Chapter 14 Review Questions

General Chemistry: Atoms First, 2e (McMurry and Fay)Chapter 14 Aqueous Equilibria: Acids and Bases

14.1 Multiple Choice Questions

1) An Arrhenius acid is best defined as aA) hydroxide donor.B) proton acceptor.C) substance that dissociates in water to produce aqueous hydrogen ions.D) substance that dissociates in water to produce aqueous hydroxide ions.Answer: CDiff: 1Topic: Section 14.1 Acid-Base Concepts: The Brønsted-Lowry Theory

2) When dissolved in water, which of the following compounds is an Arrhenius acid?A) HCNB) NaOHC) NaFD) CH3CH2OHAnswer: ADiff: 2Topic: Section 14.1 Acid-Base Concepts: The Brønsted-Lowry TheoryAlgo. Option: algorithmic

3) An Arrhenius base is best defined as aA) proton donor.B) hydroxide acceptor.C) substance that dissociates in water to produce aqueous hydrogen ions.D) substance that dissociates in water to produce aqueous hydroxide ions.Answer: DDiff: 1Topic: Section 14.1 Acid-Base Concepts: The Brønsted-Lowry Theory

4) When dissolved in water, which of the following compounds is an Arrhenius base?A) CH3OHB) HOClC) KOHD) KClAnswer: CDiff: 2Topic: Section 14.1 Acid-Base Concepts: The Brønsted-Lowry Theory

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5) A Brønsted-Lowry acid is best defined as a substance that canA) accept a hydroxide ion.B) donate a hydroxide ion.C) accept a proton.D) donate a proton.Answer: DDiff: 1Topic: Section 14.1 Acid-Base Concepts: The Brønsted-Lowry Theory

6) Which one of the following species acts as a Brønsted-Lowry acid in water?A) NaHB) NH4+

C) CH3NH2D) C6H6Answer: BDiff: 2Topic: Section 14.1 Acid-Base Concepts: The Brønsted-Lowry Theory

7) In the following chemical equation indicate the reactant that is a Brønsted-Lowry acidHCN(aq) + H2O(l) H⇌ 3O+(aq) + CN-(aq).

A) HCNB) H2O

C) H3O+

D) CN-Answer: ADiff: 2Topic: Section 14.1 Acid-Base Concepts: The Brønsted-Lowry Theory

8) Indicate all the Brønsted-Lowry acids in the following chemical reactionHCl(aq) + H2O(aq) H⇌ 3O+(aq) + Cl-(aq).

A) HCl, H2OB) HCl, C) HCl, Cl-

D) HCl, H2O, H3O+

Answer: BDiff: 2Topic: Section 14.1 Acid-Base Concepts: The Brønsted-Lowry Theory


9) What are the Brønsted-Lowry bases in the following chemical reaction C5H5N(aq) + H2O(l) C⇌ 5H5NH+(aq) + OH-(aq)?

A) C5H5N, H2O

B) C5H5N, C5H5NH+

C) C5H5N,

D) C5H5N, H2O, OH-

Answer: CDiff: 2Topic: Section 14.1 Acid-Base Concepts: The Brønsted-Lowry Theory

10) What are the Brønsted-Lowry acids in the following chemical reactionHBr(sol) + CH3COOH(sol) CH⇌ 3C(OH)2+(sol) + Br-(sol)?

A) HBr, CH3COOHB) HBr, C) CH3COOH, CH3C(OH)2+

D) CH3COOH, Br-


11) What are the conjugate acid-base pairs in the following chemical reactionNH3(aq) + H2O(l) NH⇌ 4+(aq) + OH-(aq)?

A) NH3, H2O and NH4+, OH-

B) NH3, NH4+ and H2O, OH-

C) NH3, OH- and H2O, NH4+

D) NH3 and NH4+


12) Identify the conjugate acid/base pairs present in an aqueous solution of hydrogen sulfate ion, HSO4-.

A) HSO4-/SO42- and H3O+/H2O

B) H2SO4/HSO4- and H2O/OH-

C) HSO4-/H2O and H3O+/SO42-

D) HSO4-/H2O and H2SO4/OH-

Answer: ADiff: 2Topic: Section 14.1 Acid-Base Concepts: The Brønsted-Lowry Theory


13) What is the conjugate base of the Brønsted-Lowry acid HPO42-?A) H3PO4B) H2PO4-

C) HPO42-

D) PO43-

Answer: DDiff: 2Topic: Section 14.1 Acid-Base Concepts: The Brønsted-Lowry Theory

14) What is the conjugate acid of the Brønsted-Lowry base HAsO42-?

A) H2AsO4-

B) AsO43-

C) H2O

D) H3O+

Answer: ADiff: 2Topic: Section 14.1 Acid-Base Concepts: The Brønsted-Lowry Theory

15) Which one of the following can behave either as a Brønsted-Lowry acid or a Brønsted-Lowry base in an aqueous solution reaction?A) HSO3-

B) NH3C) HID) H3PO4Answer: ADiff: 2Topic: Section 14.1 Acid-Base Concepts: The Brønsted-Lowry Theory

16) Write a balanced equation for the dissociation of the Brønsted-Lowry acid HSO4- in water.

A) HSO4-(aq) + H2O(l) H⇌ 2SO4(aq) + OH-(aq)

B) HSO4-(aq) + H2O(l) SO⇌ 42-(aq) + H3O+(aq)

C) HSO4-(aq) + H2O(l) SO⇌ 32-(aq) + OH-(aq)

D) HSO4-(aq) + H2O(l) SO⇌ 3(g) + OH-(aq) + H2O(l)Answer: BDiff: 2Topic: Section 14.1 Acid-Base Concepts: The Brønsted-Lowry Theory


17) Which of the following Brønsted-Lowry acids does not behave as a strong acid when it is dissolved in water?A) HB) HClC) HNO2D) HClO4Answer: CDiff: 2Topic: Section 14.2 Acid Strength and Base StrengthAlgo. Option: algorithmic

18) Which Brønsted -Lowry base has the strongest conjugate acid?A) CH3CO2-

B) CN-

C) F-

D) NO3-

Answer: DDiff: 2Topic: Section 14.2 Acid Strength and Base Strength

19) Which Brønsted-Lowry acid has the strongest conjugate base?A) HClB) HClO4C) HFD) HAnswer: CDiff: 2Topic: Section 14.2 Acid Strength and Base Strength

20) What is the strongest Brønsted-Lowry acid in the chemical reaction shown below?2 HNO3(aq) + Ba(OH)2(aq) → Ba(NO3)2(aq) + 2 H2O(l)

A) HNO3B) Ba(OH)2C) Ba(NO3)2D) H2OAnswer: ADiff: 2Topic: Section 14.2 Acid Strength and Base Strength


21) From the following chemical reactions determine the relative Brønsted-Lowry acid strengths (strongest to weakest).

HCl(aq) + H2O(l) → H3O+(aq) + Cl-(aq)

HCN(aq) + H2O(l) H⇌ 3O+(aq) + CN-(aq)

A) HCl > HCN > H3O+

B) HCl > H3O+ > HCN

C) H3O+ > HCl > HCN

D) HCN > H3O+ > HClAnswer: BDiff: 3Topic: Section 14.2 Acid Strength and Base Strength


HClO4(aq) + H2O(l) → H3O+(aq) + ClO4-(aq)

HNO2(aq) + H2O(l) H⇌ 3O+(aq) + NO2-(aq)

A) HClO4 > H3O+ > HNO2B) HClO4 > HNO2 > H3O+

C) H3O+ > HClO4 > HNO2D) H3O+ > HNO2 > HClO4Answer: ADiff: 3Topic: Section 14.2 Acid Strength and Base Strength


HClO4(sol) + CH3COOH(l) → CH3C2(OH)2+(sol) + ClO4-(aq)

H2SO4(sol) + CH3COOH(l) CH⇌ 3C(OH)2+(sol) + HSO4-(sol)A) HClO4 > H2SO4 > CH3COOH

B) HClO4 > H2SO4 > CH3C(OH)2+

C) HClO4 > CH3COOH > H2SO4D) HClO4 > CH3C(OH)2+ > H2SO4Answer: DDiff: 3Topic: Section 14.2 Acid Strength and Base Strength


24) From the following chemical reactions determine the relative Brønsted-Lowry base strengths (strongest to weakest).

HNO3(aq) + H2O(l) → H3O+(aq) + NO3-(aq)

HF(aq) + H2O(l) H⇌ 3O+(aq) + F-(aq)

A) HNO3 > H3O+ > HF

B) NO3- > H2O > F-

C) F- > H2O > NO3-

D) F- > NO3- > H2OAnswer: CDiff: 3Topic: Section 14.2 Acid Strength and Base Strength

25) From the following chemical reactions determine the relative Brønsted-Lowry base strengths (strongest to weakest).

2 NaH(s) + H2O(l) → 2 NaOH + H2(g)

NH3(aq) + H2O(l) NH⇌ 4+(aq) + OH-(aq)

A) H- > OH- > NH3B) H- > NH3 > OH-

C) OH-> H- > NH3D) OH- > NH3 > H-

Answer: ADiff: 3Topic: Section 14.2 Acid Strength and Base Strength

26) The equilibrium constant, K, for the reaction shown below has a value 1.8 × 10–5. In this reaction which is the strongest acid and which is the strongest base?

CH3CO2H(aq) + H2O(l) H⇌ 3O+(aq) + CH3CO2–(aq)

A) CH3CO2H and CH3CO2– B) CH3CO2H and H2O

C) H3O+ and H2O

D) H3O+ and CH3CO2–

Answer: DDiff: 3Topic: Section 14.2 Acid Strength and Base Strength


The following pictures represent aqueous solutions of binary acids of the type HA where the water molecules have been omitted for clarity.

27) Determine the strongest acid of the set.A) AB) BC) CD) DAnswer: BDiff: 2Topic: Section 14.2 Acid Strength and Base Strength

28) Arrange the acids in order of increasing acid strength.A) D < C < A < BB) D < C < B < AC) D < B < A < CD) D < A < C < BAnswer: DDiff: 3Topic: Section 14.2 Acid Strength and Base Strength

29) What is the geometric shape of the hydrated proton; that is, the hydronium ion H3O+?A) angularB) trigonal pyramidalC) trigonal planarD) tetrahedralAnswer: BDiff: 2Topic: Section 14.3 Factors That Affect Acid Strength


30) An acidic solution at 25°C hasA) [H3O+] > [OH-] > 1 × 10-7 M.

B) [H3O+] > 1 × 10-7 M > [OH-].

C) [H3O+] = [OH-] > 1 × 10-7 M.

D) [H3O+] < 1 × 10-7 M > [OH-].Answer: BDiff: 1Topic: Section 14.4 Dissociation of Water

31) At 50°C the value of Kw is 5.5 × 10-14. A basic solution at 50°C has

A) [H3O+] < [OH-] < 2.3 × 10-7 M.

B) [H3O+] < 2.3 × 10-7 M < [OH-].

C) [H3O+] = [OH-] < 2.3 × 10-7 M.

D) [H3O+] > 2.3 × 10-7 M < [OH-].Answer: BDiff: 2Topic: Section 14.4 Dissociation of Water

32) Calculate the hydronium ion concentration in an aqueous solution that contains 2.50 × 10-4 M in hydroxide ion.A) 4.00 × 10-9 MB) 4.00 × 10-10 MC) 4.00 × 10-11 MD) 5.00 × 10-11 MAnswer: CDiff: 2Topic: Section 14.4 Dissociation of WaterAlgo. Option: algorithmic

33) Calculate the hydroxide ion concentration in an aqueous solution that contains 3.50 × 10-3 M in hydronium ion.A) 2.86 × 10-4 MB) 2.86 × 10-11 MC) 2.86 × 10-12 MD) 3.50 × 10-12 MAnswer: CDiff: 2Topic: Section 14.4 Dissociation of WaterAlgo. Option: algorithmic


34) A solution with a hydrogen ion concentration of 3.25 × 10-2 M is ________ and has a hydroxide concentration of ________.A) acidic, 3.08 × 10-12 MB) acidic, 3.08 × 10-13 MC) basic, 3.08 × 10-12 MD) basic, 3.08 × 10-13 MAnswer: BDiff: 2Topic: Section 14.4 Dissociation of WaterAlgo. Option: algorithmic

35) A solution with a hydroxide ion concentration of 4.15 × 10-4 M is ________ and has a hydrogen ion concentration of ________.A) acidic, 2.41 × 10-10 MB) acidic, 2.41 × 10-11 MC) basic, 2.41 × 10-10 MD) basic, 2.41 × 10-11 MAnswer: DDiff: 2Topic: Section 14.4 Dissociation of WaterAlgo. Option: algorithmic

36) If the ionization constant of water, Kw, at 40°C is 2.92 × 10-14, then what is the hydronium ion concentration for a neutral solution?A) [H3O+] < 1.00 × 10-7 M

B) [H3O+] > 1.71 × 10-7 M

C) [H3O+] = 1.71 × 10-7 M

D) [H3O+] < 1.71 × 10-7 MAnswer: CDiff: 2Topic: Section 14.4 Dissociation of Water

37) An acidic solution at 25°C will have a hydronium ion concentration ________ and a pH value ________.A) [H3O+] > 1 × 10-7 M, pH > 7.00

B) [H3O+] > 1 × 10-7 M, pH < 7.00

C) [H3O+] < 1 × 10-7 M, pH > 7.00

D) [H3O+] < 1 × 10-7 M, pH < 7.00Answer: BDiff: 1Topic: Section 14.5 The pH Scale


38) If the ionization constant of water, Kw, at 40°C is 2.92 × 10-14, then what is the hydronium ion concentration and pH for an acidic solution?A) [H3O+] > 1.71 × 10-7 M and pH > 6.77

B) [H3O+] > 1.71 × 10-7 M and pH < 6.77

C) [H3O+] < 1.71 × 10-7 M and pH > 6.77

D) [H3O+] < 1.71 × 10-7 M and pH < 6.77Answer: BDiff: 2Topic: Section 14.5 The pH Scale

39) Calculate the pH for an aqueous solution of acetic acid that contains hydronium ion.A) 4.65 × 10-12

B) 2.15 × 10-3C) 2.67D) 11.33Answer: CDiff: 2Topic: Section 14.5 The pH ScaleAlgo. Option: algorithmic

40) Calculate the pH for an aqueous solution of pyridine that contains hydroxide ion.A) 4.65 × 10-11

B) 2.15 × 10-4 C) 3.67D) 10.33Answer: DDiff: 2Topic: Section 14.5 The pH ScaleAlgo. Option: algorithmic

41) What is the hydroxide ion concentration and the pH for a hydrochloric acid solution that has a hydronium ion concentration of A) 6.67 × 10-10 M, 4.82B) 6.67 × 10-10 M, 9.18C) 6.67 × 10-11 M, 3.82D) 6.67 × 10-11 M, 10.18Answer: CDiff: 2Topic: Section 14.5 The pH ScaleAlgo. Option: algorithmic


42) What is the hydronium ion concentration and the pH for an aqueous solution of NH3 that has a hydroxide ion concentration ofA) 4.44 × 10-11 M, 3.65B) 4.44 × 10-11 M, 10.35C) 4.44 × 10-12 M, 2.65D) 4.44 × 10-12 M, 11.35Answer: DDiff: 2Topic: Section 14.5 The pH ScaleAlgo. Option: algorithmic

43) What is the hydronium ion concentration of an acid rain sample that has a pH of 3.15?A) 1.41 × 10-11 MB) 7.08 × 10-4 M C) 3.15 MD) 10.85 MAnswer: BDiff: 2Topic: Section 14.5 The pH ScaleAlgo. Option: algorithmic

44) What is the hydroxide ion concentration of a lye solution that has a pH of 11.20?A) 6.31 × 10-12 MB) 1.58 × 10-3 MC) 2.80 M D) 11.20 MAnswer: BDiff: 2Topic: Section 14.5 The pH ScaleAlgo. Option: algorithmic

45) What statement is most consistent for an acid with a pH = 3?A) one one-hundredth as strong as an acid with a pH of 5B) half a strong as an acid with a pH = 5C) twice as strong as an acid with a pH of 5D) one hundred times as strong as an acid with a pH = 5Answer: DDiff: 2Topic: Section 14.5 The pH Scale


46) At 25°C, the pH of a vinegar solution is 2.60. What are the values of [H3O+] and [OH-] in the solution?A) 3.99 × 10-12 M, 2.51 × 10-3 MB) 2.51 × 10-3 M, 3.98 × 10-12 MC) 2.51 × 10-3 M, 11.40 MD) 2.60 M, 11.40 MAnswer: BDiff: 2Topic: Section 14.5 The pH Scale

47) What is the approximate pH of a solution X that gives the following responses with the indicators shown?

IndicatorsHIn — In-

pH range

Solution X

methyl orange red-yellow 3.2-4.4 yellow

methyl red red-yellow 4.8-6.0 yellow

bromthymol blue yellow-blue 6.0-7.6 green

phenolphthalein colorless-pink 8.2-10.0 colorless

A) 3.2 - 4.4 B) 4.8 - 6.0 C) 6.0 - 7.6D) 8.2 - 10.0Answer: CDiff: 2Topic: Section 14.6 Measuring pH




pH range

Solution X


methyl red red-yellow 4.8-6.0 orange

bromthymol blue yellow-blue 6.0-7.6 yellow

phenolphthalein colorless-pink 8.2-10.0 colorless

A) 3.2 - 4.4B) 4.8 - 6.0C) 6.0 - 7.6D) 8.2 - 10.0Answer: BDiff: 2Topic: Section 14.6 Measuring pH



pH range

Solution X


methyl red red-yellow 4.8-6.0 yellow

bromthymol blue yellow-blue 6.0-7.6 blue

phenolphthalein colorless-pink 8.2-10.0 pink

A) 4.8 - 6.0B) 6.0 - 7.6C) 7.6 - 8.2D) > 8.2Answer: DDiff: 2Topic: Section 14.6 Measuring pH


50) What is the pH of a 0.020 M HClO4 solution?A) 0.020B) 0.040C) 1.70D) 12.30Answer: CDiff: 2Topic: Section 14.7 The pH in Solutions of Strong Acids and Strong BasesAlgo. Option: algorithmic

51) What is the pH of a 0.020 M RbOH solution?A) 0.020B) 0.040C) 1.70D) 12.30Answer: DDiff: 2Topic: Section 14.7 The pH in Solutions of Strong Acids and Strong Bases

52) What is the pH of a 0.020 M Ba(OH)2 solution?A) 1.40B) 1.70C) 12.30D) 12.60Answer: DDiff: 3Topic: Section 14.7 The pH in Solutions of Strong Acids and Strong BasesAlgo. Option: algorithmic

53) What is the pH of a solution prepared by dissolving 0.15 gram of solid CaO (lime) in enough water to make 2.00 L of aqueous Ca(OH)2 (limewater)?

CaO(s) + H2O(l) → Ca2+(aq) + 2 OH-(aq)A) 2.57B) 2.87C) 11.13D) 11.43Answer: DDiff: 3Topic: Section 14.7 The pH in Solutions of Strong Acids and Strong BasesAlgo. Option: algorithmic


54) What is the pH of a solution prepared by diluting 25.00 mL of 0.10 M HCl with enough water to produce a total volume of 100.00 mL?A) 1.00B) 1.60C) 2.00D) 3.20Answer: BDiff: 3Topic: Section 14.7 The pH in Solutions of Strong Acids and Strong BasesAlgo. Option: algorithmic

55) What is the pH of a solution prepared by diluting 25.00 mL of 0.020 M Ba(OH)2 with enough water to produce a total volume of 250.00 mL?A) 2.40B) 2.70C) 11.30D) 11.60Answer: DDiff: 3Topic: Section 14.7 The pH in Solutions of Strong Acids and Strong BasesAlgo. Option: algorithmic

56) What is the pH of a solution made by mixing 100.00 mL of 0.20 M HCl with 50.00 mL of 0.10 M HCl? Assume that the volumes are additive.A) 0.15B) 0.52C) 0.78D) 1.70Answer: CDiff: 3Topic: Section 14.7 The pH in Solutions of Strong Acids and Strong BasesAlgo. Option: algorithmic

57) What is the pH of a solution made by mixing 100.0 mL of 0.10 M HNO3, 50.0 mL of 0.20 M HCl, and 100.0 mL of water? Assume that the volumes are additive.A) 0.30B) 0.82C) 1.00D) 1.10Answer: DDiff: 3Topic: Section 14.7 The pH in Solutions of Strong Acids and Strong BasesAlgo. Option: algorithmic


58) What is the pH of a solution prepared by mixing 100.00 mL of 0.020 M Ca(OH)2 with 50.00 mL of 0.100 M NaOH? Assume that the volumes are additive.A) 12.67B) 12.78C) 12.95D) 13.25Answer: BDiff: 3Topic: Section 14.7 The pH in Solutions of Strong Acids and Strong BasesAlgo. Option: algorithmic

59) What is the equilibrium constant expression (Ka) for the acid dissociation of hydrocyanic acid HCN? The equation of interest is

HCN(aq) + H2O(l) H⇌ 3O+(aq) + CN-(aq).

A) Ka = ([H3O+][CN-])/([HCN][H2O])

B) Ka = ([H3O+][CN-])/([HCN])

C) Ka = ([HCN][H2O])/([H3O+][CN-])

D) Ka = ([HCN])/([H3O+][CN-])Answer: BDiff: 2Topic: Section 14.8 Equilibria in Solutions of Weak Acids

60) What is the equilibrium constant expression (Ka) for the acid dissociation of nitrous acid HNO2? The equation of interest is

HNO2(aq) + H2O(l) H⇌ 3O+(aq) + NO2-(aq).

A) Ka = ([H3O+][NO2-])/([HNO2][H2O])

B) Ka = ([H3O+][NO2-])/([HNO2])

C) Ka = ([HNO2][H2O])/([H3O+][NO2-])

D) Ka = ([HNO2])/([H3O+][NO2-])Answer: BDiff: 2Topic: Section 14.8 Equilibria in Solutions of Weak Acids

61) Determine the acid dissociation constant for a 0.10 M acetic acid solution that has a pH of 2.87. Acetic acid is a weak monoprotic acid and the equilibrium equation of interest is

A) 1.3 × 10-2 B) 1.3 × 10-3

C) 1.8 × 10-5 D) 1.8 × 10-6Answer: CDiff: 3


Topic: Section 14.8 Equilibria in Solutions of Weak Acids

62) Determine the acid dissociation constant for a 0.010 M nitrous acid solution that has a pH of 2.70. Nitrous acid is a weak monoprotic acid and the equilibrium equation of interest is

A) 8.0 × 10-3

B) 2.0 × 10-3

C) 5.0 × 10-4

D) 4.0 × 10-4Answer: CDiff: 3Topic: Section 14.8 Equilibria in Solutions of Weak Acids

63) Determine the acid dissociation constant for a 0.020 M formic acid solution that has a pH of 2.74. Formic acid is a weak monoprotic acid and the equilibrium equation of interest is

A) 1.8 × 10-3

B) 1.8 × 10-4

C) 3.6 × 10-4

D) 3.6 × 10-5Answer: BDiff: 3Topic: Section 14.8 Equilibria in Solutions of Weak Acids

64) The pH of 0.255 M HCN is 4.95. What is the value of Ka for hydrocyanic acid?

A) 1.3 × 10-10

B) 4.9 × 10-10

C) 1.1 × 10-5


65) The pH of 0.150 M CH3CO2H, acetic acid, is 2.78. What is the value of Ka for acetic acid?

A) 2.8 × 10-6

B) 1.9 × 10-5

C) 1.7 × 10-3



66) What is the strongest monoprotic acid of the following set if all the acids are at 0.100 M concentration?A) hydrofluoric acid with Ka = 3.5 × 10-4

B) benzoic acid with Ka = 6.5 × 10-5

C) acetic acid with Ka = 1.8 × 10-5

D) hypochlorous acid with Ka = 3.5 × 10-8

Answer: ADiff: 1Topic: Section 14.8 Equilibria in Solutions of Weak Acids

67) What is the hydronium ion concentration of a 0.100 M acetic acid solution with a Ka = 1.8 ×

10-5? The equation for the dissociation of acetic acid is:CH3CO2H(aq) + H2O(l) ⇌ H3O+(aq) + CH3CO2-(aq).

A) 1.3 × 10-2 MB) 4.2 × 10-2 MC) 1.3 × 10-3 MD) 4.2 × 10-3 MAnswer: CDiff: 3Topic: Section 14.9 Calculating Equilibrium Concentrations in Solutions of Weak AcidsAlgo. Option: algorithmic

68) The p of HCN is 9.31. What is the pH of a 0.52 M solution of HCN?A) 4.80B) 5.20C) 6.79D) 6.33Answer: ADiff: 3Topic: Section 14.9 Calculating Equilibrium Concentrations in Solutions of Weak Acids

69) The of hypochlorous acid, HOCl, is 3.5 × . What is the pH of 0.78 M HOCl?A) 3.78B) 3.50C) 2.82D) 2.53Answer: ADiff: 3Topic: Section 14.9 Calculating Equilibrium Concentrations in Solutions of Weak Acids


70) What is the p of hypobromous acid, HOBr, if a 0.40 M HOBr has a pH of 4.50?A) 8.60B) 4.50C) 6.11D) 4.92Answer: ADiff: 3Topic: Section 14.9 Calculating Equilibrium Concentrations in Solutions of Weak Acids

71) What is the hydronium ion concentration of a 0.100 M hypochlorous acid solution with The equation for the dissociation of hypochlorous acid is:

HOCl(aq) + H2O(l) ⇌ H3O+(aq) + OCl-(aq).

A) 1.9 × 10-4

B) 5.9 × 10-4

C) 1.9 × 10-5

D) 5.9 × 10-5Answer: DDiff: 3Topic: Section 14.9 Calculating Equilibrium Concentrations in Solutions of Weak AcidsAlgo. Option: algorithmic

72) Para-Aminobenzoic acid (PABA), p-H2NC6H4(COOH), is used in some sunscreens and hair conditioning products. Calculate the pH of an aqueous solution with and

A) 1.52B) 3.09C) 4.66D) 6.18Answer: BDiff: 3Topic: Section 14.9 Calculating Equilibrium Concentrations in Solutions of Weak Acids

73) A tablet containing 500.0 mg of aspirin (acetylsalicylic acid or was dissolved in enough water to make 100 mL of solution. Given that Ka = 3.0 × 10–4 for aspirin, what is the pH of the solution?A) 1.57B) 2.54C) 3.52D) 5.08Answer: BDiff: 4Topic: Section 14.9 Calculating Equilibrium Concentrations in Solutions of Weak Acids


74) Benzoic acid (C6H5CO2H = HBz) solutions are sometimes used in experiments to determine the molarity of a basic solution of unknown concentration. What is the pH of a 0.100 M solution of benzoic acid if and the equilibrium equation of interest is

A) 1.00B) 2.59C) 4.19D) 5.19Answer: BDiff: 4Topic: Section 14.9 Calculating Equilibrium Concentrations in Solutions of Weak Acids

75) Potassium hydrogen phthalate (molar mass = 204.2 g/mol) is one of the most commonly used acids for standardizing solutions containing bases. KHP is a monoprotic weak acid with

Calculate the pH of the solution that results when 0.40 g of KHP is dissolved in enough water to produce 25.0 mL of solution.A) 2.10B) 3.26C) 4.30D) 5.41Answer: BDiff: 4Topic: Section 14.9 Calculating Equilibrium Concentrations in Solutions of Weak AcidsAlgo. Option: algorithmic

76) Vinegar is a 5.0% solution by weight of acetic acid (CH3CO2H) in water. Given that

for acetic acid and assuming the density of vinegar to be 1.00 g/cm3, what is the pH of this vinegar solution?A) 2.00B) 2.41C) 2.87D) 4.74Answer: BDiff: 4Topic: Section 14.10 Percent Dissociation in Solutions of Weak Acids


77) Vinegar is a 5.0% solution by weight of acetic acid (CH3CO2H) in water. Given that the pH

for acetic acid is 2.41, the and assuming the density of vinegar to be 1.00 g/cm3, what is the percent dissociation of acetic acid in vinegar?A) 0.47%B) 1.5%C) 4.0%D) 5.0%Answer: ADiff: 4Topic: Section 14.10 Percent Dissociation in Solutions of Weak Acids

78) What is the percent dissociation of a benzoic acid solution with pH = 2.59? The acid dissociation constant for this monoprotic acid is A) 0.50%B) 1.5%C) 2.5%D) 3.5%Answer: CDiff: 4Topic: Section 14.10 Percent Dissociation in Solutions of Weak Acids

79) The percent dissociation of acetic acid changes as the concentration of the acid decreases. A 100-fold decrease in acetic acid concentration results in a ________ fold ________ in the percent dissociation.A) 10, increaseB) 10, decreaseC) 100, increaseD) 100, decreaseAnswer: ADiff: 3Topic: Section 14.10 Percent Dissociation in Solutions of Weak Acids

80) Which of the following are weak diprotic acids?A) carbonic acid - H2CO3, hydrosulfuric acid - H2S, acetic acid - CH3CO2HB) formic acid - HCO2H, acetic acid CH3CO2H, benzoic acid C6H5CO2HC) carbonic acid - H2CO3, oxalic acid - H2C2O4, sulfurous acid - H2SO3D) hydrocyanic acid - HCN, sulfuric acid - H2SO4, phosphoric acid - H3PO4Answer: CDiff: 2Topic: Section 14.11 Equilibria in Solutions of Polyprotic Acids


81) What is the second stepwise equilibrium constant expression for phosphoric acid H3PO4?

A) Ka2 = ([H3O+][H2PO4-])/([H3PO4])

B) Ka2 = ([H3O+]2[HPO42-])/([H3PO4])

C) Ka2 = ([H3O+]3[PO43-])/([H3PO4])

D) Ka2 = ([H3O+][HPO42-])/([H2PO4-])Answer: DDiff: 2Topic: Section 14.11 Equilibria in Solutions of Polyprotic Acids

82) Calculate the pH of a 0.020 M carbonic acid solution, H2CO3(aq), that has the stepwise

dissociation constants and A) 1.70B) 4.03C) 6.37D) 10.25Answer: BDiff: 3Topic: Section 14.11 Equilibria in Solutions of Polyprotic AcidsAlgo. Option: algorithmic

83) Calculate the pH of a 0.20 M H2SO3 solution that has the stepwise dissociation constants

Ka1 = 1.5 × 10-2 and Ka2 = 6.3 × 10-8.A) 1.26B) 1.32C) 1.82D) 2.52Answer: ADiff: 3Topic: Section 14.11 Equilibria in Solutions of Polyprotic AcidsAlgo. Option: algorithmic

84) Calculate the concentration of bicarbonate ion, HCO3-, in a 0.010 M H2CO3 solution that

has the stepwise dissociation constants and

A) 6.6 × 10-5 MB) 4.3 × 10-7 MC) 4.3 × 10-9 MD) 5.6 × 10-11 MAnswer: ADiff: 3Topic: Section 14.11 Equilibria in Solutions of Polyprotic AcidsAlgo. Option: algorithmic


85) What is the pH of a 0.10 M H2Se solution that has the stepwise dissociation constants Ka1 =

1.3 × 10-4 and Ka2 = 1.0 × 10-11? A) 2.44B) 3.89C) 4.89D) 5.50Answer: ADiff: 3Topic: Section 14.11 Equilibria in Solutions of Polyprotic AcidsAlgo. Option: algorithmic

86) What is the selenide ion concentration [Se2-] for a 0.100 M H2Se solution that has the

stepwise dissociation constants of Ka1 = 1.3 × 10-4 and Ka2 = 1.0 × 10-11?

A) 3.6 × 10-3 MB) 1.3 × 10-4 MC) 1.3 × 10-5 MD) 1.0 × 10-11 MAnswer: DDiff: 3Topic: Section 14.11 Equilibria in Solutions of Polyprotic AcidsAlgo. Option: algorithmic

87) Which of the following can be classified as a weak base?A) CH3NH2B) NH2OHC) Both CH3NH2 and NH2OHD) Neither CH3NH2 nor NH2OHAnswer: CDiff: 2Topic: Section 14.12 Equilibria in Solutions of Weak Bases

88) What is the pH of a 0.100 M NH3 solution that has Kb = 1.8 × 10-5 ? The equation for the dissociation of NH3 is

A) 1.87B) 2.87C) 11.13D) 12.13Answer: CDiff: 3Topic: Section 14.12 Equilibria in Solutions of Weak BasesAlgo. Option: algorithmic


89) What is the concentration of N in a 0.20 M ammonia solution? The base dissociaton constant for ammonia is 1.8 × .A) 0.0019 MB) 0.20 MC) 0.020 MD) 0.040 MAnswer: ADiff: 3Topic: Section 14.12 Equilibria in Solutions of Weak Bases

90) The concentration of C N in a 0.20 M methylamine (C ) solution is 2.32 × M. What is for methylamine?A) 2.7 × B) 5.4 × C) 1.2 ×D) 3.3 × Answer: ADiff: 3Topic: Section 14.12 Equilibria in Solutions of Weak Bases

91) What is the pH of a 0.30 M pyridine solution that has a Kb = 1.9 × 10-9 ? The equation for the dissociation of pyridine is


92) Aniline, (C6H5NH2, Kb = 4.3 × 10-10 at 25°C) is an industrially important amine used in the making of dyes. Determine the pH of an aniline solution made by dissolving 3.90 g of aniline in enough water to make 100 mL of solution. A) 4.87B) 9.13C) 9.74D) 10.74Answer: BDiff: 4Topic: Section 14.12 Equilibria in Solutions of Weak BasesAlgo. Option: algorithmic


93) Determine the ammonia concentration of an aqueous solution that has a pH of 11.50. The equation for the dissociation of NH3 (Kb = 1.8 × 10-5) is

A) 2.5 MB) 0.55 MC) 5.7 × 10-3 MD) 3.2 × 10-3 MAnswer: BDiff: 4Topic: Section 14.12 Equilibria in Solutions of Weak BasesAlgo. Option: algorithmic

94) How many grams of pyridine are there in 100 mL of an aqueous solution that has a pH of 9.00? The Kb for pyridine is 1.9 × and the equation of interest is

C5H5N(aq) + H2O(l) C⇌ 5H5NH+(aq) + OH-(aq).A) 0.053 gB) 0.42 gC) 0.79 gD) 7.9 gAnswer: BDiff: 4Topic: Section 14.12 Equilibria in Solutions of Weak Bases

95) What is the relationship between Ka and Kb at 25°C for a conjugate acid base pair?

A) Ka × Kb = 1 × 10-14

B) Ka/Kb = 1 × 10-14

C) Kb/Ka = 1 × 10-14

D) Ka + Kb = 1 × 10-14

Answer: ADiff: 1Topic: Section 14.13 Relation Between Ka and Kb

96) Ammonia NH3, has a base dissociation constant of 1.8 × 10-5. What is the conjugate acid of ammonia and what is its acid dissociation constant?A) NH4+, 1.9 × 109

B) NH4+, 1.8 × 10-5

C) NH4+, 5.6 × 10-10

D) NH2-, 5.6 × 10-10

Answer: CDiff: 2Topic: Section 14.13 Relation Between Ka and Kb


97) Methylamine CH3NH2, has a base dissociation constant of 3.7 × 10-4. What is the conjugate acid of methylamine and what is its acid dissociation constant?A) CH3NH3+, 2.7 × 103

B) CH3NH3+, 3.7 × 10-4

C) CH3NH3+, 2.7 × 10-11

D) CH3NH2-, 2.7 × 10-11

Answer: CDiff: 2Topic: Section 14.13 Relation Between Ka and Kb

98) Acetic acid CH3COOH, has an acid dissociation constant of 1.8 × 10-5. What is the conjugate base of acetic acid and what is its base dissociation constant?A) CH3C(OH)2+, 5.6 × 104

B) CH3C(OH)2+, 5.6 × 10-10

C) CH3COOH, 5.6 × 10-10

D) CH3CO2-, 5.6 × 10-10

Answer: DDiff: 2Topic: Section 14.13 Relation Between Ka and Kb

99) Dihydrogen phosphate H2PO4-, has an acid dissociation constant of What is the

conjugate base of H2PO4- and what is its base dissociation constant?

A) H3PO4, 1.6 × 106

B) H3PO4, 1.6 × 10-8

C) HPO42-, 1.6 × 106

D) HPO42-, 1.6 × 10-8

Answer: DDiff: 2Topic: Section 14.13 Relation Between Ka and Kb

100) Which of the following salts are acidic?A) LiCl, NaCl, KClB) NH4Cl, CuCl2, AlCl3 C) NaCH3CO2, KCH3CO2, RbCH3CO2D) NaCl, NH4Cl, Na2CO3Answer: BDiff: 3Topic: Section 14.14 Acid-Base Properties of Salts


101) Which one of the following salts, when dissolved in water, produces the solution with the highest pH?A) NaHSO4B) LiClO4C) MgOD) CH3NH3IAnswer: CDiff: 3Topic: Section 14.14 Acid-Base Properties of SaltsAlgo. Option: algorithmic

102) If an equal number of moles of the weak acid HCN and the strong base KOH are added to water, is the resulting solution acidic, basic, or neutral?A) acidicB) basicC) neutralD) There is insufficient information provided to answer this question.Answer: BDiff: 2Topic: Section 14.14 Acid-Base Properties of SaltsAlgo. Option: algorithmic

103) Arrange the following 0.10 M aqueous solutions in order of increasing pH: NaOH, HBr, NaCH3CO2, KBr, NH4Br.A) HBr, KBr, NH4Br, NaCH3CO2, NaOHB) NaOH, NaCH3CO2, NH4Br, KBr, HBrC) NaOH, NaCH3CO2, KBr, NH4Br, HBrD) HBr, NH4Br, KBr, NaCH3CO2, NaOHAnswer: DDiff: 3Topic: Section 14.14 Acid-Base Properties of Salts

104) Which one of the following salts, when dissolved in water, produces the solution with the highest pH?A) KIB) KBrC) KClD) KFAnswer: DDiff: 3Topic: Section 14.14 Acid-Base Properties of SaltsAlgo. Option: algorithmic


105) Which one of the following salts, when dissolved in water, produces the solution with a pH closest to 7.00?A) NH4ClB) BaOC) NaHSO4D) RbIAnswer: DDiff: 3Topic: Section 14.14 Acid-Base Properties of SaltsAlgo. Option: algorithmic

106) Calculate the pH of a 0.100 M NaCH3CO2 solution. Ka for acetic acid, CH3CO2H, is

A) 2.87B) 5.13C) 8.87D) 11.13Answer: CDiff: 5Topic: Section 14.14 Acid-Base Properties of SaltsAlgo. Option: algorithmic

107) Calculate the pH of a of 0.100 M KBrO solution. Ka for hypobromous acid, HBrO, is

A) 3.15B) 4.85C) 9.15D) 10.85Answer: DDiff: 5Topic: Section 14.14 Acid-Base Properties of SaltsAlgo. Option: algorithmic

108) Calculate the pH of a 0.100 M CH3NH3Cl solution. Kb for methylamine, CH3NH2, is

A) 2.22B) 5.78C) 8.22D) 11.78Answer: BDiff: 5Topic: Section 14.14 Acid-Base Properties of SaltsAlgo. Option: algorithmic


109) Equal volumes of 0.10 M NH3 (Kb = 1.8 × 10-5) and 0.10 M HCN (Ka = 4.9 × 10-10) are mixed together. Will the resulting solution be acidic, basic, or neutral?A) acidicB) basicC) neutralD) insufficient information to solveAnswer: BDiff: 3Topic: Section 14.14 Acid-Base Properties of Salts

110) Which one of the following salts, when dissolved in water, produces the solution with the lowest pH?A) NaClB) NH4ClC) MgCl2D) AlCl3Answer: DDiff: 3Topic: Section 14.14 Acid-Base Properties of SaltsAlgo. Option: algorithmic

111) What is the identity of M in the hydrate M(H2O)6n+ that has the 0.10 M solution with the lowest pH?A) Li+

B) Na+

C) Mg2+

D) Al3+Answer: DDiff: 3Topic: Section 14.14 Acid-Base Properties of Salts

112) What is the identity of M in the hydrate M(H2O)6n+ that has the 0.10 M solution with the highest pH?A) Li+

B) Na+

C) Mg2+

D) Al3+Answer: BDiff: 3Topic: Section 14.14 Acid-Base Properties of Salts


113) What is the strongest acid among the following?A) HFB) HClC) HBrD) HIAnswer: DDiff: 2Topic: Section 14.3 Factors That Affect Acid Strength

114) What is the strongest acid among the following?A) H2OB) H2SC) H2SeD) H2TeAnswer: DDiff: 2Topic: Section 14.3 Factors That Affect Acid Strength

115) What is the strongest acid among the following?A) HFB) HClC) H2OD) H2SAnswer: BDiff: 2Topic: Section 14.3 Factors That Affect Acid Strength

116) What is the weakest acid among the following?A) SiH4B) PH3C) H2SD) HClAnswer: ADiff: 2Topic: Section 14.3 Factors That Affect Acid Strength

117) Which acid of the following set has the strongest conjugate base?A) CH4B) NH3C) H2OD) HFAnswer: ADiff: 3Topic: Section 14.3 Factors That Affect Acid Strength


118) What is the strongest base among the following?A) ClO-

B) ClO2-

C) ClO3-

D) ClO4-

Answer: ADiff: 3Topic: Section 14.3 Factors That Affect Acid Strength

119) What is the strongest acid among the following?A) H2SO3B) H2SO4C) H2SeO3D) H2SeO4Answer: BDiff: 3Topic: Section 14.3 Factors That Affect Acid Strength

120) What is the strongest acid of the following?A) HOIB) HOBrC) HOClD) All are equivalent.Answer: CDiff: 2Topic: Section 14.3 Factors That Affect Acid Strength

121) What is the strongest acid among the following?A) HIOB) HIO2C) HIO3D) HIO4Answer: DDiff: 2Topic: Section 14.3 Factors That Affect Acid Strength

122) What is the strongest acid among the following?A) CH3CO2HB) ClCH2CO2HC) Cl2CHCO2HD) Cl3CCO2HAnswer: DDiff: 3Topic: Section 14.3 Factors That Affect Acid Strength


123) Identify the Lewis acid that acts as a reactant in the following reaction Fe(H2O)63+(aq) + 6 CN-(aq) → Fe(CN)63-(aq) + 6 H2O(l).

A) Fe3+B) H2O

C) CN-

D) Fe(H2O)63+

Answer: ADiff: 3Topic: Section 14.15 Lewis Acids and Bases

124) Identify the Lewis acid that acts as a reactant in the following reactionCo(H2O)63+(aq) + 6 NH3(aq) → Co(NH3)63+(aq) + 6 H2O(l).

A) Co(H2O)63+

B) Co3+C) NH3D) H2OAnswer: BDiff: 3Topic: Section 14.15 Lewis Acids and Bases

125) For Cu2+ and CO2, which will behave as a Lewis acid toward OH- in water?

A) only Cu2+B) only CO2C) Cu2+ and CO2D) neither Cu2+ nor CO2Answer: CDiff: 3Topic: Section 14.15 Lewis Acids and Bases

126) Which one of the following is not considered to be a Lewis base?A) H2OB) NH3C) NH4+

D) Cl-Answer: CDiff: 3Topic: Section 14.15 Lewis Acids and Bases


127) Which one of the following is least able to behave as a Lewis base?A) CH3NH2B) (CH3)2NHC) (CH3)3N

D) (CH3)3NH+

Answer: DDiff: 3Topic: Section 14.15 Lewis Acids and Bases

128) The compound BF3 can be described as a(n)A) Arrhenius acid.B) Brønsted-Lowry acid.C) Lewis acid.D) Lewis base.Answer: CDiff: 3Topic: Section 14.15 Lewis Acids and Bases

129) Identify the set of Lewis acids.A) BH3, BF3, Cu2+, CO2B) Cl-, OH-, NH3, H2O

C) H3PO4, H2PO4-, HPO42-, PO43-

D) CH3-, NH2-, OH-, F-

Answer: ADiff: 3Topic: Section 14.15 Lewis Acids and Bases

130) Which one of the following is expected to be the strongest Lewis acid?A) FeB) Fe+

C) Fe2+

D) Fe3+Answer: DDiff: 3Topic: Section 14.15 Lewis Acids and Bases


In the following reaction the unshaded spheres represent H atoms.

131) Identify the Brønsted-Lowry acids.A) (1) and (3)B) (1) C) (2) and (3)D) (2) and (4)Answer: BDiff: 2Topic: Conceptual Problems

132) Identify the Brønsted-Lowry bases.A) (1) and (3)B) (1) and (4)C) (2) D) (2) and (4)Answer: CDiff: 2Topic: Conceptual Problems



133) Identify the Brønsted-Lowry acids.A) (1) and (3)B) (1) and (4)C) (2) D) (2) and (4)Answer: CDiff: 2Topic: Conceptual Problems

134) Identify the Brønsted-Lowry bases.A) (1) and (3)B) (1) C) (2) and (3)D) (2) and (4)Answer: BDiff: 2Topic: Conceptual Problems



135) Identify the Brønsted-Lowry acid/base conjugate pairs.A) (1)/(2) and (3)/(4)B) (1)/(3) and (2)/(4)C) (1)/(4) and (2)/(3)Answer: BDiff: 2Topic: Conceptual Problems


136) Identify the Brønsted-Lowry acid/base conjugate pairs.A) (1)/(2) and (3)/(4)B) (1)/(3) and (2)/(4)C) (1)/(4) and (2)/(3)Answer: BDiff: 2Topic: Conceptual Problems


The following pictures represent aqueous solutions of three acids HA (A = X, Y, or Z); water molecules have been omitted for clarity.

137) Arrange the three acids in order of increasing acid strength.A) HZ < HY < HXB) HY < HZ < HXC) HZ < HX < HYD) HX < HZ < HYAnswer: DDiff: 2Topic: Conceptual Problems

138) Which acid, if any, is a strong acid?A) All are strong acids.B) HX and HZC) HYD) None are strong acids.Answer: CDiff: 2Topic: Conceptual Problems

139) Which acid has the smallest value of Ka?A) HXB) HYC) HZD) All have the same Ka value.Answer: ADiff: 2


Topic: Conceptual Problems

140) Which acid has the lowest percent dissociation?A) HXB) HYC) HZD) All have the same percent dissociation.Answer: ADiff: 2Topic: Conceptual Problems

141) Which acid solution has the lowest pH?A) HXB) HYC) HZD) All have the same pH.Answer: BDiff: 2Topic: Conceptual Problems


142) Which of the above pictures represents a solution of a weak diprotic acid H2A for which (Water molecules have been omitted for clarity.)

A) picture (a)B) picture (b)C) picture (c)D) picture (d)Answer: CDiff: 3Topic: Conceptual Problems

143) Which of the above pictures represents a solution of a diprotic acid H2A for which and Ka2 is exceptionally small. (Water molecules have been omitted for clarity.)A) picture (a)B) picture (b)C) picture (c)D) picture (d)Answer: BDiff: 3Topic: Conceptual Problems


The following pictures represent equal volumes of aqueous solutions of three acids HA (A = X, Y, or Z); water molecules have been omitted for clarity.

144) Arrange the acids in order of increasing acid strength.A) HZ < HY < HXB) HY < HZ < HXC) HZ < HX < HYD) HX < HZ < HYAnswer: BDiff: 2Topic: Conceptual Problems

145) Arrange the acids in order of increasing value of Ka.A) Ka(HZ) < Ka(HY) < Ka(HX)B) Ka(HY) < Ka(HZ) < Ka(HX)C) Ka(HZ) < Ka(HX) < Ka(HY)D) Ka(HX) < Ka(HZ) < Ka(HY)Answer: BDiff: 2Topic: Conceptual Problems

146) Arrange the acids in order of increasing value of percent dissociation.A) HZ < HY < HXB) HY < HZ < HXC) HZ < HX < HYD) HX < HZ < HYAnswer: BDiff: 2Topic: Conceptual Problems


147) Arrange the acids in order of increasing pH.A) HZ < HY < HXB) HY < HZ < HXC) HZ < HX < HYD) HX < HZ < HYAnswer: DDiff: 2Topic: Conceptual Problems

148) Arrange the conjugate bases (A- = X-, Y-, or Z-) in order of increasing base strength.A) Z- < Y- < X-

B) Y- < Z- < X-

C) Z- < X- < Y-

D) X- < Z- < Y-Answer: DDiff: 3Topic: Conceptual Problems

149) Arrange the conjugate bases (A- = X-, Y-, or Z-) in order of increasing value of Kb.

A) Kb(Z-) < Kb(Y-) < Kb(X-)

B) Kb(Y-) < Kb(Z-) < Kb(X-)

C) Kb(Z-) < Kb(X-) < Kb(Y-)

D) Kb(X-) < Kb(Z-) < Kb(Y-)Answer: DDiff: 3Topic: Conceptual Problems


150) The following pictures represent solutions of three salts NaA (A- = X-, Y-, or Z-); water molecules and Na+ ions have been omitted for clarity. Arrange the three A- ions in order of decreasing base strength.

A) X- > Y- > Z-

B) X- > Z- > Y-

C) Y- > Z- > X-

D) Z- > Y- > XZ-Answer: BDiff: 2Topic: Conceptual Problems


The following pictures represent solutions of three salts MA; water molecules have been omitted for clarity. Dotted spheres represent Ay- ions; gray spheres represent Mx+ ions; black spheres represent oxygen atoms; and unshaded spheres represent hydrogen atoms.

151) Which picture represents an acidic salt?A) (1)B) (2)C) (3)D) none of the aboveAnswer: BDiff: 3Topic: Conceptual Problems

152) Which picture represents a neutral salt?A) (1)B) (2)C) (3)D) none of the aboveAnswer: CDiff: 3Topic: Conceptual Problems

153) Which picture represents a basic salt?A) (1)B) (2)C) (3)D) none of the aboveAnswer: ADiff: 3Topic: Conceptual Problems


154) Of the elements indicated on the periodic table shown above, which forms the strongest binary acid, H2X or HX, where A) AB) BC) CD) DAnswer: DDiff: 3Topic: Conceptual Problems

155) Of the elements indicated on the periodic table shown above, which forms the weakest binary acid, H2X or HX, where A) AB) BC) CD) DAnswer: ADiff: 3Topic: Conceptual Problems

156) Of the elements indicated on the periodic table shown above, which forms the strongest oxoacid acid with the formula H2XO3 or HXO3, where A) AB) BC) CD) DAnswer: BDiff: 3Topic: Conceptual Problems


157) Of the elements indicated on the periodic table shown above, which forms the weakest oxoacid acid with the formula H2XO3 or HXO3, where A) AB) BC) CD) DAnswer: CDiff: 3Topic: Conceptual Problems

158) SO3 reacts with H2O to form H2SO4. Which picture below correctly represents the curved arrow notation for the initial Lewis acid-Lewis base interaction in this reaction; what is the Lewis acid and the Lewis base?

A) Picture (1) is correct; H2O is the Lewis acid and SO3 is the Lewis base.B) Picture (1) is correct; SO3 is the Lewis acid and H2O is the Lewis base.C) Picture (2) is correct; H2O is the Lewis acid and SO3 is the Lewis base.D) Picture (2) is correct; SO3 is the Lewis acid and H2O is the Lewis base.Answer: DDiff: 4Topic: Conceptual Problems


159) CO2 reacts with H2O to form HCO3- and H+. Which picture below correctly represents the curved arrow notation for the initial Lewis acid-Lewis base interaction in this reaction; what is the Lewis acid and the Lewis base?

(1) (2)

A) Picture (1) is correct; H2O is the Lewis acid and CO2 is the Lewis base.B) Picture (1) is correct; CO2 is the Lewis acid and H2O is the Lewis base.C) Picture (2) is correct; H2O is the Lewis acid and CO2 is the Lewis base.D) Picture (2) is correct; CO2 is the Lewis acid and H2O is the Lewis base.Answer: BDiff: 4Topic: Conceptual Problems

160) BF3 and NH3 undergo a Lewis acid-base reaction forming an adduct. Which picture below correctly represents the curved arrow notation for the initial Lewis acid-Lewis base interaction in this reaction; what is the Lewis acid and the Lewis base?

A) Picture (1) is correct; NH3 is the Lewis acid and BF3 is the Lewis base.B) Picture (2) is correct; BF3 is the Lewis acid and NH3 is the Lewis base.C) Picture (3) is correct; NH3 is the Lewis acid and BF3 is the Lewis base.D) Picture (4) is correct; BF3 is the Lewis acid and NH3 is the Lewis base.Answer: BDiff: 4Topic: Conceptual Problems


14.2 Algorithmic Questions

1) When dissolved in water, which compound is generally considered to be an Arrhenius acid? A) H NO2 B) KOHC) Li F D) CH3OH Answer: ADiff: 2Topic: Section 14.1 Acid-Base Concepts: The Brønsted-Lowry TheoryAlgo. Option: algorithmic

2) Calculate the hydronium ion concentration in an aqueous solution that contains 2.50 × 10-6 M in hydroxide ion.A) 4.00 × 10-7 MB) 4.00 × 10-8 MC) 4.00 × 10-9 MD) 5.00 × 10-9 MAnswer: CDiff: 2Topic: Section 14.4 Dissociation of WaterAlgo. Option: algorithmic

3) Calculate the hydroxide ion concentration in an aqueous solution that contains 3.50 × 10-4 M in hydronium ion.A) 2.86 × 10-3 MB) 2.86 × 10-10 MC) 2.86 × 10-11 MD) 3.50 × 10-11 MAnswer: CDiff: 2Topic: Section 14.4 Dissociation of WaterAlgo. Option: algorithmic


4) A solution with a hydrogen ion concentration of 3.25 × 10-6 M is ________ and has a hydroxide ion concentration of ________. A) acidic, 3.08 × 10-8 MB) acidic, 3.08 × 10-9 MC) basic, 3.08 × 10-8 MD) basic, 3.08 × 10-9 MAnswer: BDiff: 2Topic: Section 14.4 Dissociation of WaterAlgo. Option: algorithmic

5) A solution with a hydroxide ion concentration of 4.15 × 10-6 M is ________ and has a hydrogen ion concentration of ________. A) acidic, 2.41 × 10-8 MB) acidic, 2.41 × 10-9 MC) basic, 2.41 × 10-8 MD) basic, 2.41 × 10-9 MAnswer: DDiff: 2Topic: Section 14.4 Dissociation of WaterAlgo. Option: algorithmic

6) Calculate the pH for an aqueous solution of acetic acid that contains hydronium ion. A) 4.65 × 10-12 MB) 2.15 × 10-3 MC) 2.67D) 11.33Answer: CDiff: 2Topic: Section 14.5 The pH ScaleAlgo. Option: algorithmic

7) Calculate the pH for an aqueous solution of pyridine that contains hydroxide ion.A) 4.65 × 10-11

B) 2.15 × 10-4 C) 3.67D) 10.33Answer: DDiff: 2Topic: Section 14.5 The pH ScaleAlgo. Option: algorithmic


8) What is the hydroxide ion concentration and the pH for a hydrochloric acid solution that has a hydronium ion concentration of

A) 6.67 × 10-12 M, 2.82B) 6.67 × 10-12 M, 11.18C) 6.67 × 10-13 M, 1.82D) 6.67 × 10-13 M, 12.17Answer: CDiff: 2Topic: Section 14.5 The pH ScaleAlgo. Option: algorithmic

9) What is the hydronium ion concentration and the pH for an aqueous solution of NH3 that has

a hydroxide ion concentration of

A) 4.44 × 10-12 M and 2.65B) 4.44 × 10-12 M and 11.35C) 4.44 × 10-13 M and 1.65D) 4.44 × 10-13 M and 12.35Answer: DDiff: 2Topic: Section 14.5 The pH ScaleAlgo. Option: algorithmic

10) What is the hydronium ion concentration of an acid rain sample that has a pH of 3.45? A) 2.82 × 10-11 MB) 3.55 × 10-4 M C) 3.45 MD) 10.55 MAnswer: BDiff: 2Topic: Section 14.5 The pH ScaleAlgo. Option: algorithmic

11) What is the hydroxide ion concentration of a lye solution that has a pH of 9.20? A) 6.31 × 10-10 MB) 1.58 × 10-5 MC) 4.80 M D) 9.20 MAnswer: BDiff: 2Topic: Section 14.5 The pH ScaleAlgo. Option: algorithmic


12) What is the pH of a 0.020 M HClO4 solution?A) 0.020B) 0.040C) 1.70D) 12.30Answer: CDiff: 2Topic: Section 14.7 The pH in Solutions of Strong Acids and Strong BasesAlgo. Option: algorithmic

13) What is the pH of a 0.040 M Ba(OH)2 solution?A) 1.10B) 1.40C) 12.60D) 12.90Answer: DDiff: 3Topic: Section 14.7 The pH in Solutions of Strong Acids and Strong BasesAlgo. Option: algorithmic

14) What is the pH of a solution prepared by dissolving 0.45 grams of solid CaO (lime) in enough water to make 2.00 L of aqueous Ca(OH)2 (limewater)?

CaO(s) + H2O(l) → Ca2+(aq) + 2 OH-(aq)A) 2.10B) 2.40C) 11.60D) 11.90Answer: DDiff: 3Topic: Section 14.7 The pH in Solutions of Strong Acids and Strong BasesAlgo. Option: algorithmic

15) What is the pH of a solution prepared by diluting 20.00 mL of 0.10 M HCl with enough water to produce a total volume of 100.00 mL?A) 1.00B) 1.70C) 2.00D) 3.40Answer: BDiff: 3Topic: Section 14.7 The pH in Solutions of Strong Acids and Strong BasesAlgo. Option: algorithmic


16) What is the pH of a solution prepared by diluting 100.00 mL of 0.020 M Ba(OH)2 with enough water to produce a total volume of 250.00 mL?A) 1.80B) 2.10C) 11.90D) 12.20Answer: DDiff: 3Topic: Section 14.7 The pH in Solutions of Strong Acids and Strong BasesAlgo. Option: algorithmic

17) What is the pH of a solution prepared by mixing 100.00 mL of 0.20 M HCl with 150.00 mL of 0.10 M HCl? Assume that the volumes are additive. A) 0.17B) 0.52C) 0.85D) 1.70Answer: CDiff: 3Topic: Section 14.7 The pH in Solutions of Strong Acids and Strong BasesAlgo. Option: algorithmic

18) What is the pH of a solution prepared by mixing 100.00 mL of 0.020 M Ca(OH)2 with 50.00 mL of 0.300 M NaOH? Assume that the volumes are additive.A) 13.05B) 13.10C) 13.28D) 13.58Answer: BDiff: 3Topic: Section 14.7 The pH in Solutions of Strong Acids and Strong BasesAlgo. Option: algorithmic

19) What is the hydronium ion concentration of a 0.500 M acetic acid solution with Ka = 1.8 ×

10-5? The equation for the dissociation of acetic acid is:CH3CO2H(aq) + H2O(l) ⇌ H3O+(aq) + CH3CO2-(aq).

A) 3.0 × 10-2 MB) 4.2 × 10-2 MC) 3.0 × 10-3 MD) 4.2 × 10-3 MAnswer: CDiff: 3Topic: Section 14.9 Calculating Equilibrium Concentrations in Solutions of Weak AcidsAlgo. Option: algorithmic


20) What is the hydronium ion concentration of a 0.150 M hypochlorous acid solution with The equation for the dissociation of hypochlorous acid is:

HOCl(aq) + H2O(l) ⇌ H3O+(aq) + OCl-(aq).

A) 1.9 × 10-4 MB) 7.2 × 10-4 MC) 2.8 × 10-5 MD) 7.2 × 10-5 MAnswer: DDiff: 3Topic: Section 14.9 Calculating Equilibrium Concentrations in Solutions of Weak AcidsAlgo. Option: algorithmic

21) Potassium hydrogen phthalate (molar mass = 204.2 g/mol)is one of the most commonly used acids for standardizing solutions containing bases. KHP is a monoprotic weak acid with

Calculate the pH of the solution that results when 0.50 g of KHP is dissolved in enough water to produce 25.0 mL of solution. A) 2.05B) 3.21C) 4.40D) 5.41Answer: BDiff: 4Topic: Section 14.9 Calculating Equilibrium Concentrations in Solutions of Weak AcidsAlgo. Option: algorithmic

22) Calculate the pH of a 0.080 M carbonic acid solution, H2CO3(aq), that has the stepwise

dissociation constants Ka1 = 4.3 × 10-7 and Ka2 = 5.6 × 10-11. A) 1.10B) 3.73C) 6.37D) 10.25Answer: BDiff: 4Topic: Section 14.11 Equilibria in Solutions of Polyprotic AcidsAlgo. Option: algorithmic


23) Calculate the pH of a 0.60 M H2SO3, solution that has the stepwise dissociation constants

Ka1 = 1.5 × 10-2 and A) 1.02B) 1.06C) 1.82D) 2.04Answer: BDiff: 5Topic: Section 14.11 Equilibria in Solutions of Polyprotic AcidsAlgo. Option: algorithmic

24) Calculate the concentration of bicarbonate ion, HCO3-, in a 0.010 M H2CO3 solution that

has the stepwise dissociation constants Ka1 = 4.3 × 10-7 and Ka2 = 5.6 × 10-11.

A) 6.6 × 10-5 MB) 4.3 × 10-7 MC) 4.3 × 10-9 MD) 5.6 × 10-11 MAnswer: ADiff: 4Topic: Section 14.11 Equilibria in Solutions of Polyprotic AcidsAlgo. Option: algorithmic

25) What is the pH of a 0.40 M H2Se solution that has the stepwise dissociation constants Ka1 =

1.3 × 10-4 and A) 2.14B) 3.89C) 4.28D) 5.57Answer: ADiff: 3Topic: Section 14.11 Equilibria in Solutions of Polyprotic AcidsAlgo. Option: algorithmic

26) What is the selenide ion concentration [Se2-] for a 0.100 M H2Se solution that has the

stepwise dissociation constants of and

A) 3.6 × 10-3 MB) 1.3 × 10-4 MC) 1.3 × 10-5 MD) 1.0 × 10-11 MAnswer: DDiff: 3Topic: Section 14.11 Equilibria in Solutions of Polyprotic AcidsAlgo. Option: algorithmic


27) What is the pH of a 0.200 M NH3 solution that has Kb = 1.8 × 10-5? The equation for the dissociation of NH3 is

A) 2.02B) 2.72C) 11.98D) 11.28Answer: DDiff: 3Topic: Section 14.12 Equilibria in Solutions of Weak BasesAlgo. Option: algorithmic

28) What is the pH of a 0.30 M pyridine solution that has Kb = 1.9 × 10-9? The equation for the dissociation of pyridine is


29) Aniline, (C6H5NH2, Kb = at 25°C) is an industrially important amine used in the making of dyes. Determine the pH of an aniline solution made by dissolving 6.90 g of aniline in enough water to make 100 mL of solution. A) 4.75B) 9.25C) 9.50D) 10.50Answer: BDiff: 4Topic: Section 14.12 Equilibria in Solutions of Weak BasesAlgo. Option: algorithmic


30) Determine the ammonia concentration of an aqueous solution that has a pH of 11.00. The equation for the dissociation of NH3 (Kb = 1.8 × 10-5) is

A) 3.0 MB) 0.056 MC) 1.8 × 10-2 MD) 1.0 × 10-3 MAnswer: BDiff: 4Topic: Section 14.12 Equilibria in Solutions of Weak BasesAlgo. Option: algorithmic

31) Which one of the following salts, when dissolved in water, produces the solution with the highest pH? A) KHCO3B) CsClO4C) RaOD) CH3CH3NH3ClAnswer: CDiff: 3Topic: Section 14.14 Acid-Base Properties of SaltsAlgo. Option: algorithmic

32) If an equal number of moles of the weak acid HCN and the strong base KOH are added to water, is the resulting solution acidic, basic, or neutral? A) acidicB) basicC) neutralD) There is insufficient information provided to answer this question.Answer: BDiff: 2Topic: Section 14.14 Acid-Base Properties of SaltsAlgo. Option: algorithmic

33) Which one of the following salts, when dissolved in water, produces the solution with the highest pH?A) RbIB) RbBrC) RbClD) RbFAnswer: DDiff: 3Topic: Section 14.14 Acid-Base Properties of SaltsAlgo. Option: algorithmic


34) Which one of the following salts, when dissolved in water, produces the solution with a pH closest to 7.00?A) NH4Br B) Ca OC) K HSO4D) CsIAnswer: DDiff: 3Topic: Section 14.14 Acid-Base Properties of SaltsAlgo. Option: algorithmic

35) Calculate the pH of a 0.800 M NaCH3CO2 solution. Ka for acetic acid, CH3CO2H, is

A) 2.42B) 4.68C) 9.32D) 11.58Answer: CDiff: 5Topic: Section 14.14 Acid-Base Properties of SaltsAlgo. Option: algorithmic

36) Calculate the pH of a 1.60 M KBrO solution. Ka for hypobromous acid, HBrO, is A) 2.55B) 4.25C) 9.75D) 11.45Answer: DDiff: 5Topic: Section 14.14 Acid-Base Properties of SaltsAlgo. Option: algorithmic

37) Calculate the pH of a 1.60 M CH3NH3Cl solution. Kb for methylamine, CH3NH2, is

A) 1.61B) 5.18C) 8.82D) 12.39Answer: BDiff: 5Topic: Section 14.14 Acid-Base Properties of SaltsAlgo. Option: algorithmic


38) Which one of the following salts, when dissolved in water, produces the solution with the lowest pH?A) NaClB) KClC) MgCl2D) AlCl3Answer: DDiff: 3Topic: Section 14.14 Acid-Base Properties of SaltsAlgo. Option: algorithmic

14.3 Short Answer Questions

1) The Brønsted-Lowry acid in the chemical equation below is _________.HNO2(aq) + H2O(l) H⇌ 3O+(aq) + NO2–(aq)

Answer: HNO2Diff: 2Topic: Section 14.1 Acid-Base Concepts: The Brønsted-Lowry Theory

2) The equilibrium constant for the reaction below has the value Ka = 3.5 × 10–4. In this reaction the Brønsted-Lowry acid is ________.

HF(aq) + H2O(l) H⇌ 3O+(aq) + F–(aq)Answer: HFDiff: 2Topic: Section 14.2 Acid Strength and Base Strength

3) A proton hydrated by four water molecules has the formula ________.Answer: H9O4+

Diff: 3Topic: Section 14.1 Acid-Base Concepts: The Brønsted-Lowry Theory

4) An acidic solution with hydronium ion concentration [H+] = 1.60 × 10–3 M has a hydroxide ion concentration [OH–] = ________.Answer: 6.25 × 10–12 MDiff: 2Topic: Section 14.4 Dissociation of Water

5) At 50°C the value of Kw is 5.5 × 10–14, and the pH of a neutral solution at 50°C is ________.Answer: 6.63Diff: 3Topic: Section 14.5 The pH Scale


6) The pH of a 0.025 M KOH solution is ________.Answer: 12.40Diff: 2Topic: Section 14.7 The pH in Solutions of Strong Acids and Strong Bases

7) The value of Ka for a 0.250 M HCN solution having a pH of 4.956 is ________.

Answer: 4.90 × 10–10Diff: 3Topic: Section 14.8 Equilibria in Solutions of Weak Acids

8) A 0.050 M solution of hydroxylamine, NH2OH, having Kb = 9.1 × 10–9 has a pH of ________.Answer: 9.33Diff: 4Topic: Section 14.12 Equilibria in Solutions of Weak Bases

9) A 0.10 M KNO2 solution will have a pH ________ seven.Answer: greater thanDiff: 2Topic: Section 14.14 Acid-Base Properties of Salts

10) The acid strength of an oxoacid having the general formula HnYOm increases as the electronegativity of Y ________ and as the oxidation number of Y ________.Answer: increases, increasesDiff: 3Topic: Section 14.3 Factors That Affect Acid Strength


Chapter 14 Review Questions

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