Chapter 9

Question 1

In the Brφnsted theory, both acids and bases are defined in terms of how substances lose or gain

a. OH−-
b. H3O+
c. H+
d. Cl−

Answer 1

c. H+

Question 2

Identify all Brφnsted bases in the following reactions.
      \+ H2O  HN3 + OH−
a.  H2O 
b. ?   
c.  OH− 
d.  more than one response is correct

Answer 2

d. more than one response is correct

Question 3

What is the function of in the first ionization of citric acid?
H3C6H5O7 → H+ +
a. The ion serves as an Arrhenius acid in this reaction.
b. The ion serves as an Arrhenius base in this reaction.
c. The ion serves as the conjugate base of the acid, H3C6H5O7.
d. The ion serves as the conjugate acid of the base, H3C6H5O7.

Answer 3

c. The ion serves as the conjugate base of the acid, H3C6H5O7.

Question 4

Which of the following is present in pure water?

a. H3O+
b. OH−
c. H2O
d. more than one response is correct

Answer 4

d. more than one response is correct

Question 5

Which of the following statements is true for neutral solutions in which water is the solvent?

a. Neutral solutions contain no H3O+ ions.
b. Neutral solutions contain no OH− ions.
c. Neutral solutions contain H3O+ and OH− ions in equal concentrations.
d. More than one response is correct.

Answer 5

c. Neutral solutions contain H3O+ and OH− ions in equal concentrations.

Question 6

A water solution is found to have a molar OH− concentration of 3.2 × 10^−5. The solution would be classified as

a. acidic
b. basic
c. neutral
d. can’t be classified

Answer 6

b. basic

Question 7

What volume of 6.0 M HNO3 would be needed to make 500 mL of 0.50 M solution?

a. 6 mL
b. 417 mL
c. 42 mL
d. 6 liters

Answer 7

c. 42 mL

Question 8

What are the missing products in the following reaction when it is written as a full equation?
     2HBr + SrCO3 → \_\_\_\_ + \_\_\_\_ + H2O
a.  SrBr2 + CO2 
b.  SrBr2 +  
c.  Sr2 + H2CO3 
d.  HBr + CO2

Answer 8

a. SrBr2 + CO2

Question 9

In the following reaction, all substances are soluble, and all dissociate except H2O. Identify the spectator ions.
     HCl + KOH → KCl + H2O
a.  H+ and OH− 
b.  K+ and Cl− 
c.  H+ and K+ 
d.  Cl− and OH−

Answer 9

b. K+ and Cl−

Question 10

The cation (positive ion) in a salt comes from

a. an acid
b. a base
c. either an acid or a base
d. water

Answer 10

b. a base

Question 11

What salt would be produced by the reaction of H2SO4 with LiHCO3?

a. Li2S
b. LiSO4
c. Li2SO4
d. Li2CO3

Answer 11

c. Li2SO4

Question 12

The molar concentration of OH in a water solution is 1.0 × 10−9. The pH of the solution is
a.  9.00 
b.  5.00 
c.  > 9.00 
d.

Answer 12

b. 5.00

Question 13

The molar concentration of H+ ions in a solution is 5.8 × 10−9. The pH is

a. 9.00
b. 5.80
c. between 8.00 and 9.00
d. between 9.00 and 10.00

Answer 13

c. between 8.00 and 9.00

Question 14

A solution for which [OH−] = 3.0 × 10^−10 is classified as

a. acidic
b. basic
c. neutral
d. more than one response is correct

Answer 14

a. acidic

Question 15

The classification of an acid or base as weak or strong is based upon

a. the solubility of the acid or base
b. the extent of dissociation of the acid or base
c. the concentration of acid or base in solution
d. more than one response is correct

Answer 15

b. the extent of dissociation of the acid or base

Question 16

A 25.00 mL sample of hydrochloric acid solution, HCl, is titrated with 0.0512 M NaOH solution. The volume of NaOH solution required is 21.68 mL. What is the molarity of the HCl solution?

a. 0.0444
b. 0.0590
c. 0.0295
d. 0.0148

Answer 16

a. 0.0444

Question 17

Which of the following salts would produce a basic solution (pH higher than 7) upon being dissolved in pure, distilled water?

a. NaCl
b. Na2CO3
c. Mg(NO3)2
d. NH4Cl

Answer 17

b. Na2CO3

Question 18

Which salt shifts the pH when dissolved in water?

a. KCl
b. Al(NO3)3
c. NaCl
d. NaNO3

Answer 18

b. Al(NO3)^3

Question 19

Which of the following mixtures would represent a buffer?

a. sodium chloride/hydrochloric acid
b. sodium sulfate/sulfuric acid
c. sodium formate/formic acid
d. none of these

Answer 19

c. sodium formate/formic acid

Question 20

The term, strong acid, refers to:

a. the number of hydrogens attached to the acid molecule
b. the speed at which it will dissolve metal
c. if it will cause burns to the skin
d. the ability for the acid to completely dissociate in solution

Answer 20

d. the ability for the acid to completely dissociate in solution

Question 21

A patient comes to you suffering from a battery acid burn (sulfuric acid). What is the best thing to use to neutralize the acid, while you continue to run cool water over the affected area?

a. a 1 M sodium hydroxide solution (NaOH)
b. a 1 M sodium bicarbonate solution (NaHCO3)
c. a 1 M acetic acid solution (CH3COOH)
d. a 1 M carbonic acid solution (H2CO3)

Answer 21

b. a 1 M sodium bicarbonate solution (NaHCO3)

Question 22

A reaction in which an acid and a base react completely, leaving only a salt and water, is referred to as a(n)

a. hydrolysis reaction
b. neutralization reaction
c. oxidation reaction
d. none of the choices

Answer 22

b. neutralization reaction

Question 23

What is the pKb of an acid with a Ka of 1.82 × 10^−5?

a. 4.74
b. −4.74
c. 9.26
d. −9.26

Answer 23

c. 9.26

Question 24

When a strong acid is added to a weak base and mixed, which of the following would not be produced?

a. conjugate acid
b. conjugate base
c. salt
d. water

Answer 24

b. conjugate base

Question 25

Which of the following would you expect to be a weak electrolyte?

a. acetic acid
b. sodium acetate
c. water
d. more than one answer is correct

Answer 25

d. more than one answer is correct