CH 3 NH 2 + H 2 O <=== CH 3 NH 3 + OH - b. CH 3 CH 2 NH 2 + H 2 O <=== CH 3 CH 2 NH OH - c. HC 2 H 3 O 2 + H 2 O <=== H 3 O + -

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1 Sample Test 2 CHAPTER Acids and bases can be defined in several ways. Which of the following are definitions of bases according to these definitions? a compound the produces hydronium ions in water b. a proton acceptor c. an electron pair acceptor d. an electron pair donor e. both b and d statements. 2. When H 2 SO is dissolved in water, which species would be found in the water at equilibrium in measurable amounts? H 2 SO b. H 3 SO c. HSO d. SO 2 e. OH 3. Which of the following is the net ionic equation for the reaction that occurs during the titration of nitrous acid with potassium hydroxide? a) HNO 2 K OH KNO 2 H 2 O b) HNO 2 H 2 O NO 2 H 3 O c) HNO 2 KOH K NO 2 H 2 O d) HNO 2 OH NO 2 H 2 O e) H OH H 2 O. Calculate the ph of a 0.10 M solution of Ca(OH) 2. a) b) c) 0.20 d) 0.10 e) none of these 5. Which of the following is the equilibrium constant expression for the dissociation of the weak acid HOCl? a) K = [H [OCl / [HOCl b) K = [H [OCl c) K = [HOCl / [H [OCl d) K = [H [O 2 [Cl / [HOCl e) none of these answers 6. A substance that can accept an electron pair to form a covalent bond is an Arrhenius acid. b. an Arrhenius base. c. a Lewis acid. d. a BronstedLowry base. 7. Which is the WEAKEST among the following acids? HNO 2 ;.0 x 10. b. HOCl 2 ; 1.2 x c. HOCl ; 3.5 x d. HCN ;.9 x Which of the following dissociation reaction is NOT associated with the definition of K b CH 3 NH 2 H 2 O <=== CH 3 NH 3 OH b. CH 3 CH 2 NH 2 H 2 O <=== CH 3 CH 2 NH 3 OH c. HC 2 H 3 O 2 H 2 O <=== H 3 O C 2 H 3 O 2 d. d. NH 3 H 2 O <=== NH OH 9. If the [H in an aqueous solution is 2 x 10 M, then the [OH is (K w =1.0 x 10 1 ) 5 x b. 2 x c. 5 x d. 2 x e. 5 x The poh of an aqueous solution at ph = 8 is 10 b. 1 x 10 6 c. 1 x d. 6 e. 11. What is the [H of a 0.05 M solution of HNO 3 (a strong acid)? 0.02 b. 1.7 c d. 12 e

2 12. What is the poh of a M NaOH (a strong base) solution? 9.8 x 10 3 b. 1.0 x c. 2.3 d If you know Ka for acetic acid, HC 2 H 3 O 2, you can calculate the equilibrium constant, K b, for the reaction, C 2 H 3 O 2 H 2 O <== OH HC 2 H 3 O 2, by the equation: K b = K w K a b. K b = K w /K a c. K b = K w K a d. K b = K a /K w e. K b = K w K a 1. For acetic acid (HC 2 H 3 O 2 ) 1.8 x What percent of the acid has dissociated in a 0.02 M solution? 10% b. 6% c. 3 % d. 2% e. 5% 15. If K a for HCN is 6.2 x 10 10, what is K b for CN? Note: CN H 2 O <== HCN OH, K b = [HCN[OH / [CN a) 6.2 x 10 2 b) 6.2 x 10 c) 1.6 x 10 5 d) 1.6 x e) none of these 16. If 50 ml of a 0.01 M HCl solution is titrated with a 0.01 M NaOH solution, what will be the initial ph and the ph at the endpoint. 2 and 3.5 b. 2 and 7 c and 7 d. 12 and 7 e. None of these 17. What is the ph of a 1.0 M aqueous solution of NaCl? a) 7.0 b) greater than 7.0 c) less than 7.0 d) there is not enough information given 18. A 50.00mL sample of M KOH is being titrated with M HNO 3. Calculate the ph of the solution after ml of HNO 3 is added. a) 6.50 b) 3.01 c) 2.71 d) 2.1 e) none of these 19. If the following substance is dissolved in pure water, will the solution be acidic, neutral, or basic? solid sodium carbonate: (Na 2 CO 3 ). a) acidic b) neutral c) basic A solution prepared by dissolving SO 2 in water would be: acidic b. basic c. neutral d. none of the above 21. If a M solution of an acid, HCN, has a 6.2 x 10 10, the ph of the solution is:.0 b. 3.0 c d. 5.0 e The salt that forms an alkaline (basic) aqueous solution is KNO 3. b. NH Cl. c. NaC 2 H 3 O 2. d. NaCl. 23. A weak monoprotic acid (HA) is 1.1% dissociated in a 1.0 M solution. The K a for this acid is.0 x b. 5.6 x c. 2.0 x 10. d. 9.9 x Milk of magnesia has a ph of What is its [OH? 1.0 x 10 7 M b. 2.5 x 10 M c..0 x M 25. In an aqueous solution with [H =.1 x 10 9 M, [OH =2. x 10 6 M. b. the solution is basic. c. ph=8.39. d. Each statement is true. 26. A solution which is formed by combining 700. ml of 0.20 M HCl with 300. ml of 0.50 M NaOH has a [H concentration of

3 b c d e. 1.0 x What is the percent dissociation of a 0.15 M propionic acid (CH 3 CH 2 COOH) solution? ( 1.3 x 10 5 ) 0.95 b. 1.3 c. 1.8 d..5 e According to the Arrhenius acidbase theory, are responsible for the properties of acidic aqueous solutions and are responsible for the properties of basic aqueous solutions. hydrogen atoms; oxygen atoms b. oxygen atoms; hydrogen atoms c. hydronium ions; hydroxide ions d. hydronium ions; water molecules e. hydrogen ions; nitrogen atoms 29. A BronstedLowry acid is a(an) in aqueous solution and a BronstedLowry base is a(an) in aqueous solution. hydrogen atom acceptor; hydrogen atom donor b. electron acceptor; electron pair donor c. nitrogen atom donor; nitrogen atom acceptor d. hydrogen ion acceptor; nitrogen atom donor e. hydrogen ion donor; hydrogen ion acceptor 30. A BronstedLowry base must have a(an). atom that does not obey the octet rule b. nitrogen atom c. hydroxide ion d. atom with an unshared pair of electrons e. amphiprotic atom 31. All of the following can act as BronstedLowry bases except Al 3 b. H 2 O c. NH 3 3 d. PO e. HSO 32. Because water can act as a BronstedLowry acid or base, it is said to be. acidic b. amphiprotic c. basic d. strong e. weak 33. Which reaction illustrates water acting as a base? HSO H 2 O > H 3 O 2 SO b. 2 HPO H 2 O > OH H 3 PO c. NH 3 H 2 O > NH OH d. Cu(H 2 O) 2 NH 3 > Cu(NH 3 ) 2 H 2 O e. H 2 CO 3 > H 2 O CO 2 3. When the weak base pyridine reacts with water, the products are and. The formula for pyridine is C 5 H 5 N. H and OH b. H 3 O and OH c. H 3 O and C 5 H 6 N d. OH and C 5 H 6 N e. OH and C 5 H N 35. Which of the following is a conjugate acidbase pair? H and OH b. CH 3 COOH and CH 3 COO c. CH 3 COOH and OH d. CH 3 COOH and H e. CH 3 COOH and H 3 O 36. The conjugate acid of NH 3 is. NH 2 b. NH c. H d.h 3 O e. NH OH 37. Organic compounds classified as acids generally have the formula. RNH 2 b. RCOOH c. ROH d. RCHO e. CH 3 (CH 2 ) n CH Organic compounds classified as bases often have the formula. RNH 2 b. RCOOH c. ROH d. RCHO e. CH 3 (CH 2 ) n CH 39. Which of the following contributes to the acidity of the hydrogen atom in the carboxylic acid functional group?

4 33 the electronegativity of the O that is bonded to the H b. the attraction of the other atom of O for the electrons in the OH bond c. resonance stabilization of the resulting anion d. the lack of polarity in the CH bonds in the rest of the molecule e. all of these 0. The reaction between butanoic acid and water is written as. The formula for butanoic acid is CH 3 CH 2 CH 2 COOH. CH 3 CH 2 CH 2 COOH H 2 O <===> CH 2 CH 2 CH 2 COOH H 3 O b. CH 3 CH 2 CH 2 COOH H 2 O <===> CH 3 CH 2 CH 2 COO OH c. CH 3 CH 2 CH 2 COOH H 2 O <===> CH 3 CH 2 CH 2 COO H 3 O d. CH 3 CH 2 CH 2 COOH H 2 O <===> CH 3 CH 2 CH 2 COOH 2 OH e. CH 3 CH 2 CH 2 COOH H 2 O <===> CH 3 CH 2 CHCOOH H 3 O 1. The reaction between ethylamine, an organic base, and hydrochloric acid is written as. The formula for ethylamine is CH 3 CH 2 NH 2. CH 3 CH 2 NH 2 HCl <===> CH CH 2 NH 2 Cl b. CH 3 CH 2 NH 2 HCl <===> CH 3 CH 3 NH 2 Cl c. CH 3 CH 2 NH 2 2HCl <===> CH 3 CH 2 NH 2 Cl 2 d. CH 3 CH 2 NH 2 HCl <===> CH 3 CH 2 NH 3 Cl e. CH 3 CH 2 NH 2 HCl <===> CH 3 CH 2 NH H 2 Cl 2. Classify each compound as a carboxylic acid or an amine. C 6 H 5 COOH (CH 3 ) 2 NH CH 3 COOH acid, acid, amine b. amine, acid, amine c. amine, amine, acid d. acid, amine, acid e. acid, acid, acid 3. The reaction between water molecules is called, and the value of the equilibrium constant for the reaction at 25ºC is. neutralization; 1.0 x 10 6 b. autoionization; 1.0 x 10 1 c. protonation; 5.5 x 10 1 d. hydrolysis; 1.0 x 10 1 e. autoionization; 1.0 x A neutral solution is one in which [H > [OH and [H > 1.0 x 10 7 M b. [H < [OH and [H < 1.0 x 10 7 M c. [H = [OH = 1.0 x 10 7 M d. [H = [OH = 1.0 x 10 1 M e. [H = [OH = 1.0 x 10 7 M 5. An acidic solution is one in which [H > [OH and [H > 1.0 x 10 7 M b. [H < [OH and [H < 1.0 x 10 7 M c. [H = [OH = 1.0 x 10 7 M d. [H = [OH = 1.0 x 10 1 M e. [H = [OH = 1.0 x 10 7 M 6. A basic solution is one in which [H > [OH and [H > 1.0 x 10 7 M b. [H < [OH and [H < 1.0 x 10 7 M c. [H = [OH = 1.0 x 10 7 M d. [H = [OH = 1.0 x 10 1 M e. [H = [OH = 1.0 x 10 7 M 7. Calculate the ph and poh in a 1.2 M KOH solution, a strong base. ph =, and poh =.

5 3 1.2 M; 1.2 M b. 1.2 M; 8.3 x M c. 8.3 x M; 1.2 M d. 8.3 x M; 1.0 x 10 1 M e. 1.0 x 10 7 M; 1.0 x 10 7 M 8. Calculate the [H and [OH in a 1.2 M HClO solution, a strong acid. [H =, and [OH =. 1.2 M; 1.2 M b. 1.2 M; 8.3 x M c. 8.3 x M; 1.2 M d. 8.3 x M; 1.0 x 10 1 M e. 1.0 x 10 7 M; 1.0 x 10 7 M 9. Calculate the ph of a solution where [H =.6 x 10. Is this solution acidic or basic?.60; acidic b..60: basic c. 3.3; acidic d. 3.3; basic e ; acidic 50. Calculate the ph of a solution where [OH =.6 x 10. Is this solution acidic or basic?.60; basic b ; basic c ; acidic d. 3.3; basic e. 3.3; acidic 51. The ph of an egg mixture used in pet food is 6.2. Calculate the value of [H. Is the solution acidic or basic? 0.80 M; acidic b x 10 7 M; basic c x 10 7 M; acidic d. 1.7 x 10 8 M; acidic e. 1.7 x 10 8 M; basic 52. Arrange the solutions in order of increasing acidity: I. indicator with [H =.2 x 10 6 M II. lemonade, ph = 2.65 III M nitric acid IV. pickle juice, ph = 3.10 IIIIIIIV b. IIIIIIVI c. IIIVIIII d. IIVIIIII e. IVIIIIII 53. Phenolphthalein is an acidbase indicator that is colorless in its acid form and pink in its basic form, changing at ph = 8.5. Bromcresol green is yellow in its acidic form and blue in its basic form, changing at ph =.8. A solution is colorless in phenolphthalein and blue in bromcresol green. Therefore we can conclude that the ph of the solution is. less than.8 b. exactly 7.0 c. between.8 and 8.5 d. between 7.0 and 8.5 e. greater than Write the acid ionization constant expression for the ionization of acetic acid, CH 3 COOH, in aqueous solution. b. c. d. e. H [H [H H H[OH [H 2O H[H [H 2O [H 2O COOH[H O Write the acid ionization constant expression for the ionization of the hydrogen sulfate ion, HSO 2 [SO [H 2O [H O 3, in aqueous solution.

6 b. [H 2O [H 2SO [H c. [H 2SO [H d. 2 [SO [H e. [H 2SO [OH 56. Which statement about a 0.50 M sample of the weak acid, HNO 2, Ka =.5 x 10, is not correct? [H = 0.50 M. b. The acid is only slightly ionized. c. The sample contains mostly unionized HNO 2 molecules. d. The ph is slightly less than 2.0. e. [H > [OH. 57. Which acid is polyprotic? acetic acid b. nitric acid c. nitrous acid d. phosphoric acid e. perchloric acid 58. In a polyprotic acid, the value of K a1 will be the value of K a2 because. the same as; both hydrogen ions are bonded to the same anion b. larger than; it is easier to remove a hydrogen ion from a neutral molecule than from an anion c. larger than; it is easier to remove a hydrogen ion from a neutral molecule than from a cation d. smaller than; it is easier to remove a hydrogen ion from a neutral molecule than from an anion e. smaller than; it is easier to remove a hydrogen ion from a neutral molecule than from a cation 59. The ph of a solution of a 0.15 M solution of HOCl is.1. What is the Ka for HOCl? 3.5 x 10 8 b..8 x 10 c. 5.7 x 10 2 d. 7.2 x 10 5 e. 8.8 x The value of the ionization constant for HA is.2 x What is the ph of a 0.35 M solution of this acid? 3.8 x 10 b. 1.5 x 10 7 c d. 3.2 e Calculate the ph of a 0.1 M solution of an acid with Ka = 6.2 x b..03 c d e For the basic compound strychnine, the value of Kb is 1.8 x What is the ph of a M solution of this poison? 3.1 b c d e Which is the weakest acid? HBr b. HCl c. HF d. HI e. More information is needed to answer this question. 6. Which compound is the most acidic? AsH 3 b. HBr c. GeH d. H 2 Se e. More information is needed to answer this question. 65. At ph =.5, the amino acid aspartic acid will exist in its form. acidic b. basic c. resonance d. unionized e. zwitterion 66. An aqueous solution of potassium perchlorate in pure water is predicted to be. strongly acidic b. weakly acidic c. neutral d. weakly basic e. strongly basic 67. An aqueous solution of potassium benzoate is predicted to be. strongly acidic b. weakly acidic c. neutral d. weakly basic e. strongly basic 68. A solution of pyridinium hydrochloride is predicted to be. strongly acidic b. weakly acidic c. neutral d. weakly basic e. strongly basic 35

7 The reaction between the ion of a weak acid or a weak base and water is called a(an) reaction. neutralization b. autoionization c. protonation d.hydrolysis e. decomposition 70. Which compound would not be used as an antacid for the treatment of heartburn? Al(OH) 3 b. CaCO 3 c. KOH d. Mg(OH) 2 e. NaHCO Acidbase chemistry causes some baked goods to "rise" by producing carbon dioxide when an acid reacts with sodium bicarbonate in baking sod b. hydrogen gas from trace metals that react with acids in the batter. c. steam from the water formed in neutralization. d. carbon dioxide and ethanol as fermentation products. e. sulfur dioxide from sulfitecontaining foods. 72. Drain cleaners cause grease to dissolve by a(an) reaction. combustion b. esterification c. hydrogenation d. neutralization e. saponification 73. The association between a Lewis acid and a Lewis base is called a(an) bond. acidic b. coordinate covalent c. hydrogen d. ionic e. metallic 7. Metal hydroxides that can act either as Lewis acids or Lewis bases are described as. acidic b. amphoteric c. basic d. hydrated e. neutral Answers to Questions 1. e. both b and d statements. 2. c. HSO 3. d) HNO 2 OH NO 2 H 2 O. a) a) K = [H [OCl / [HOCl 6. c. a Lewis acid. 7. d. HCN ;.9 x c. HC 2 H 3 O 2 H 2 O <=== H 3 O C 2 H 3 O 2 9. e. 5 x d c c b. K b = K w /K a 1. c. 3 % 15. c) 1.6 x b) 2 and c c. basic 20. acidic 21. d c. NaC 2 H 3 O c. 2.0 x d. 5 x 10 M 25. e. Each statement is true x c. hydronium ions; hydroxide ions 29. e. hydrogen ion donor; hydrogen ion acceptor 30. d. atom with an unshared pair of electrons 31. Al b. amphiprotic 33. HSO H 2 O > 3 O 2 SO 3. d. OH and C 5 H 6 N

8 b. CH 3 COOH and CH 3 COO 36. b. NH 37. b. RCOOH 38. RNH e. all of these 0. c. CH 3 CH 2 CH 2 COOH H 2 O <===> CH 3 CH 2 CH 2 COO H 3 O 1. d. CH 3 CH 2 NH 2 HCl <===> CH 3 CH 2 NH 3 Cl 2. d. acid, amine, acid 3. b. autoionization; 1.0 x c. [H = [OH = 1.0 x 10 7 M 5. [H > [OH and [H > 1.0 x 10 7 M 6. b. [H < [OH and [H < 1.0 x 10 7 M 7. c. 8.3 x M; 1.2 M 8. b. 1.2 M; 8.3 x M 9. c. 3.3; acidic 50. b ; basic 51. c x 10 7 M; acidic 52. d. IIVIIIII 53. c. between.8 and b. 55. d. [H H 2 [SO [H 56. [H = 0.50 M. 57. d. phosphoric acid 58. b. larger than; it is easier to remove a hydrogen ion from a neutral molecule than from an anion x d b d c. HF 6. b. HBr 65. acidic 66. c. neutral 67. d. weakly basic 68. b. weakly acidic 69. d.hydrolysis 70. c. KOH 71. carbon dioxide when an acid reacts with sodium bicarbonate in baking sod 72. e. saponification 73. b. coordinate covalent 7. b. amphoteric

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