Test Questions & Answers Acids And Bases Bauer Ch.13

Introduction to Chemistry, 5e (Bauer)

Chapter 13 Acids and Bases

1) Which of the following is not an attribute of an acid?

A) It provides H+ ions in aqueous solution.

B) It is a nonelectrolyte.

C) It tastes sour.

D) It reacts with some organic dyes to cause them to change color.

E) It reacts with active metals.

2) Which of the following is not an attribute of a base?

A) It provides OH− ions in aqueous solution.

B) It is an electrolyte.

C) It reacts with some organic dyes to cause them to change color.

D) It has the ability to neutralize acids.

E) It would taste sour.

3) Which of the following acids is not normally found in foods or beverages?

A) citric acid

B) acetic acid

C) phosphoric acid

D) carbonic acid

E) sulfuric acid

4) Which of the following bases is not commonly found in household products or antacids?

A) sodium hydroxide, NaOH

B) ammonia, NH3

C) calcium carbonate, CaCO3

D) magnesium hydroxide, Mg(OH)2

E) methyl amine, CH3NH2

5) Which of the following statements regarding acids is incorrect?

A) An acid will react with an active metal.

B) An acid is a substance that will change the color of blue litmus paper.

C) An acid is a substance that would taste sour.

D) An acid is a substance that produces hydrogen ions, H+, (or H3O+) in aqueous solution.

E) An acid is always a strong electrolyte.

6) Which of the following statements regarding bases is incorrect?

A) A base is a substance that may act as an antacid.

B) A base is a substance that will not change the color of red litmus paper.

C) A base is a substance that tastes bitter.

D) A base is a substance that produces hydroxide ions, OH−, in aqueous solution.

E) A base is a substance that is an electrolyte.

7) The substance HCl(aq) is

A) a strong acid.

B) a weak acid.

C) a strong base.

D) a weak base.

E) neither an acid nor a base.

8) The substance NaOH(aq) is

A) a strong acid.

B) a weak acid.

C) a strong base.

D) a weak base.

E) neither an acid nor a base.

9) The substance NH3(aq) is

A) a strong acid.

B) a weak acid.

C) a strong base.

D) a weak base.

E) neither an acid nor a base.

10) The substance HNO3(aq) is

A) a strong acid.

B) a weak acid.

C) a strong base.

D) a weak base.

E) neither an acid nor a base.

11) The substance Mg(OH)2(aq) is

A) a strong acid.

B) a weak acid.

C) a strong base.

D) a weak base.

E) neither an acid nor a base.

12) When the following reaction goes in the reverse direction (from products to reactants), what is the base?

HCN(aq) + H2O(l) ⇌ CN− (aq) + H3O+(aq)

A) HCN

B) H2O

C) CN−

D) H3O+

E) both CN− and H3O+

13) When the following reaction goes in the reverse direction (from products to reactants), what is the base?

HF(aq) + H2O(l) ⇌ F−(aq) + H3O+(aq)

A) HF

B) H2O

C) F−

D) H3O+

E) both F− and H3O+

14) When the following reaction goes in the reverse direction (from products to reactants), what is the acid?

HCN(aq) + H2O(l) ⇌ CN− (aq) + H3O+(aq)

A) HCN

B) H2O

C) CN−

D) H3O+

E) both CN− and H3O+

15) When the following reaction goes in the reverse direction (from products to reactants), what is the acid?

HF(aq) + H2O(l) ⇌ F− (aq) + H3O+(aq)

A) HF

B) H2O

C) F−

D) H3O

E) both F− and H3O

16) List the acid, base, conjugate acid, and conjugate base, in that order, for the following reaction:

HOCl(aq) + H2O(l) ⇌ OCl−(aq) + H3O+(aq)

A) HOCl, H2O, OCl−, H3O+

B) H2O, HOCl, OCl−, H3O+

C) HOCl, H2O, H3O+, OCl−

D) H2O, HOCl, H3O+, OCl−

E) OCl−, H3O+, H2O, HOCl

17) List the acid, base, conjugate acid, and conjugate base, in that order, for the following reaction:

CH3CO2H(aq) + H2O(l) ⇌ CH3CO2−(aq) + H3O+(aq)

A) CH3CO2H, H2O, CH3CO2−, H3O+

B) H2O, CH3CO2H, CH3CO2−, H3O+

C) CH3CO2H, H2O, H3O+, CH3CO2−

D) H2O, CH3CO2H, H3O+, CH3CO2−

E) CH3CO2−, H3O+, H2O, CH3CO2H

18) Select the two Brønsted-Lowry acids in the following equation:

HNO2(aq) + H2O(l) ⇌ NO2−(aq) + H3O+(aq)

A) HNO2 and H2O

B) HNO2 and NO2−

C) HNO2 and H3O+

D) H2O and H3O+

E) NO2− and H3O+

19) Select the two Brønsted-Lowry acids in the following equation:

HCN(aq) + H2O(l) ⇌ CN−(aq) + H3O+(aq)

A) HCN and H2O

B) HCN and CN−

C) H2O and CN−

D) HCN and H3O+

E) H3O+ and CN−

20) Select the two Brønsted-Lowry acids in the following equation:

HF(aq) + H2O(l) ⇌ F−(aq) + H3O+(aq)

A) HF and H2O

B) HF and F−

C) H2O and F−

D) HF and H3O+

E) H3O+ and F−

21) Select the two Brønsted-Lowry bases in the following equation:

NH3(aq) + H2O(aq) ⇌ NH4+(aq) + OH−(aq)

A) NH3 and  H2O

B) NH3 and OH−

C)  H2O and OH−

D) NH3 and NH4+

E) NH4+ and OH−

22) Select the two Brønsted-Lowry bases in the following equation:

CH3NH2(aq) + H2O(l) ⇌ CH3NH3+(aq) + OH−(aq)

A) CH3NH2 and H2O

B) CH3NH2 and OH−

C) H2O and OH−

D) CH3NH2 and CH3NH3+

E) CH3NH3+ and OH−

23) Select the two Brønsted-Lowry bases in the following equation:

CO32−(aq) + H2O(l) ⇌ HCO3−(aq) + OH−(aq)

A) CO32− and H2O

B) CO32− and HCO3−

C)  H2O and OH−

D) CO32− and OH−

E) H2O and HCO3−

24) Select the two Brønsted-Lowry acids in the following equation:

CO32–(aq) + HF(aq) ⇌ HCO3–(aq) + F–(aq)

A) CO32– and HF

B) CO32– and HCO3–

C) HF and F–

D) CO32– and F–

E)  HF and HCO3–

25) Select the two Brønsted-Lowry acids in the following equation:

NH3(aq) + HF(aq) ⇌ NH4+(aq) + F−(aq)

A) NH3 and HF

B) NH3 and F−

C) HF and F−

D) NH4+ and F–

E) HF and NH4+

26) Select the pair that consists of an acid and its conjugate base in that order.

A) NH3/NH4+

B) CO32−/HCO3−

C) H2CO3/HCO3−

D) HPO42−/H3PO4

E) CO32–/ CO22–

27) Select the pair that consists of an acid and its conjugate base in that order.

A) NH4+/NH2–

B) CO32−/HCO3−

C) CO32−/H2CO3−

D) H2PO4–/H3PO4

E) H2CO3/HCO3−

28) Select the pair that consists of an acid and its conjugate base in that order.

A) NH3/NH4+

B) SO42−/HSO3−

C) H2SO3/HSO3−

D) H2PO4−/H3PO4

E) CO32−/HCO32−

29) Select the pair that consists of a base and its conjugate acid in that order.

A) NH3/NH4+

B) HCO3−/CO32−

C) H2CO3/HCO3−

D) H3PO4/ HPO42−

E) CO32−/CO22−

30) Select the pair that consists of a base and its conjugate acid in that order.

A) NH4+/NH3

B) HCO3−/CO32−

C) HCO3−/H2CO3

D) H3PO4/ HPO42−

E) CO32−/CO22−

31) The conjugate acid of H2PO4− is:

A) HPO42−

B) H2PO3−

C) H3PO4

D) PO43−

E) H3PO3

32) The conjugate base of H2PO4− is:

A) HPO42−

B) H2PO3−

C) H3PO4

D) PO43−

E) H2PO4OH−

33) The conjugate acid of HCO3− is:

A) H2CO3

B) HCO2−

C) CO32−

D) CO2

E) H3CO3+

34) The conjugate base of HCO3– is:

A) H2CO3

B) HCO2−

C) CO32−

D) CO2

E) H3CO3+

35) When sodium hydroxide, NaOH, is dissolved in water, which species are present in addition to water?

A) NaOH(aq)

B) Na+(aq) and OH−(aq)

C) Na+(aq) and H3O−(aq)

D) Na+(aq) and O2H22−(aq)

E) NaO−(aq) and H3O+(aq)

36) When ammonia, NH3, is dissolved in water, which ions are formed?

A) NH3−(aq) and OH−(aq)

B) NH3+(aq) and OH−(aq)

C) NH4+(aq) and OH−(aq)

D) NH4+(aq) and H−(aq)

E) NH2−(aq) and H+(aq)

37) When acetate ion, CH3CO2−, reacts with water, what are the products?

A) H+(aq) and OH−(aq)

B) CH3CO2+(aq) and OH−(aq)

C) CH3CO2+(aq) and H2O(aq)

D) CH3CO2+(aq) and H−(aq)

E) CH3CO2H(aq) and OH−(aq)

38) When carbonate ion, CO32−, reacts with water, what are the products?

A) H+(aq) and OH−(aq)

B) HCO3(aq) and OH−(aq)

C) HCO3+(aq) and H2O(aq)

D) HCO3−(aq) and H−(aq)

E) HCO3−(aq) and OH−(aq)

39) When fluoride ion, F−, reacts with water, what are the products?

A) H+(aq) and OH−(aq)

B) F+(aq) and OH−(aq)

C) F+(aq) and H2O(aq)

D) HF(aq) and H−(aq)

E) HF(aq) and OH−(aq)

40) Which of the following is an amphoteric substance?

A) NaCl

B) LiOH

C) KBr

D) NaHCO3

E) CH3OH

41) Which of the following is an amphoteric substance?

A) NaOH

B) LiCl

C) CsBr

D) H2O

E) CH4

42) Which of the following ions is amphoteric?

A) Cl−

B) OH−

C) H+

D) NO3–

E) HCO3–

43) Which of the following ions is amphoteric?

A) Br−

B) H−

C) OH+

D) SO42−

E) HPO42−

44) Which of the following equations represents the behavior of HCO3− as an acid?

A) HCO3−(aq) + H3O+(aq) ⇌ H2CO3(aq) + H2O(l)

B) HCO3−(aq) + HF(aq) ⇌ H2CO3(aq) + F−(aq)

C) HCO3−(aq) + HCN(aq) ⇌ H2CO3(aq) + CN−(aq)

D) HCO3−(aq) + OH−(aq) ⇌ CO32−(aq) + H2O(l)

E) HCO3−(aq) + H2O(l) ⇌ H2CO3(aq) + OH−(aq)

45) Which of the following equations represents the behavior of HCO3− as a base?

A) HCO3−(aq) + H3O+(aq) ⇌ H2CO3(aq) + H2O(l)

B) HCO3−(aq) + F−(aq) ⇌ CO32−(aq) + HF(aq)

C) HCO3−(aq) + CN−(aq) ⇌ CO32−(aq) + HCN(aq)

D) HCO3−(aq) + OH−(aq) ⇌ CO32−(aq) + H2O(l)

E) HCO3−(aq) + H2O(l) ⇌ H2CO3(aq) + H3O+(aq)

46) Which of the following equations represents the behavior of H2PO4– as an acid?

A) H2PO4–(aq) + H3O+(aq) ⇌ H3PO4(aq) + H2O(l)

B) H2PO4–(aq) + HF(aq) ⇌ H3PO4(aq) + F–(aq)

C) H2PO4–(aq) + HCN(aq) ⇌ H3PO4(aq) + CN–(aq)

D) H2PO4–(aq) + OH–(aq) ⇌ HPO42–(aq) + H2O(l)

E) H2PO4–(aq) + H2O(l) ⇌ H3PO4(aq) + OH–(aq)

47) Which of the following equations represents the behavior of H2PO4– as a base?

A) H2PO4–(aq) + H3O+(aq) ⇌ H3PO4(aq) + H2O(l)

B) H2PO4–(aq) + F–(aq) ⇌ HPO42–(aq) + HF(aq)

C) H2PO4–(aq) + CN–(aq) ⇌ HPO42–(aq) + HCN(aq)

D) H2PO4–(aq) + OH–(aq) ⇌ HPO42–(aq) + H2O(l)

E) H2PO4–(aq) + H2O(l) ⇌ H3PO4(aq) + H3O+(aq)

48) The bicarbonate ion, HCO3–, is amphoteric. What are the conjugate acid and conjugate base, in that order, of HCO3–?

A) CO32–, HCO3–

B) HCO3–, CO32–

C) CO32–, H2CO3

D) H2CO3, CO32–

E) H3O+, CO32–

49) The H2PO4– ion is amphoteric. What are the conjugate acid and conjugate base, in that order, of H2PO4–?

A) PO43–, H2PO4–

B) H2PO4–, PO43–

C) H2PO4–, H3PO4

D) H3PO4, HPO42–

E) H3O+, PO43–

50) Select the strong acid from the following list.

A) H3PO4(aq)

B) CH3CO2H(aq)

C) H2S(aq)

D) H2SO4(aq)

E) HF(aq)

51) Select the strong acid from the following list.

A) HNO3(aq)

B) HClO3(aq)

C) HF(aq)

D) H3PO4(aq)

E) HCN(aq)

52) Select the strong acid from the following list.

A) H2SO3(aq)

B) H2C2O4(aq)

C) H2S(aq)

D) HNO2(aq)

E) HI(aq)

53) All of the following species are weak bases except:

A) NH3(aq)

B) Na2CO3(aq)

C) KF(aq)

D) CH3NH2(aq)

E) NH4Cl(aq)

54) All of the following species are weak bases except:

A) NaCN(aq)

B) K2CO3(aq)

C) KOH(aq)

D) CH3NH2(aq)

E) NH3(aq)

55) All of the following species are weak bases except:

A) KCN(aq)

B) NaNO2(aq)

C) LiCl(aq)

D) C6H5NH2(aq)

E) CH3CH2NH2(aq)

56) The image shows a molecular-level representation of part of a solution after ammonia, NH3, is dissolved in water. (Besides water, there are 2 NH4+ ions, 6 NH3 molecules, and 2 OH− ions present in the solution.). Which of the following best describes NH3?

A) strong acid

B) strong base

C) weak acid

D) weak base

E) amphoteric

57) The image shows a molecular-level representation of part of a solution after HF is dissolved in water. (Besides water, there are 6 HF molecules, 1 H3O+ ion, and 1 F− ion present in the solution.) Which of the following best describes HF?

A) strong acid

B) strong base

C) weak acid

D) weak base

E) amphoteric

58) The image shows a molecular-level representation of part of a solution after HCl is dissolved in water. What best describes this image? (Besides water, there are 6 H3O+ ions and 6 Cl− ions present in the solution.) Which of the following best describes HCl?

A) strong acid

B) strong base

C) weak acid

D) weak base

E) amphoteric

59) Match the molecular-level diagrams to each of the following compounds in aqueous solution: HCl, HF, NH3

A) I = HCl, II = HF, III = NH3

B) I = HF, II = HCl, III = NH3

C) I = HF, II = NH3, III = HCl

D) I = NH3, II = HF, III = HCl

E) I = NH3, II = HCl, III = HF

60) Which of the following is the strongest acid?

A) HF, Ka = 6.3 × 10–4

B) HCN, Ka = 6.2 × 10−10

C) HOCl, Ka = 4.0 × 10−8

D) CH3CO2H, Ka = 1.8 × 10−5

E) HCO2H, Ka = 1.8 × 10−4

61) Which of the following is the strongest acid?

A) HNO2, Ka = 5.6 × 10−4

B) HCN, Ka = 6.2 × 10−10

C) NH4+, Ka = 5.6 × 10−10

D) CH3CO2H, Ka = 1.8 × 10−5

E) HCO2H, Ka = 1.8 × 10−4

62) Which of the following is the strongest acid?

A) HOCl, Ka = 4.0 × 10−8

B) HCN, Ka = 6.2 × 10−10

C) NH4+, Ka = 5.6 × 10−10

D) CH3CO2H, Ka = 1.8 × 10−5

E) HCO2H, Ka = 1.8 × 10−4

63) Given 0.10 M solutions of the following acids, which contains the highest concentration of H3O+?

A) HF, Ka = 6.3 × 10−4

B) HCN, Ka = 6.2 × 10−10 

C) HOCl, Ka = 4.0 × 10−8

D) CH3CO2H, Ka = 1.8 × 10−5

E) HCO2H, Ka = 1.8 × 10−4

64) Given 0.10 M solutions of the following acids, which contains the highest concentration of H3O+?

A) HNO2, Ka = 5.6 × 10−4

B) HCN, Ka = 6.2 × 10−10

C) NH4+, Ka = 5.6 × 10−10

D) CH3CO2H, Ka = 1.8 × 10−5

E) HCO2H, Ka = 1.8 × 10−4

65) Given 0.10 M solutions of the following acids, which contains the lowest concentration of H3O+?

A) HF, Ka = 6.3 × 10−4

B) HCN, Ka = 6.2 × 10−10

C) HOCl, Ka = 4.0 × 10−8

D) CH3CO2H, Ka = 1.8 × 10−5

E) HCO2H, Ka = 1.8 × 10−4

66) Which of the following ionizes to the greatest extent?

A) HF, Ka = 6.3 × 10−4

B) HCN, Ka = 6.2 × 10−10

C) HOCl, Ka = 4.0 × 10−8

D) CH3CO2H, Ka = 1.8 × 10−5

E) HCO2H, Ka = 1.8 × 10−4

67) Which of the following ionizes to the greatest extent?

A) HNO2, Ka = 5.6 × 10−4

B) HCN, Ka = 6.2 × 10−10

C) NH4+, KKa = 5.6 × 10−10

D) CH3CO2H, Ka = 1.8 × 10−5

E) HCO2H, Ka = 1.8 × 10−4

68) Rank the following 0.100 M solutions in order of increasing H3O+ concentration:

HOCl, Ka = 4.0 × 10−8; HCN, Ka = 6.2 × 10−10; NH4+, Ka = 5.6 × 10−10

A) HOCl < HCN < NH4+

B) HOCl < NH4+ < HCN

C) HCN < NH4+ < HOCl

D) HCN < HOCl < NH4+

E) NH4+ < HCN < HOCl

69) Rank the following 0.100 M solutions in order of increasing H3O+ concentration:

HF, Ka = 6.3 × 10−4; HCN, Ka = 6.2 × 10−10; HOCl, Ka = 4.0 × 10−8

A) HF < HCN < HOCl

B) HF < HOCl < HCN

C) HOCl < HF < HCN

D) HOCl < HCN < HF

E) HCN < HOCl < HF

70) Rank the following 0.100 M solutions in order of increasing H3O+ concentration:

HCN, Ka = 6.2 × 10–10; NH4+, Ka = 5.6 × 10–10; CH3CO2H, Ka = 1.8 × 10–5

A) HCN < NH4+ < CH3CO2H

B) HCN < CH3CO2H < NH4+

C) CH3CO2H < NH4+ < HCN 

D) CH3CO2H < HCN < NH4+

E) NH4+ < HCN < CH3CO2H

71) The Ka for acetic acid is 1.8 × 10–5. Which of the following statements best describes the pH of a 0.010 M solution of acetic acid?

A) The pH is greater than 0 but less than 2.

B) The pH is exactly 2.

C) The pH is greater than 2 but less than 7.

D) The pH is exactly 7.

E) The pH is greater than 7 but less than 12.

72) The Ka for formic acid is 1.8 × 10–4. Which of the following statements best describes the pH of a 0.0010 M solution of formic acid?

A) The pH is greater than 0 but less than 3.

B) The pH is exactly 3.

C) The pH is greater than 3 but less than 7.

D) The pH is exactly 7.

E) The pH is greater than 7 but less than 11.

73) List the species present in order of increasing concentration in a 0.1 M solution of H2Se.

A) H2Se < HSe– < Se2−

B) H2Se < Se2− < HSe−

C) Se2– < HSe– < H2Se

D) HSe– < Se2– < H2Se

E) Se2− < H2Se < HSe−

74) List the species present in order of increasing concentration in a 0.1 M solution of H2C2O4.

A) H2C2O4 < HC2O4− < C2O42−

B) H2C2O4 < C2O42− < HC2O4−

C) C2O42− < HC2O4− < H2C2O4

D) HC2O4− < C2O42− < H2C2O4

E) C2O42− < H2C2O4 < HC2O4−

75) List the species present in order of increasing concentration in a 0.1 M solution of H2S.

A) H2S < HS– < S2–

B) H2S < S2– < HS–

C) S2– < HS– < H2S

D) HS– < S2– < H2S

E) S2– < H2S < HS–

76) Select the solution below that is the most acidic.

A) [H3O+] = 1.0 × 10–4 M

B) [H3O+] = 1.0 × 10–6 M

C) [H3O+] = 1.0 × 10–7 M

D) [H3O+] = 1.0 × 10–8 M

E) [H3O+] = 1.0 × 10–10 M

77) Select the solution below that is the most basic.

A) [H3O+] = 1.0 × 10–4 M

B) [H3O+] = 1.0 × 10–6 M

C) [H3O+] = 1.0 × 10–7 M

D) [H3O+] = 1.0 × 10–8 M

E) [H3O+] = 1.0 × 10–10 M

78) Select the solution below that is the most acidic.

A) [OH–] = 1.0 × 10–4 M

B) [OH–] = 1.0 × 10–5 M

C) [OH–] = 1.0 × 10–7 M

D) [OH–] = 1.0 × 10–9 M

E) [OH–] = 1.0 × 10–11 M

79) Select the solution below that is the most basic.

A) [OH–] = 1.0 × 10–4 M

B) [OH–] = 1.0 × 10–5 M

C) [OH–] = 1.0 × 10–7 M

D) [OH–] = 1.0 × 10–9 M

E) [OH–] = 1.0 × 10–11 M

80) Select the solution below that is the most acidic.

A) [OH–] = 1.0 × 10–4 M

B) [OH–] = 1.0 × 10–5 M

C) [H3O+] = 1.0 × 10–6 M

D) [H3O+] = 1.0 × 10–8 M

E) [H3O+] = 1.0 × 10–10 M

81) Select the solution below that is the most acidic.

A) [OH–] = 1.0 × 10–10 M

B) [OH–] = 1.0 × 10–5 M

C) [H3O+] = 1.0 × 10–6 M

D) [H3O+] = 1.0 × 10–8 M

E) [H3O+] = 1.0 × 10–10 M

82) Select the solution below that is the most basic.

A) [OH–] = 1.0 × 10–10 M

B) [OH–] = 1.0 × 10–4 M

C) [H3O+] = 1.0 × 10–6 M

D) [H3O+] = 1.0 × 10–7 M

E) [H3O+] = 1.0 × 10–9 M

83) Given an OH– concentration of 0.10 M, calculate the H3O+ concentration, and then identify the solution as acidic, basic, or neutral.

A) [H3O+] = 1.0 × 10–7, neutral

B) [H3O+] = 1.0 × 10–1, acidic

C) [H3O+] = 1.0 × 10–13, acidic

D) [H3O+] = 1.0 × 10–13, basic

E) [H3O+] = 1.0 × 10–1, basic

84) Given an OH− concentration of 1.0 × 10−4 M, calculate the H3O+ concentration, and then identify the solution as acidic, basic, or neutral.

A) [H3O+] = 1.0 × 10–7, neutral

B) [H3O+] = 1.0 × 10–4, acidic

C) [H3O+] = 1.0 × 10–10, acidic

D) [H3O+] = 1.0 × 10–10, basic

E) [H3O+] = 1.0 × 10–4, basic

85) Given an OH– concentration of 1.0 × 10–6 M, calculate the H3O+ concentration, and then identify the solution as acidic, basic, or neutral.

A) [H3O+] = 1.0 × 10–7, neutral

B) [H3O+] = 1.0 × 10–6, acidic

C) [H3O+] = 1.0 × 10–8, acidic

D) [H3O+] = 1.0 × 10–8, basic

E) [H3O+] = 1.0 × 10–6, basic

86) Given an H3O+ concentration of 1.0 × 10–4 M, calculate the OH– concentration, and then identify the solution as acidic, basic, or neutral.

A) [OH–] = 1.0 × 10–7, neutral

B) [OH–] = 1.0 × 10–4, acidic

C) [OH–] = 1.0 × 10–10, acidic

D) [OH–] = 1.0 × 10–10, basic

E) [OH–] = 1.0 × 10–4, basic

87) Given an H3O+ concentration of 1.0 × 10–6 M, calculate the OH– concentration, and then identify the solution as acidic, basic, or neutral.

A) [OH–] = 1.0 × 10–7, neutral

B) [OH–] = 1.0 × 10–6, acidic

C) [OH–] = 1.0 × 10–8, acidic

D) [OH–] = 1.0 × 10–8, basic

E) [OH–] = 1.0 × 10–6, basic

88) Calculate the pH of a solution that has [H3O+] = 1.0 × 10–7 M.

A) pH = 1.00

B) pH = 7.00

C) pH = 6.00

D) pH = 8.00

E) pH = 14.00

89) Calculate the pH of a solution that has [H3O+] = 1.0 × 10–6 M.

A) pH = 1.00

B) pH = 7.00

C) pH = 6.00

D) pH = 8.00

E) pH = 14.00

90) Calculate the pH of a solution that has [OH–] = 1.0 × 10–6 M.

A) pH = 1.00

B) pH = 7.00

C) pH = 6.00

D) pH = 8.00

E) pH = 14.00

91) Calculate the pH of a solution that has [OH–] = 1.0 × 10–8 M.

A) pH = 1.00

B) pH = 7.00

C) pH = 14.00

D) pH = 8.00

E) pH = 6.00

92) Calculate the pH of a solution that has [H3O+] = 5.2 × 10–7 M.

A) pH = 5.20

B) pH = 6.28

C) pH = 7.00

D) pH = 5.27

E) pH = 7.72

93) Calculate the pH of a solution that has [H3O+] = 3.1 × 10–8 M.

A) pH = 7.51

B) pH = 8.00

C) pH = 3.10

D) pH = 3.18

E) pH = 6.49

94) Calculate the pH of a solution that has [H3O+] = 5.9 × 10–5 M.

A) pH = 5.90

B) pH = 4.23

C) pH = 5.00

D) pH = 5.59

E) pH = 9.77

95) Calculate the pH of a solution that has [OH–] = 5.9 × 10–5 M.

A) pH = 5.90

B) pH = 5.00

C) pH = 4.23

D) pH = 9.77

E) pH = 5.59

96) Calculate the pH of a solution that has [OH–] = 3.1 × 10–8 M.

A) pH = 3.10

B) pH = 8.00

C) pH = 7.51

D) pH = 3.18

E) pH = 6.49

97) Calculate the pH of a solution that has [OH–] = 5.2 × 10–7 M.

A) pH = 5.20

B) pH = 7.00

C) pH = 6.28

D) pH = 5.27

E) pH = 7.72

98) Calculate the pOH of a solution that has [OH–] = 3.1 × 10–8 M.

A) pOH = 3.10

B) pOH = 8.00

C) pOH = 7.51

D) pOH = 3.18

E) pOH = 6.49

99) Calculate the pOH of a solution that has [OH–] = 5.9 × 10–5 M.

A) pOH = 5.90

B) pOH = 5.00

C) pOH = 4.23

D) pOH = 5.59

E) pOH = 9.77

100) Calculate the pOH of a solution that has [H3O+] = 5.2 × 10–7 M.

A) pOH = 7.72

B) pOH = 7.00

C) pOH = 6.28

D) pOH = 5.27

E) pOH = 5.20

101) Calculate the pOH of a solution that has [H3O+] = 3.1 × 10–8 M.

A) pOH = 3.10

B) pOH = 6.49

C) pOH = 7.51

D) pOH = 3.18

E) pOH = 8.00

102) If the pH of a certain soft drink is 3.60, what is the H3O+ concentration in the soft drink?

A) 3.6 M

B) 2.5 × 10–3 M

C) 2.5 × 10–5 M

D) 2.5 × 10–4 M

E) 10. M

103) If the pH of a blood sample is 7.60, what is the H3O+ concentration in the blood?

A) 7.6 M

B) 2.5 × 10–8 M

C) 2.5 × 10–7 M

D) 2.5 × 10–9 M

E) 6.4 M

104) If the pH of a coffee sample is 5.15, what is the H3O+ concentration in the coffee?

A) 5.2 M

B) 7.1 × 10–8 M

C) 7.1 × 10–7 M

D) 7.1 × 10–6 M

E) 8.8 M

105) If the pOH of a coffee sample is 8.85, what is the H3O+ concentration in the coffee?

A) 5.2 M

B) 7.1 × 10–8 M

C) 7.1 × 10–7 M

D) 7.1 × 10–6 M

E) 8.8 M

106) If the pOH of a borax solution is 4.55, what is the H3O+ concentration in the borax solution?

A) 4.6 M

B) 3.5 × 10–9 M

C) 3.5 × 10–10 M

D) 3.5 × 10–11 M

E) 9.4 M

107) If the pOH of an orange juice sample is 10.38, what is the H3O+ concentration in the orange juice?

A) 10. M

B) 2.4 × 10–4 M

C) 2.4 × 10–10 M

D) 4.2 × 10–11 M

E) 3.6 M

108) What is the pH of a 0.015 M HNO3 solution?

A) 0.015

B) 1.82

C) 7.00

D) 12.18

E) −1.82

109) What is the pH of a 0.020 M HCl solution?

A) 0.020

B) 1.70

C) 7.00

D) 12.30

E) −1.70

110) What is the pH of a 0.015 M NaOH solution?

A) 0.015

B) 1.82

C) 7.00

D) 12.18

E) −1.82

111) What is the pH of a 0.020 M KOH solution?

A) 0.020

B) 1.70

C) 7.00

D) 12.30

E) −1.70

112) Calculate the H3O+ concentration in 0.0010 M HCl.

A) 1.0 × 10–2 M

B) 1.0 × 10–3 M

C) 1.0 × 103 M

D) 1.0 × 102 M

E) 3.0 M

113) Calculate the H3O+ concentration in 0.10 M NaOH.

A) 1.0 × 10–1 M

B) 1.0 × 10–2 M

C) 1.0 × 1013 M

D) 1.0 × 10–12 M

E) 1.0 × 10–13 M

114) The indicator phenolphthalein changes from colorless to pink between pH 8.2 and pH 10. If phenolphthalein is added to a solution, and the solution remains colorless, then

A) the solution is acidic, and the pH must be at or below 7.0.

B) the pH of the solution must be below 8.2, and the solution is basic.

C) the pH of the solution must be below 8.2, but the solution could be either acidic or basic.

D) the pH of the solution must be above 10, and the solution is basic.

E) the pH of the solution is above 10, and the solution is acidic.

115) The indicator phenol red changes from yellow to red between pH 6.8 and pH 8.4. If phenol red is added to a solution, and the solution turns yellow, then

A) the solution is basic, and the pH must be at or below 7.0.

B) the pH of the solution must be below 6.8, and the solution is basic.

C) the pH of the solution must be below 6.8, and the solution is acidic.

D) the pH of the solution must be above 8.4, and the solution is basic.

E) the pH of the solution is above 8.4, and the solution is acidic.

116) The indicator phenol red changes from yellow to red between pH 6.8 and pH 8.4. If phenol red is added to a solution, and the solution turns red, then

A) the solution is basic, and the pH must be at or below 7.0.

B) the pH of the solution must be below 6.8, and the solution is basic.

C) the pH of the solution must be below 6.8, and the solution is acidic.

D) the pH of the solution must be above 8.4, and the solution is basic.

E) the pH of the solution is above 8.4, and the solution is acidic.

117) If CH3NH2 is added to water, what other compound could also be added in order to make a buffered solution?

A) H2O

B) NaOH

C) CH3NH3Cl

D) NaCH3NH2

E) NaCl

118) If Na2HPO4 is added to water, what other compound could also be added in order to make a buffered solution?

A) H3PO4

B) NaHPO4

C) NaH2PO4

D) Na2PO3

E) NaCl

119) If NaH2PO4 is added to water, what other compound or compounds could also be added in order to make a buffered solution?

A) H3PO4 only

B) NaHPO4 only

C) Na2HPO4 only

D) Na2PO3 only

E) either H3PO4 or Na2HPO4

120) Which of the following will not change when an acid is added to water?

A) pH

B) pOH

C) Kw

D) hydronium ion concentration

E) hydroxide ion concentration

121) A solution of a strong acid will have a greater H3O+ concentration than a solution of a weak acid under any circumstances.

122) Polyprotic acids possess more than one ionizable hydrogen atom.

123) In polyprotic acids, the first ionizable hydrogen always ionizes to a greater extent than the second or third ionizable hydrogen(s).

124) In pure water at 25°C, the concentration of H3O+ is equal to the concentration of OH–.

125) The H3O+ concentration in a 0.010 M solution of NaOH is 0.010 M.

126) The H3O+ concentration in a 0.050 M solution of HClO4 is 0.050 M.

127) If you take an antacid tablet, the pH in your stomach will increase. This means your stomach juice becomes more acidic.

128) The pH of an aqueous HCl solution can be greater than 7.

129) If one solution has an H3O+ concentration that is 10 times less than that of another solution, the difference in pH is 10 units.

130) The symbol In– can be used to represent the base form of an indicator.

131) Is it possible for a solution of a weak acid to have a higher hydronium ion concentration, [H3O+], than a solution of a strong acid? Explain.

132) Identify gastric juice, pH = 1.0, as acidic, basic, or neutral.

133) Identify orange juice, pH = 3.5, as acidic, basic, or neutral.

134) Identify blood, pH = 7.4, as acidic, basic, or neutral.

135) Would you expect the pH of a 0.010 M solution of HF to be less than, greater than, or equal to 2.00? Explain.

136) Is it possible for an indicator to change color in two different pH ranges? If so, under what circumstances is this possible?

137) How does a buffered solution resist changes in pH due to added acid or base?