when sodium hydroxide and hydrochloric acid solutions are mixed? (A) Na + + HCl NaCl + H + (B) OH + HCl H 2 O + Cl (C) OH + H 3 O + 2H 2 O (D) NaOH + H 3 O + 2H 2 O + Na Calculate the ph of a solution formed by mixing 25 ml of 0.1 M acetic acid with 12.5 ml of 0.1 M NaOH? (A) 2.87 (B) 3.02 (C) 4.74 (D) Calculate the ph of a solution formed by mixing 25 ml of 0.1 M acetic acid with 12.5 ml of 0.2 M NaOH? (A) 2.87 (B) 5.12 (C) 5.21 (D) What is the resultant ph when 0.6 moles of NaOH are added to 1 L of 0.90 M HCOOH solution (A) 10.0 (B) 7.00 (C) 2.55 (D) 4.05 (E) ml of 0.10 M C 2 H 5 NH 2 (ethylamine) is titrated with 9.00 ml of 0.15 M HCl. Given that the K b of ethylamine is 6.5 x 10 4, what is the ph of the solution? (A) (B) (C) (D) (E) What is the ph at the equivalence point for the titration of 30.0 ml of a 0.20 M C 6 H 5 COOH solution with 0.30 M KOH (K a of C 6 H 5 COOH = 6.5 x 10 5 )? (A) (B) 8.63 (C) 5.37 (D) 3.26 (E) What is the ph halfway to the equivalence point for the titration of 0.20 M CH 3 NH 2 with 0.20 M HCl? (K b of CH 3 NH 2 = 4.4 x 10 4 ) (A) 10.6 (B) 3.4 (C) 9.3 (D) 4.7 (E) What is the resultant ph when 20 ml of 0.30 M HCl is added to a 30.0 ml sample of 0.20 M NH 3 (K b for NH 3 = 1.8 x 10 5 ) (A) 6.0 (B) 8.9 (C) 11.3 (D) 2.72 (E) What is the resultant ph when 10.0 ml of M NaOH is added to 100 ml of a buffer solution that consists of 0.10 M CH 3 COOH and 0.10 M NaCH 3 COO. K a for CH 3 COOH is 1.8 x (A) 3.2 (B) 4.7 (C) 10.8 (D) 9.3 (E) 6.3 9

10 ANSWERS: 1 D 21 B 41 A 61 B 81 B 2 B 22 E 42 D 62 D 82 A 3 C 23 B 43 E 63 B 83 E 4 B 24 B 44 D 64 C 84 E 5 D 25 D 45 E 65 D 6 A 26 D 46 A 66 B 7 C 27 C 47 C 67 C 8 C 28 D 48 A 68 B 9 A 29 E 49 A 69 A 10 C 30 B 50 C 70 C 11 A 31 D 51 D 71 C 12 A 32 D 52 B 72 A 13 A 33 C 53 C 73 D 14 C 34 D 54 D 74 C 15 B 35 C 55 B 75 D 16 A 36 A 56 C 76 C 17 C 37 E 57 E 77 C 18 B 38 B 58 E 78 D 19 B 39 B 59 B 79 D 20 A 40 C 60 E 80 C 10

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