Ch. 10

16) What is the concentration of a nitric acid solution if a 10.00 mL sample of the acid requires 31.25 mL of 0.135 M KOH for neutralization? A) 0.422 M B) 0.211 M C) 0.135 M D) 0.0432 M E) 0.844 M

A) 0.422 M

80) What is the concentration of a weak base solution if a 25.0 mL sample is neutralized by 48.3 mL of 0.105 M H3PO4? A) 0.609 M B) 0.0676 M C) 0.203 M D) 0.0543 M E) 0.163 M

A) 0.609 M

52) Calculate the hydrogen ion concentration in a solution with pH = 6.35. A) 4.5 × 10^-7 M B) 2.2 × 10^-8 M C) 0.80 M D) 6.35 M E) 7.65 M

A) 4.5 × 10^-7 M

31) What is the pH of a solution in which [H3O+] = 3.8 × 10^-8 M? A) 7.42 B) 3.80 C) 6.58 D) 2.6 x 10^-7 E) 1.0 x 10^-8

A) 7.42

64) Which of the following is a strong acid? A) HNO3 B) H3PO4 C) H2O D) HCO3^- E) NH4+

A) HNO3

46) Which of the following cannot act as a Bronsted base? A) NH4+ B) CO32- C) HCO3- D) NH2- E) NH3

A) NH4+

17) What is the value of [H3O+] in a solution with pH = 10.82? A) 6.6 × 10^-4 M B) 1.5 × 10^-11 M C) 10.82 M D) 3.18 M E) 1.03 M

B) 1.5 × 10^-11 M

60) Which compound has a very large value of Ka in aqueous solution? A) KOH B) HNO3 C) NH3 D) NaCl E) H3PO4

B) HNO3

47) What is the normality of a solution containing 100 g HNO3 in 500 mL of solution? A) 1.59 N B) 0.630 N C) 3.17 N D) 0.500 N E) 1.26 N

C) 3.17 N

8) What is the hydrogen ion concentration in a solution with pH = 2.34? A) 2.34 × 10^-3 M B) 1.17 × 10^1 M C) 4.57 × 10^-3 M D) 4.27 × 10^-12 M E) 2.19 × 10^-12 M

C) 4.57 × 10^-3 M

71) What is the normality of a solution prepared by dissolving 75.0 g citric acid, a triprotic acid with molar mass of 192.14 g, in water to make 250. mL solution: A) 0.0576 N B) 0.293 N C) 4.68 N D) 0.173 N E) 1.56 N

C) 4.68 N

62) Which of the following pH's corresponds to a neutral solution? A) 1.8 B) 6.2 C) 7.0 D) 14.0 E) 8.5

C) 7.0

28) What is the conjugate acid of HSO4-? A) H3O+ B) H2SO3 C) H2SO4 D) OH- E) SO42-

C) H2SO4

77)The H3O+ ion is called the ________ ion. A) water B) hydroxide C) hydronium D) hydrogen E) protium

C) hydronium

70) Ammonia reacts with acids because A) it is neutral. B) it is itself an acid. C) it contains a lone pair of electrons. D) it contains the hydroxide group. E) it is a salt.

C) it contains a lone pair of electrons.

42) What is the conjugate acid of water? A) O2- (aq) B) H2O (l) C) OH- (aq) D) H3O+ (aq) E) H+ (aq)

D) H3O+ (aq)

78) Which of the following pH's corresponds to a strongly basic solution? A) 7.4 B) 6.9 C) 2.7 D) 4.3 E) 11.5

E) 11.5

74) Which of the following compounds is a salt? A) C6H12O6 B) HBr C) H2SO4 D) NaOH E) KNO3

E) KNO3

44) Water and HSO4- can either accept protons or donate protons. Such substances are said to be A) triprotic. B) monoprotic. C) conjugate. D) diprotic. E) amphoteric.

E) amphoteric.

19) At 25°C, the value of Kw is ________. A) 1.00 B) 1.00 × 10^14 C) 1.00 × 10^7 D)1.00 × 10^-7 E)1.00 × 10^-14

E)1.00 × 10^-14

45) How many mL of 0.100 M NaOH are needed to neutralize 50.00 mL of a 0.150 M solution ofCH3CO2H, a monoprotic acid? A) 75.00 mL B) 25.00 mL C) 37.50 mL D) 50.00 mLE)100.00 mL

A) 75.00 mL

76) All of the statements regarding equivalents of acids and bases are true except A) Equivalents are the same as moles. B) The equivalent weight of a base is the weight that produces one mole of hydroxide ions. C) Equivalents of acid are based on the number of hydrogen ions produced per formula unit of acid. D) One equivalent of any acid will neutralize one equivalent of any base. E) Equivalents are used to determine normality of solutions.

A) Equivalents are the same as moles.

32) Which of the following is a triprotic acid? A) H3PO4 B) NH3 C)CH3COOH D) Al(OH)3 E) HNO3

A) H3PO4

38) The net ionic equation for the reaction of formic acid, a weak acid, with potassium hydroxide, a strong base, is A) HCO2H (aq) + OH- (aq) → HCO2- (aq) + H2O (l) B) HCO2H (aq) + K+ (aq) + OH- (aq) → K+ (aq) + HCO2- (aq) + H2O (l) C) HCO2H (aq) + KOH (aq) → KHCO2 (aq) + H2O (l) D) H+ (aq) + HCO2- (aq) + K+ (aq) + OH- (aq) → K+ (aq) + HCO2- (aq) + H2O (l) E) HCO2- (aq) + KOH (aq) → KHCO2 (aq) + OH- (aq)

A) HCO2H (aq) + OH- (aq) → HCO2- (aq) + H2O (l)

3) Which net ionic equation correctly represents the neutralization of a solution of barium hydroxide by a solution of nitric acid? A) H^1+ + OH-→ H2O B) Ba^2+ + 2 NO3-→ Ba(NO3)2 C) Ba(NO3)2+ H2O → Ba2++ 2 NO3- D) H^1++ NO3-→ HNO3 E) Ba2++ 2 OH-→ Ba(OH)2

A) H^1+ + OH-→ H2O

5) Which compound produces an acidic solution when dissolved in water? A) NH4Cl B) Ca(NO3)2 C) KCl D) NaF E) K2SO4

A) NH4Cl

33) Which of the following compounds is a salt? A) NH4NO3 B) Al(OH)3 C)C6H6 D)CH3CO2HE)NH3

A) NH4NO3

22) A necessary requirement for a Bronsted base is A) a lone pair of electrons in its Lewis dot structure. B) the presence of water as a reaction medium. C) the presence of a metal ion in its formula. D) the presence of hydroxide in its formula. E) the production of hydronium ion upon reaction with water.

A) a lone pair of electrons in its Lewis dot structure.

56) A Bronsted-Lowry base is a substance which A) accepts protons from other substances. B) produces hydrogen ions in aqueous solution. C) donates protons to other substances. D) accepts hydronium ions from other substances.E)produces hydroxide ions in aqueous solution.

A) accepts protons from other substances.

53) Acetic acid is a weak acid in water because it is A) only slightly dissociated into ions. B) only slightly soluble. C) dilute. D) completely dissociated into hydronium ions and acetate ions. E) unable to hold onto its hydrogen ion.

A) only slightly dissociated into ions.

75) According to Bronsted-Lowry theory, acid-base reactions can be described as ________ reactions. A) proton transfer B) gas phase C) nuclear transfer D) electron transfer E) electrolytic

A) proton transfer

54) Which example is not basic? A) vinegar B) limewater C) window cleaner D) shampoo E) Mg(OH)2, used in remedies for upset stomach

A) vinegar

10) The pH of a solution with [H+] = 5.9 × 10-3 M, to the correct number of significant figures, is________. A) 2.2 B) 2.23 C) 1.01 D) 5.9 × 10-3E)2.229

B) 2.23

59) What is the normality of a solution prepared by dissolving 37.5 g citric acid, a triprotic acid with molar mass of 192.14 g, in water to make 250. mL solution: A) 0.288 N B) 2.35 N C) 0.780 N D) 0.0865 N E) 0.147 N

B) 2.35 N

67) Which of the following pH's corresponds to a weakly acidic solution? A) 1.4 B) 5.3 C) 7.8 D) 11.5 E)9.2

B) 5.3

61) What is the pH of a solution in which the hydrogen ion concentration is 5.1 × 10^-8 M? A) 1.96 × 10^-7 B) 7.29 C) 8.90 D) 5.10 E) 6.71

B) 7.29

24) Which of the following is a weak acid? A) HCl B) H3PO4 C) OH- D) HNO3 E) NH3

B) H3PO4

26)Which of the following statements is correct? A) In a basic solution, [H3O+] > 10^-7; [OH-] > 10^-7. B) In a basic solution, [H3O+] < 10^-7; [OH-] > 10^-7. C) In a basic solution, [H3O+] > 10^-7; [OH-] = 10-7. D) In a basic solution, [H3O+] < 10-7; [OH-] < 10^-7. E) In a basic solution, [H3O+] > 10^-7; [OH-] < 10^-7.

B) In a basic solution, [H3O+] < 10^-7; [OH-] > 10^-7.

30) Which statement is correct for pure water? A) Pure water contains larger amounts of hydroxide, [OH-], ions than hydronium, [H3O+], ions. B) Pure water contains equal amounts of hydroxide, [OH-], and hydronium, [H3O+], ions. C) Pure water contains no ions. D) Pure water is an electrolyte. E) Pure water contains larger amounts of hydronium, [H3O+], ions than hydroxide, [OH-], ions.

B) Pure water contains equal amounts of hydroxide, [OH-], and hydronium, [H3O+], ions.

34) What is the conjugate base of HSO4-? A) H2SO3 B) SO4^2- C) H3O+ D) OH- E) H2SO4

B) SO4^2-

29) What is the concentration of a phosphoric acid solution of a 25.00 mL sample of the acid requires 42.24 mL of 0.135 M NaOH for neutralization? A) 0.684 M B) 0.228 M C) 0.0760 M D) 0.0266 M E) 0.0799 M

C) 0.0760 M

72) What is the concentration of a solution of HCl in which a 10.0 mL sample of acid required 50.0 mL of 0.150 M NaOH for neutralization? A) 0.60 M B) 7.5 M C) 0.75 M D) 0.15 M E) 0.030 M

C) 0.75 M

18) If the [H+] of a water sample is 1 × 10^-4 M, the [OH-] is A) 1 × 10^-14 M. B) 1 × 10^4 M. C) 1 × 10^-10 M. D) 1 × 10^-4 M. E) none of the above

C) 1 × 10^-10 M.

37) If the concentration of H3O+ in an aqueous solution is 7.6 × 10-9 M, the concentration of OH- is________. A) 7.6 × 10^-9 M B) 7.6 × 10^-23 M C) 1.3 × 10^-6 M D) 6.4 × 10^-5 M E) 1.3 × 10^+8 M

C) 1.3 × 10^-6 M

39) What is the pH of a solution in which [H3O+] = 4.1 × 10^-2 M? A) 12.90 B) 12.61 C) 1.39 D) 1.10 E) 4.10

C) 1.39

55) How many mL of 0.360 M HNO3 are needed to neutralize a 22.5 mL sample of 0.240 M KOH? A) 22.5 mL B) 33.8 mL C) 15.0 mL D)62.5 mL E)5.40 mL

C) 15.0 mL

49) What is the [H3O+] in a solution with pH = 11.61? A) 4.07 × 10^-3 M B) 1.16 × 10^+1 M C) 2.45 × 10^-12 M D) 1.00 × 10^-14 M E) 2.39 × 10^+1 M

C) 2.45 × 10^-12 M

14) If the concentration of H3O+ is 3.5 × 10-3 M, the concentration of OH- is ________ M. A) 3.5 × 10^-11 B) 10.5 × 10^-3 C) 2.9 × 10^-12 D) 1.0 × 10^-7 E) 1.0 × 10^-12

C) 2.9 × 10^-12

11) What is the pH of a solution in which [H3O^1+] = 1.2 × 10^-3 M? A) 8.33 × 10-12 B) 11.08 C) 2.92 D) 12.80 E) 1.20

C) 2.92

4) If the [H+] of a water sample is 1 × 10^-4 M, the pH of the sample is ________, and the sample is________. A) 10; basic B) -10; basic C) 4; acidic D) -4; acidicE)4; basic

C) 4; acidic

68) How many mL of 0.150 M NaOH are needed to neutralize 50.00 mL of a 0.120 M solution ofH2SO4? A) 50.00 mL B) 40.00 mL C) 80.00 mL D) 160.00 mL E) 120.00 mL

C) 80.00 mL

82) Which compound produces a basic solution when dissolved in water? A) NH4Cl B) KClO4 C) NaF D) Ca(NO3)2 E) KCl

C) NaF

7)Which example is not acidic? A) lake water that turns blue litmus to red B) orange juice C) a solution in which [H3O+] = 1.00 x 10^-7 D) soil for azaleas with pH of 4.8 E) a solution of NH4NO3 with pH < 7.00

C) a solution in which [H3O+] = 1.00 x 10^-7

23) A buffer solution A) neutralizes only acids. B) is a salt solution. C) closely maintains its original pH. D) maintains pH at 7.00. E) is a strong base.

C) closely maintains its original pH.

6) In an aqueous solution that is acidic, [H3O^+] is ________ than 1.0 x 10^-7 and ________ than [OH-]. A) less; greater B) less; less C) greater; greater D) greater; less E) none of the above

C) greater; greater

85) In an aqueous solution that is basic, [H3O+] is ________ than 1.0 × 10^-7 and ________ than [OH-]. A) less; greater B) greater; greater C) less; less D) greater; less E) none of the above

C) less; less

57) How many mL of 0.241 M H2SO4 will be needed to neutralize a 50.0 mL sample of 0.191 M KOH? A) 79.3 mL B) 39.6 mL C) 31.5 mL D) 19.8 mL E) 126 mL

D) 19.8 mL

35) Which equation correctly represents the neutralization of aluminum hydroxide by sulfuric acid? A) Al(OH)3+H3SO4→ AlSO4+ 3 H2O B) 2 Al(OH)3^+ 3 H2SO4→Al2(SO4)^3+ 3 H2O C) Al(OH)2+H2SO4→ AlSO4+ 2 H2O D) 2 Al(OH)3+ 3 H2SO4→ Al2(SO4)3+ 6 H2O E) 3 Al(OH)3+ 2 H3SO4→ Al3(SO4)2+ 6 H2O

D) 2 Al(OH)3+ 3 H2SO4→ Al2(SO4)3+ 6 H2O

48) The pH of a cup of coffee is measured as 5.45. Express this measurement as [H+], using the correct number of significant figures. A) 3.548 × 10^-6 M B) 3.55 × 10^-6 M C) 2.82 × 10^5 M D) 3.5 × 10^-6 M E) 4 × 10^-6 M

D) 3.5 × 10^-6 M

50) How many mL of 0.100 M NaOH are needed to neutralize 24.0 mL of 0.150 M HCl? A) 12.0 mL B) 48.0 mL C) 24.0 mL D) 36.0 mL E) 18.0 mL

D) 36.0 mL

36) The normality of a solution prepared by dissolving 50.0 g of Ca(OH)2 in water to make 250. mL solution is ________ N. A) 7.02 B) 2.70 C) 3.51 D) 5.40 E) 1.35

D) 5.40

51) Which compound has a value of Ka that is close to 10^-5? A) NaCl B) NH3 C) HNO3 D) CH3CH2CO2H E) KOH

D) CH3CH2CO2H

79) Which pair of compounds is used in the manufacture of fertilizers? A) HNO3 and HCl B) HCl and H3PO4 C) HNO3 and NaOH D) H2SO4 and H3PO4 E) HCl and NaOH

D) H2SO4 and H3PO4

86) Which substance produces carbon dioxide and water upon reaction with an acid? A) H2C2O4 B) C8H18 C) NH4NO3 D) MgCO3 E) NaCH3CO2

D) MgCO3

63) Which of the following solutions is a buffer? A) a solution of acetic acid and sodium sulfate B) a solution of sulfuric acid and sodium sulfate C) a solution of hydrochloric acid and sodium sulfate D) a solution of acetic acid and sodium acetate E) a solution of hydrochloric acid and sodium acetate

D) a solution of acetic acid and sodium acetate

66) A Bronsted-Lowry acid is a substance which A) accepts hydronium ions from other substances. B) produces hydroxide ions in aqueous solution. C) produces hydrogen ions in aqueous solution. D) donates protons to other substances. E) accepts protons from other substances.

D) donates protons to other substances.

65) When acids and bases react the product other than water is a A) hydronium ion. B) metal. C) hydroxide ion. D) salt. E) hydrogen ion.

D) salt.

83) Which of the following is a diprotic acid? A) nitric acid B) acetic acid C) phosphoric acid D) sulfuric acid E)hydrochloric acid

D) sulfuric acid

69) If the concentration of OH- is 1 × 10^-2 M, the concentration of H3O+ is ________ M. A) 1 × 10^-7 B) 1 × 10^0 C) 1 × 10^-14 D) 1 × 10^-2 E) 1 × 10^-12

E) 1 × 10^-12

73) What is the normality of a solution containing 49 g of H2SO4 in enough water to make 400 mL of solution? A) 5.0 N B) 1.0 N C) 0.20 N D) 10 N E) 2.5 N

E) 2.5 N

1) The normality of a solution prepared by dissolving 25.0 g of Ca(OH)2 in water to make 250. mL solution is ________ N. A) 1.35 B) 1.75 C) 3.51 D)0.675 E) 2.70

E) 2.70

84) If the concentration of OH- in an aqueous solution is 1.4 × 10^-7 M, the concentration of H3O+ is________. A) 7.1 × 10^+6 M B) 1.0 × 10^-7 M C) 1.4 × 10^-7 M D) 1.3 × 10^-8 M E) 7.1 × 10^-8 M

E) 7.1 × 10^-8 M

13) The pH of a 250. mL sample of a buffer solution is 9.85. If 1.0 mL of 6 M HCl is added, the pH of there sulting mixture is closest to A) 7.00 B) 10.00 C) 1.65 D) 0.00 E) 9.70

E) 9.70

12) Which compound is manufactured in larger quantities in the U.S. than any other industrial chemical? A) HNO3 B) HCl C) H3PO4 D) NaOH E) H2SO4

E) H2SO4

41) Which solution is basic? A) [OH-] = 1.0 × 10^-10 B) [H3O+] = 1.0 × 10^-4 C) [OH-] = 1.0 × 10^-7 D) [H3O+] = 1.0 × 10^-7 E) [H3O+] = 1.0 × 10^-10

E) [H3O+] = 1.0 × 10^-10

15) The base forms a new ________ bond in a Bronsted-Lowry acid-base reaction. A) hydrogen B) ionic C) metallic D) aquo E) covalent

E) covalent

58) Which statement concerning Arrhenius acid-base theory is not correct? A) An Arrhenius base produces hydroxide ions in water solution. B) Acid-base reactions must take place in aqueous solution. C) An Arrhenius acid produces hydrogen ions in water solution. D) A neutralization reaction produces water plus a salt. E) none of the above

E) none of the above

9) All of the following species are involved in the blood buffer system except ________. A) CO2 B) HCO3- C) CO32- D) H2CO3 E) none of the above

E) none of the above

2) To prepare a buffer using sodium phosphate, which of the following would also be needed? A) hydrochloric acid B) ammonium phosphate C) sodium hydroxide D) ammonium hydroxide E) phosphoric acid

E) phosphoric acid

20) Which of the following statements is correct? A)In an acidic solution, [H3O+] > 10^-7; [OH-] = 10^-7. B)In an acidic solution, [H3O+] > 10^-7; [OH-] > 10-7. C)In an acidic solution, [H3O+] < 10^-7; [OH-] > 10^-7. D)In an acidic solution, [H3O+] < 10^-7; [OH-] < 10^-7. E)In an acidic solution, [H3O+] > 10^-7; [OH-] < 10^-7.

E)In an acidic solution, [H3O+] > 10^-7; [OH-] < 10^-7.