Acids, Bases, and Salts

Question 1

Which of the following substances could behave as an Arrhenius base?

Select one:

a. Na2CO3
b. Na3PO4
c. K2S
d. KOH

Answer 1

d. KOH

Question 2

According to the Arrhenius theory, what is produced when an acid dissolves in water?

Select one:

a. H+
b. OH-
c. H3O+
d. NH4+

Answer 2

a. H+

Question 3

In the Bronstead theory, both acids and bases are defined in terms of how substances behave toward

Select one:

a. OH- ions.
b. H3O+ ions.
c. H+ ions (protons).
d. Cl- ions.

Answer 3

c. H+ ions (protons).

Question 4

The procedure commonly used to determine the amount of base in a solution by adding a measured quantity of acid is called

Select one:

a. dissociation.
b. titration.
c. ionization.
d. normalization.

Answer 4

b. titration.

Question 5

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

Select one:

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

Answer 5

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

Question 6

Which of the following is a property of basic solutions?

Select one:

a. sour taste
b. slippery feel
c. change blue litmus to red

Answer 6

b. slippery feel

Question 7

Many cleaning agents contain bases because bases react with

Select one:

a. salts.
b. oils.
c. acids.
d. water.

Answer 7

a. salts.

Question 8

Salts contain a cation (positive ion) that comes from

Select one:

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

Answer 8

b. a base.

Question 9

Some salts isolated by evaporating a solution in which they are dissolved retain water that is called

Select one:

a. the water of hydration.
b. hydrate.
c. hydro water.
d. crystallization water.

Answer 9

a. the water of hydration.

Question 10

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

Select one:

a. the solubility of the acid or base.
b. the extent of dissociation of dissolved acid or base.
c. the concentration of acid or base in solution.

Answer 10

b. the extent of dissociation of dissolved acid or base.

Question 11

What volume of 6 M HNO3 would be needed to make 500 mL of 0.5 M solution?

Select one:

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

Answer 11

c. 42 mL

Question 12

A solution for which [H+] = 1.0 X 10-5 will have a pH of

Select one:

a. 1.0.
b. 4.0.
c. 5.0.
d. -5.0.

Answer 12

c. 5.0.

Question 13

Identify two Bronsted base(s) in the reaction:

HIO3 + H2O –> IO-3 + H3O+

Select one:

a. HIO3 and H2O
b. HIO3 and H3O+
c. HIO3 and IO-3
d. H2O and IO-3

Answer 13

c. HIO3 and IO-3

Question 14

A solution has a pH of 11.6. The value of [H+] is

Select one:

a. 2.5 X 10^-4
b. 4.0 X 10^-3
c. 4.0 X 10^-11
d. 2.5 X 10^-12

Answer 14

d. 2.5 X 10^-12

Question 15

A solution’s pH of 8.72. What is the value of [H+]?

Select one:

a. 5.2 X 10^-6
b. 1.9 X 10^-9
c. 5.2 X 10^-8
d. 1.9 X 10^-5

Answer 15

b. 1.9 X 10^-9

Question 16

A 25.00 mL sample of hydrochloric acid, 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?

Select one:

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

Answer 16

a. 0.0444

Question 17

How many equivalents are contained in 0.25 moles of H2SO3?

Select one:

a. 0.25
b. 0.13
c. 0.50
d. 0.75

Answer 17

c. 0.50

Question 18

What are the missing products in the following reaction when it is written as a full equation?

2HBr + SrCO3  ____ + ____ + H2O

Select one:

a. SrBr2 + CO2
b. SrBr2 + HCO-3
c. Sr2 + H2CO3
d. HBr + CO2

Answer 18

a. SrBr2 + CO2

Question 19

What would be the pH of a solution of NH4Cl in pure water?

Select one:

a. higher than 7
b. lower than 7
c. equal to 7

Answer 19

b. lower than 7

Question 20

In the following reaction, all substances are soluble, and all dissociate except H2O. Identify the specetator ions

HCl + KOH  KCl + H2O

Select one:

a. H+ and OH-
b. K+ and Cl-
c. H+ and K+
d. Cl- and OH-

Answer 20

b. K+ and Cl-