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Acids and Bases Review

Total questions: 116

Worksheet time: 4hrs 35mins

Name
Class
Date
1.

Which of the following is the strongest base?

a)

oven cleaner - 13.5

b)

lemon juice - 2.5

c)

soap - 10

d)

blood - 7.4

2.

Which of the following is the weakest base?

a)

oven cleaner - 13.5

b)

lemon juice - 2.5

c)

soap - 10

d)

blood - 7.4

3.

Which of the following is a strong base?

a)

NH3

b)

HCl

c)

LiOH

d)

Mg(OH)2

4.

Which of the following best describes a Bronsted-Lowry base?

a)

It increases the amount of H+ in solution

b)

It increases the amount of OH- in solution

c)

It is a proton acceptor

d)

It is a proton donor

5.

Identify which is NOT a strong acid

a)

HNO3

b)

H2SO4

c)

HI

d)

H2CO3

6.

Which of the following is NOT a name for H+ (H3O+)?

a)

Hydronium Ion

b)

Hydrogen Ion

c)

Hydroxide Ion

d)

Proton

7.

if the pOH of a solution is 2.8 what is the pH?

a)

2.8

b)

7.2

c)

0.45

d)

11.2

8.

If the H+ of a solution is 9.1 x 10-3, what is the pH?

a)

2.0

b)

3.0

c)

11

d)

12

9.

If the H+ concentration of a solution is 2.8 x 10-9, what is the pOH?

a)

9.00

b)

8.55

c)

5

d)

5.45

10.

Which is NOT true about indicators?

a)

They each have a certain pH where they change color

b)

They come in a variety of colors

c)

They are useful in titrations

d)

They neutralize acids and bases

11.

Which of the following is a weak acid?

a)

HCl

b)

HBr

c)

HI

d)

HF

12.
Acids react with
a)
water to produce bases and salts
b)
salts to produce bases and water
c)
neither bases, salts nor water
d)
bases to produce salts and water
13.

A substance is found to have the following characteristics:


Very bitter taste

Feels slippery to the touch

Produces OH- ions when dissolved in water


In what category would the substance be classified?

a)

acid

b)

base

c)

enzyme

d)

fatty acid

14.

The pH of a solution is 2.0. What is the [OH-] concentration?

a)

1x10-12M

b)

12 M

c)

1x10-2M

d)

2 M

15.
Which of the following statements is correct?
a)
Blue litmus paper turns red when placed in a base.
b)
Red litmus paper turns blue when placed in a base.
c)
Blue litmus paper stays blue when placed in an acid.
d)
Red litmus paper stays red when placed in a base.
16.

What is the pH of a solution where the [H+] is 1.0 x 10-11?

a)

11

b)

13

c)

14

d)

1

17.

What is the pOH of a 1 x 10-8 M solution of HNO3?

a)

8

b)

6

c)

7

d)

9

18.

What is the [H+] if the pH is 4.0?

a)

1.0 x 10-10 M

b)

1.0 x 10-4 M

c)

1.0 x 10-14 M

d)

1.0 x 10-7 M

19.
What is the pOH of a solution that has a pH of 2?
a)
10
b)
12
c)
14
d)
1
20.

Phenolophalein turns from clear to pink when the pH turns

a)

acidic

b)

basic

c)

saline

d)

ionic

21.

What completely ionizes in solution?

a)

Weak acids

b)

Strong acids

c)

Strong Salts

d)

Neutral salts

22.
Which of the following word pairs correctly completes the sentence below?
_______ are corrosive substances characterized as having a strong smell, a sour taste, and a _______.
a)
Acids; pH less than 7
b)
Acids; pH greater than 7
c)
Bases; pH greater than 7
d)
Bases; pH less than 7
23.
The esophagus is the tube that connects the mouth to the stomach. Heartburn occurs when some of the stomach juices flow backwards up the esophagus. To help relieve heartburn, a person should take medicine that is
a)
neutral
b)
basic
c)

acidic or basic.
d)
acidic
24.
Holly has an unknown substance in a beaker. She wants to determine the relative pH of the unknown substance. She places a piece of blue litmus paper into the substance, and the litmus paper stays blue.
The substance in the beaker
a)
is a base.
b)
has a neutral pH.
c)
is an acid.
d)
does not have a pH.
25.
Which of the following is a base?
a)
orange juice
b)
water
c)
vinegar
d)
dishwashing detergent
26.
What would be considered the weakest base? 
a)
8
b)
14
c)
7.8
d)
11.6
27.
Many cleaning solutions are bases. Which of the following is a property of most bases?
a)
feels slippery
b)
white color
c)
can only be liquid
d)
tastes sour
28.

Which of these pH values represent an acid?

a)

4

b)

8

c)

10

d)

12

29.

Milk is a very weak acid. What might its pH value be?

a)

6.5

b)

7.8

c)

4.2

d)

12.2

30.

When acids react with metals, they produce hydrogen gas and salt.

a)

True

b)

False

31.
What is the [OH-] if the pH is 4.9?
a)
7.94 x 10-10 M
b)
1.0 x 10-4  M
c)
7.94 x 10-14 M
d)
4.9 x 10-10 M
32.
If [H3O+]=1.7 x 10-3 M, what is the pH of the solution?
a)
2.13
b)
1.81
c)
2.77
d)
2.42
33.
If a solution has a [H+] of
1.2 x 10-4M what is the [OH-]?
a)
8.3 x 10-4M 
b)
8.3 x 10-11M 
c)
1.2 x 1010M 
d)
1.2 x 10-4M 
34.
If [H3O+]=1.7 x 10-3 M, what is the pH of the solution?
a)
2.13
b)
1.81
c)
2.77
d)
2.42
35.
What is the pH of a
4.3 x 10-7 solution of H2CO3?
a)
7
b)
6.4
c)
7.6
d)
4.3
36.
What is the pH of a 3 x 10-3 M solution of Al(OH)3?
a)
11.5
b)
2.5
c)
3
d)
3.1
37.
A solution prepared with the base CN- (Kb = 2.5 x 10-5) has a concentration of 0.25 M of the base.  Calculate the pH for the solution.
a)
4.6
b)
9.4
c)
2.6
d)
11.4
38.
A solution contains 0.04 M of a weak acid. Calculate the pH of the solutionknowing that the Ka for the acid is 1.6 x 10-7
a)
It is not possible to solve if the identity of the acid is not known
b)
4.1
c)
4.9
d)
Because the Ka is very small, the pH is close to neutral (about 6)
39.

HZ is a weak acid. An aqueous solution of HZ is prepared by dissolving 0.020 mol of HZ in sufficient water to yield 1.0 L of solution. The pH of the solution was 4.93 at 25.0°C. The Ka of HZ is

a)

1.2 x10-5

b)

9.9 x 10-2

c)

1.4 x 10-10

d)

6.9 x 10-9

40.

The Ka of hypochlorous acid (HClO) is 3.0 x 10-8 at 25.0°C. Calculate the pH of a 0.0385 M hypochlorous acid solution.

a)

1.41

b)

8.94

c)

4.47

d)

7.52

41.

The Ka of hypochlorous acid (HClO) is 3.0 x 10-8 at 25.0°C. Calculate the pH of a 0.0385 M hypochlorous acid solution.

a)

1.41

b)

8.94

c)

4.47

d)

7.52

42.

What is the concentration (in M) of hydroxide ions in a solution at 25.0 °C with pH = 4.282?

a)

9.72

b)

1.91 x 10-10

c)

5.22 x 10-5

d)

1.66 x 104

43.

In which of the following aqueous solutions does the weak acid exhibit the highest percentage ionization?

a)

0.01 M HC2H3O2    (Ka = 1.8 x 10-5)

b)

0.01 M HNO2    (Ka = 4.5 x 10-4)

c)

0.01 M HF    (Ka = 6.8 x 10-4)

d)

0.01 M HClO    (Ka = 3.0 x 10-8)

44.

The Ka of hydrofluoric acid (HF) at 25.0°C is 6.8 x 10-4. What is the pH of a 0.35 M aqueous solution of HF?

a)

3.25

b)

1.81

c)

3.64

d)

1.22

45.

Determine the pH of a 0.35 M aqueous solution of CH3NH2 (methylamine). The Kb of methylamine is 4.4 x 10-4.

a)

10.00

b)

3.86

c)

12.09

d)

1.96

46.

An aqueous solution contains 0.050 M of methylamine. The concentration of hydroxide ion in this solution is __________ M. Kb for methylamine is 4.4 x 10-4.

a)

0.050

b)

2.2 x 10-5

c)

2.9 x 10-3

d)

4.5 x 10-3

47.

The Ka for HCN is 4.9 x 10-10. What is the value of Kb for CN-?

a)

2.0 x 10-5

b)

4.0 x 10-6

c)

4.9 x 10-24

d)

2.0 x 109

48.

Calculate the pH of 0.726 M anilinium hydrochloride (C6H5NH3Cl) solution in water, given that Kb for aniline is 3.83 x 10-4.

a)

1.77

b)

12.64

c)

5.36

d)

8.64

49.

Kb for NH3 is 1.8 x 10-5. What is the pH of a 0.35 M aqueous solution of NH4Cl at 25.0°C?

a)

9.76

b)

4.35

c)

9.11

d)

4.86

50.

The Ka for formic acid (HCO2H) is 1.8 x 10-4. What is the pH of a 0.35 M aqueous solution of sodium formate (NaHCO2)?

a)

11.64

b)

5.42

c)

4.26

d)

8.64

51.

Ka for HCN is 4.9 x 10-10. What is the pH of a 0.068 M aqueous solution of sodium cyanide?

a)

2.96

b)

11.07

c)

13.24

d)

7.00

52.

The pH of a 0.15 M aqueous solution of NaZ (the sodium salt of HZ) is 10.7. What is the Ka for HZ?

a)

1.6 x 10-6

b)

6.0 x 10-9

c)

8.9 x 10-4

d)

1.3 x 10-12

53.

A 0.1 M aqueous solution of __________ will have a pH of 7.0 at 25.0 °C.

a)

NaOCl

b)

KCl

c)

NH4Cl

d)

Ca(OAc)2

54.

Buffer is defined as

a)

ability to resist pH change

b)

ability to prevent pH from decreasing

c)

ability to resist a pH increase

d)

ability to resist pH change when small amount of acid or base are added

55.
Acidic buffer is made up of
a)
weak acid and weak base
b)
weak acid and its conjugate salt
c)
weak acid and its conjugate base
d)
strong acid and its conjugate base
56.
Basic buffer is made up of
a)
weak base and weak acid
b)
weak base and its conjugate salt
c)
weak base and its conjugate acid
d)
strong base and its conjugate acid
57.
Which solution A and B of equal volume and concentration mixed together to form a buffer?
a)
Nitric acid and potassium hydroxide
b)
Nitric acid and potassium nitrate
c)
Propanoic acid and potassium hydroxide
d)
Propanoic acid and potassium propanoate
58.
Which of the following pair is correct?
a)
(FeCI3 - acidic) (Na2CO3 - basic)
b)
(FeCI3 - neutral) (Na2CO3 - basic)
c)
(FeCI3 - acidic) (Na2CO3 - neutral)
d)
(FeCI3 - neutral) (Na2CO3 - neutral)
59.

Which mixture of strong acid and weak base could produce a buffer solution?

a)

A

b)

B

c)

C

d)

D

60.
Which will produce an acidic salt?
a)
A
b)
B
c)
C
d)
D
61.
Which will produce an alkaline salt?
a)
A
b)
B
c)
C
d)
D
62.
The salt shown below is
a)
Acidic
b)
Basic
c)
Neutral
d)
None of the above
63.
What kind of acid does not completely dissociate?
a)
weak
b)
strong
c)
ionic
d)
pH
64.
Water is ____, meaning it can be both and acid or a base
a)
Amphoteric
b)
Atmospheric
c)
Amphibious
d)
Aqueous
e)
Amplified
65.

When making a buffer of pH = 5, acids with the following Ka values are available. Which would be the best acid to use?

a)

1.8 x 10-5

b)

1.8 x 10-8

c)

4.9 x 10-10

d)

3.0 x 10-8

66.

A buffer has a pH of 4.85 and contains formic acid and potassium formate. What can you conclude about the concentrations of the components of the buffer? The Ka of formic acid is 1.8 x 10-4.

a)

Formic acid > Potassium formate

b)

Formic acid < Potassium formate

c)

Formic acid = Potassium formate

d)

More information is needed to determine the relative concentrations

67.
What is the pH of a buffer that is 0.08 M NaA and 0.1 HA. The Ka of HA = 1.0 x 10-4.
a)
2.16
b)
3.91
c)
4.00
d)
4.10
68.

What might happen if buffers did not exist within the human body?

a)

Our blood and other bodily fluids might become too acidic or basic.

b)

Our stomach acid would not be able to break down food.

c)

We would not be able to process glucose within our cells.

d)

We would not be able to inhale oxygen into our lungs.

69.
Which mixtures act as buffer solutions?
a)
I and II
b)
I and III
c)
II and III
d)
I, II and III
70.
Which solutions have a pH less than 7?
a)
I and II
b)
I and III
c)
II and III
d)
I, II and III
71.
Which mixtures could act as buffers?
a)
I and II
b)
I and III
c)
II and III
d)
I, II and III
72.
Suppose you have a solution of 0.3 M HBrO and 0.3 M BrO. You add a small amount of NaOH to this buffer solution. What is the reaction that takes place?
a)
H+ + BrO- --> HBrO
b)
OH- + H+ --> H2O
c)
OH- + HBrO --> H2O + BrO-
d)
OH- + BrO- --> O-2 + HBrO
73.

Which one of these substances would NOT dissolve more readily by the addition some acid?

a)

ZnCO3

b)

Fe(CN)2

c)

Cu3(PO4)2

d)

Ag2S

e)

KCl

74.

A sour taste is a characteristic of:

a)

acids

b)

bases

c)

neutral

d)

pH scale

75.

Which is a characteristic of a base?

a)

tastes sour

b)

found mostly in foods

c)

feels slippery

d)

turn litmus paper red

76.

According to Arrhenius, what is the definition of an ACID?

a)

a substance that contains hydroxide and ionizes to produce OH-

b)

a substance that contains hydrogen and ionizes to produce H+

c)

a substance that contains hydrogen and ionizes to produce OH-

d)

a substance that contains hydroxide and ionizes to produce H+

77.

NaOH is:

a)

an Arrhenius base

b)

an Arrhenius acid

c)

neither an acid nor a base

d)

both an acid and a base

78.

When using the Arrhenius model, what types of ions indicate that a compound is a base?

a)

H+1

b)

OH-1

79.

Which substance below would be an Arrhenius Acid?

a)

CH4

b)

C2H6

c)

NaCl

d)

H3PO4

80.

Which substance below is an Arrhenius Base?

a)

CH3OH

b)

KOH

c)

HCl

d)

HF

81.

An Arrhenius acid:

a)

donates H+ to another substance

b)

accepts H+ from another substance

c)

produces H+

d)

produces OH-

82.

An Arrhenius base:

a)

donates H+

b)

accepts H+

c)

produces H+

d)

produces OH-

83.

NaOH is:

a)

an Arrhenius base

b)

an Arrhenius acid

c)

neither an acid nor a base

d)

both an acid and a base

84.

A compound that when in an aqueous solution increase the the number of hydrogen ions or protons is called

a)

acid

b)

arrhenius acid

c)

arrhenius base

d)

base

85.

HC2H3O2 + H2O ---> H3O+ + C2H3O2- This reaction shows acetic acid reacting with water. What is the arrrhenius acid above?

a)

H2O

b)

HC2H3O2

c)

H3O+

d)

C2H3O2

86.

What does a very large Ka value indicate?

a)

a strong acid

b)

a weak acid

87.

Which statement is true about ammonia, NH3?

a)

It is an Arrhenius base.

b)

It is a Bronsted-Lowry base.

c)

both (A) & (B)

d)

neither (A) nor (B)

88.
The following statement is true for arrhenius acid and base EXCEPT
a)
Arrhenius acid produces H+ ions
b)
Arrhenius base produces OH- ions
c)
H2O need to be present for arrhenius acid base to dissociate
d)
Hydrogen atoms that make the solution acidic
89.

A Bronsted Lowry base:

a)

donates H+ to another substance

b)

accepts H+ from another substance

c)

produces H+

d)

produces OH-

90.
The Acid-Base classification system that defined a __________ is any compound that can donate a proton (an H+ ion) to an appropriate acceptor. A _________ is a compound that can remove (or accept) a proton.
a)
Bronsted-Lowry
b)
Arrhenius acid-base
c)
Lewis acid-base
d)
Monoprotic and Polyprotic Acids
91.
What is the conjugate acid in the following equation?
a)
PO43- 
b)
HNO3 
c)
NO3- 
d)
HPO42-
92.
What is the conjugate base in the following reaction?
a)
HCO3- 
b)
HCl
c)
 H2CO3 
d)
Cl-
93.
What is the conjugate base of HCO3-?
a)
HCO3-
b)
H2CO3-
c)
H2CO3
d)
CO32-
94.
Which accepts protons?
a)
Brønsted-Lowry Acids
b)
Brønsted-Lowry Bases
c)
Arrhenius Acids
d)
Arrhenius Bases
95.
When citric acid is produced by the cells of an orange and dissolves in water, it produces a relatively small number of hydronium ions. Citric acid is best described as a
a)
concentrated acid. 
b)
weak acid. 
c)
dilute acid.
d)
strong acid.
96.
The Kw constant is:
a)
1.0 x 10-14
b)
1.0 x 1014
c)
6.022 x 1023
d)
6.0634 x 10-34
97.

The Acid-Base classification system that defined any chemical species that accepts a pair of electrons as an acid, and a base is a chemical species that donates a pair of electrons.

a)

Bronsted-Lowry

b)

Arrhenius acid-base

c)

Lewis acid-base

d)

Monoprotic and Polyprotic Acids

98.

Accepts a pair of electrons

a)

Lewis Acid

b)

Lewis Base

c)

Bronsted Lowry Acid

d)

Arrhenius Base

99.

Lewis bases are defined as

a)

H+ acceptors

b)

electron pair acceptors

c)

H+ donors

d)

electron pair donors

100.

Classify the following molecule

a)

Lewis Acid

b)

Lewis Base

101.

Classify the following molecule

a)

Lewis Acid

b)

Lewis Base

102.

Classify this acid.

a)

Arrhenius Acid

b)

Bronsted Lowry Acid

c)

Lewis Acid

103.

True or False? All acids are Lewis acids.

a)

True

b)

False

104.

Classify this acid.

a)

Arrhenius Acid

b)

Bronsted Lowry Acid

c)

Lewis Acid

105.

Classify this acid.

a)

Arrhenius Acid

b)

Bronsted Lowry Acid

c)

Lewis Acid

106.
The Acid-Base classification system that defined any chemical species that accepts a pair of electrons as a _______, and a _________ is a chemical species that donates a pair of electrons.
a)
Bronsted-Lowry
b)
Arrhenius acid-base
c)
Lewis acid-base
d)
Monoprotic and Polyprotic Acids
107.
The Acid-Base classification system that defined a __________ is any compound that can donate a proton (an H+ ion) to an appropriate acceptor. A _________ is a compound that can remove (or accept) a proton.
a)
Bronsted-Lowry
b)
Arrhenius acid-base
c)
Lewis acid-base
d)
Monoprotic and Polyprotic Acids
108.
Accepts a pair of electrons
a)
Lewis Acid
b)
Arrhenius Acid 
c)
Bronsted Lowry Acid 
d)
Arrhenius Base
109.
An Arrhenius base increases the concentration of OH-.
a)
True
b)
False
110.
A Lewis acid is an electron donor.
a)
True
b)
False
111.
NaOH is a Lewis base.
a)
True
b)
False
112.
If you want to make a buffer with a pH of 2.97, what is the best choice to use?
a)

HF/NaF

b)

HCOOH/NaCOOH

c)

HCN/NaCN

113.
Accepts a pair of electrons
a)
Lewis Acid
b)
Arrhenius Acid 
c)
Bronsted Lowry Acid 
d)
Arrhenius Base
114.

In the equation below, what is the Bronsted Lowry acid (donates H+)?

HCl + NH3 → Cl- + NH4+

a)

HCl

b)

NH3

c)

Cl-

d)

NH4+

115.

Which reactant in the following equation is a Bronsted Lowry acid?

H2O + HCl → H3O+ + Cl-

a)

Water

b)

Hydrogen chloride

c)

Hydronium

d)

Chloride

116.

Which product in the following equation is a conjugate base?

H2O + HCl → H3O+ + Cl-

a)

Water

b)

Hydrogen chloride

c)

Hydronium

d)

Chloride

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