Chapter 15 1 Which The Following Concerning The Relative Strength

Chapter 15 – Acids and Bases

1. Which of the following reactions is not readily explained by the Arrhenius concept of acids

and bases?

A)

HCl(g) + NH3(g) → NH4Cl(s)

B)

HCl(aq) + NaOH(aq) → NaCl(aq) + H2O(l)

C)

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

D)

HC2H3O2(aq) + H2O(l) H3O+(aq) + C2H3O2−(aq)

E)

H3O+(aq) + OH−(aq) → 2H2O(l)

2. Which of the following statements is/are consistent with the Arrhenius concept of acids and

bases?

1.

An Arrhenius acid will increase the concentration of hydronium ion in an

aqueous or nonaqueous solvent.

2.

All Arrhenius acids are strong electrolytes in water.

3.

All strong acid-strong base reactions have the same heat of reaction (H) per

mole of water formed.

A)

1 only

B)

2 only

C)

3 only

D)

1 and 3

E)

1, 2 and 3

3. Which of the following statements does not describe a characteristic of an Arrhenius acid?

A)

An Arrhenius acid reacts with an Arrhenius base to produce a salt.

B)

An Arrhenius acid turns red litmus blue.

C)

An Arrhenius acid is an electrolyte.

D)

An Arrhenius acid reacts with CaCO3 to produce CO2.

E)

An Arrhenius acid tastes sour.

Test Bank General Chemistry, 10th edition 2

4. Which of the following species is not capable of acting as an Arrhenius acid in aqueous

solution?

A)

Br–

B)

HF

C)

H2SO3

D)

H3O+

E)

HNO3

5. Which of the following species is not capable of acting as an Arrhenius acid in aqueous

solution?

A)

CHCl3

B)

HNO3

C)

H2SO4

D)

H3O+

E)

HClO4

6. Which of the following statements is correct concerning the neutralization of sulfurous acid

by a strong base?

2OH–(aq) + H2SO3(aq) → SO32–(aq) + 2H2O(l)

A)

H2SO3 is both an Arrhenius acid and a Brønsted–Lowry acid.

B)

H2SO3 is a Brønsted–Lowry acid, but not an Arrhenius acid.

C)

H2SO3 is neither an Arrhenius acid nor a Brønsted–Lowry acid.

D)

H2SO3 is an Arrhenius acid, but not a Brønsted–Lowry acid.

E)

H2SO3 is a Lewis base.

7. Which of the following statements is/are consistent with the Brønsted-Lowry concept of

acids and bases?

1.

A conjugate acid-base pair may differ by only one proton.

2.

A base is defined as a hydroxide ion donor.

3.

Brønsted-Lowry acid-base reactions are restricted to aqueous solutions.

A)

1 only

B)

2 only

C)

3 only

D)

1 and 2

E)

1, 2, and 3

8. Which are the Brønsted–Lowry bases in the following equilibrium?

CH3COO–(aq) + H2O(l) CH3COOH(aq) + OH–(aq)

A)

CH3COO– and OH–

B)

H2O and OH–

C)

H2O, CH3COOH, and OH–

D)

CH3COO– and CH3COOH

E)

H2O and CH3COOH

9. Which of the following pairs of species is not a conjugate acid–base pair?

A)

HOCl, OCl–

B)

HNO2, NO2+

C)

O2–, OH–

D)

HSO4–, SO42–

E)

H2CO3, HCO3–

10. What is a conjugate acid–base pair for the following equilibrium?

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

A)

H2O is an acid and HPO42– is its conjugate base.

B)

HPO42– is an acid and OH– is its conjugate base.

C)

H2O is an acid and OH– is its conjugate base.

D)

HPO42– is an acid and H2PO4– is its conjugate base.

E)

HPO42– is an acid and H2O is its conjugate base.

11. What is the conjugate base of H2PO4–(aq)?

A)

PO43–

B)

H3O+

C)

HPO4−

D)

H3P

E)

H3PO4

12. What is a conjugate acid–base pair for the following equilibrium?

H2O(l) + NH4+(aq) NH3(aq) + H3O+(aq)

A)

H2O is an acid and NH3 is its conjugate base.

B)

H2O is an acid and H3O+ is its conjugate base.

C)

NH4+ is an acid and NH3 is its conjugate base.

D)

H2O is a base and NH3 is its conjugate acid.

E)

H2O is a base and NH4+ is its conjugate acid.

13. Which of the following species is amphiprotic in aqueous solution?

A)

CH3NH2

B)

H3O+

C)

NH4+

D)

F−

E)

H2O

14. Which of the following species cannot act as a Lewis base?

A)

H2S

B)

S2–

C)

Al3+

D)

SH–

E)

H2O

15. Which of the following species cannot act as a Lewis base?

A)

H2O2

B)

OH–

C)

O2–

D)

H2O

E)

Be2+

16. Which of the following species cannot act as a Lewis base?

A)

NH3

B)

NH4+

C)

N3–

D)

NH2–

E)

NH2–

17. Which of the following species cannot act as a Lewis acid?

A)

H+

B)

H–

C)

K+

D)

Mg2+

E)

Al3+

18. In the reaction

CuO(s) + SO2(g) → CuSO3(s),

A)

O2– acts as a Lewis base and SO2 acts as a Lewis acid.

B)

O2– acts as a Lewis base and Cu2+ acts as a Lewis acid.

C)

CuO is the Lewis acid and CuSO3 is its conjugate base.

D)

SO2 is the Lewis acid and CuSO3 is its conjugate base.

E)

Cu2+ acts as a Lewis acid and SO32– acts as a Lewis base.

19. Consider the following reaction:

AgBr(s) + 2CN–(aq) → Ag(CN)2–(aq) + Br–(aq)

The species that are acting as a Lewis acid and Lewis base, respectively, are

A)

Br– and CN–.

B)

Ag+ and CN–.

C)

AgBr and Ag(CN)2–.

D)

Ag(CN)2– and Ag+.

E)

Ag+ and Br–.

20. Which of the following is not an example of an acid–base reaction?

A)

Al(OH)3(s) + 3H+(aq) → Al3+(aq) + 3H2O(l)

B)

C2H6(g) → C2H4(g) + H2(g)

C)

MgO(s) + CO2(g) → MgCO3(s)

D)

Al(OH)3(s) + OH–(aq) → Al(OH)4–(aq)

E)

CN–(aq) + H2O(l) HCN(aq) + OH–(aq)

21. Which of the following is/are an appropriate classification of the reaction given below?

KOH(aq) + CO2(g) → KHCO3(aq)

1.

The above reaction may be classified as an Arrhenius acid-base reaction.

2.

The above reaction may be classified as a Brønsted-Lowry acid-base reaction.

3.

The above reaction may be classified as a Lewis acid-base reaction.

A)

1 only

B)

2 only

C)

3 only

D)

1 and 3

E)

none

Test Bank General Chemistry, 10th edition 7

22. Which of the following species cannot act as a Lewis acid?

A)

BeCl2

B)

H+

C)

Ag+

D)

BF3

E)

NH4+

23. Which acid has the strongest conjugate base in aqueous solution?

A)

HF

B)

HNO3

C)

HClO4

D)

HI

E)

H2SO4

24. Which of the following concerning the relative strength of acids and bases is/are correct?

1.

As the acidity of the acid decreases, the basicity of the conjugate base

increases.

2.

The hydronium ion is the strongest acid that can be found in aqueous solution.

3.

All acids classified as strong acids in aqueous solution have the same acidity

in a more acidic solvent like acetic acid.

A)

1 only

B)

2 only

C)

3 only

D)

1 and 2

E)

1, 2, and 3

25. Which of the following acids has the weakest conjugate base in aqueous solution?

A)

CH3COOH

B)

HOCl

C)

HF

D)

HNO2

E)

HClO4

Test Bank General Chemistry, 10th edition 8

26. Which of the following acids has the strongest conjugate base?

A)

HClO

B)

HClO4

C)

HClO2

D)

HClO3

E)

HCl

27. The acid strength decreases in the series HBr > HSO4– > CH3COOH > HCN > HCO3–.

Which of the following is the strongest base?

A)

SO42–

B)

CO32–

C)

CH3COO–

D)

Br–

E)

CN–

28. What is the leveling effect?

A)

All bases are 100% ionized in water.

B)

All acids are 100% ionized in solvents other than water.

C)

All strong acids are 100% ionized in water.

D)

An acid with a higher concentration in water has a lower pH than an acid with a

lower concentration in water.

E)

A base with a higher concentration in water has a lower pH than a base with a

lower concentration in water.

29. Which of the following reactions is not product-favored?

A)

NaOH(aq) → Na+(aq) + OH–(aq)

B)

NH3(aq) + H2O(l) → NH4+(aq) + OH–(aq)

C)

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

D)

HCl(aq) + H2O(l) → H3O+(aq) + Cl–(aq)

E)

H2SO4(aq) + H2O(l) → H3O+(aq) + HSO4–(aq)

30. Given equal concentrations of the following acids, which exhibits the greatest amount of

ionization in water?

A)

nitrous acid

B)

chlorous acid

C)

ascorbic acid

D)

hydrobromic acid

E)

citric acid

31. Which of the following statements is true concerning an aqueous solution of the weak base

NH3?

A)

OH– is a stronger base than NH3.

B)

OH– is a stronger acid than NH4+.

C)

NH4+ is a stronger acid than H3O+.

D)

NH3 is a weaker base than H2O.

E)

H2O is a stronger acid than H3O+.

32. Which of the following statements is true concerning an aqueous solution of the strong acid

HBr?

A)

Br– is a stronger acid than H2O.

B)

Br– is a stronger base than OH–.

C)

H3O+ is a stronger acid than HBr.

D)

H2O is a stronger acid than HBr.

E)

H2O is a stronger base than Br–.

Test Bank General Chemistry, 10th edition 10

33. Rank the following in order of decreasing acid strength in aqueous solution: HCl, HOCl,

HOBr, HOI.

A)

HCl > HClO > HBrO > HIO

B)

HIO > HBrO > HClO > HCl

C)

HCl > HIO > HBrO > HClO

D)

HClO > HCl > HBrO > HIO

E)

HClO > HBrO > HCl > HIO

34. Which of the following statements is incorrect?

A)

One reason why HCl is a stronger acid than HF is that the H–Cl bond is weaker

than the H–F bond.

B)

F– is a stronger base than Cl–.

C)

One reason why HCl is a stronger acid than HF is that Cl is more electronegative

than F.

D)

The acids HBr and HI both appear equally strong in water.

E)

One reason why HCl is a stronger acid than HF is that Cl has a larger atomic radius

than F.

35. Which solution has the highest pH?

A)

0.10 M HBr(aq)

B)

0.10 M HI(aq)

C)

0.10 M HF(aq)

D)

0.10 M HCl(aq)

E)

0.10 M HClO4(aq)

36. Which of the following is the strongest acid in aqueous solution?

A)

H3AsO4

B)

H3PO4

C)

H3PO3

D)

H3SbO4

E)

H3AsO3

37. Rank the following in order of decreasing acid strength: H2O, H2S, H2Se, H2Te

A)

H2Te > H2Se > H2S > H2O

B)

H2O > H2S > H2Se > H2Te

C)

H2Se > H2Te > H2S > H2O

D)

H2S > H2Te > H2Se > H2O

E)

H2Se > H2S > H2Te > H2O

38. Which of the following is the strongest acid?

A)

HClO2

B)

HCl

C)

HClO4

D)

HClO

E)

HClO3

39. Which of the following solutes, dissolved in 1.0 kg of water, would be expected to provide

the fewest particles and to freeze at the highest temperature?

A)

0.10 mol HClO

B)

0.10 mol HClO3

C)

0.10 mol HClO2

D)

0.10 mol HClO4

E)

0.10 mol HCl

40. Rank H3PO4, H2PO4–, and HPO42– in order of increasing acid strength.

A)

HPO42– < H2PO4– < H3PO4

B)

H2PO4– < HPO42– < H3PO4

C)

H2PO4– < H3PO4 < HPO42–

D)

HPO42– < H3PO4 < H2PO4–

E)

H3PO4 < H2PO4– < HPO42–

41. The ionization constant of water at a temperature above 25°C is 1.7  10–14. What is the pH

of pure water at this temperature?

2H2O(l) H3O+(aq) + OH–(aq)

A)

7.88

B)

5.68

C)

6.88

D)

13.85

E)

7.00

42. The autoionization of water, as represented by the equation below, is known to be

endothermic. Which of the following correctly states what occurs as the temperature of

water is raised?

H2O(l) + H2O(l) H3O+(aq) + OH–(aq)

A)

The pH of the water decreases, and the water becomes more acidic.

B)

The pH of the water decreases, and the water remains neutral.

C)

The pH of the water increases, and the water remains neutral.

D)

The pH of the water does not change, and the water remains neutral.

E)

The pH of the water increases, and the water becomes more acidic.