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Types of Acids and Bases

Total questions: 120

Worksheet time: 2hrs 49mins

Name
Class
Date
1.

A sour taste is a characteristic of:

a)

acids

b)

bases

c)

neutral

d)

pH scale

2.

Which is a characteristic of a base?

a)

tastes sour

b)

found mostly in foods

c)

feels slippery

d)

turn litmus paper red

3.

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+

4.

NaOH is:

a)

an Arrhenius base

b)

an Arrhenius acid

c)

neither an acid nor a base

d)

both an acid and a base

5.
If a solution is basic which ion will be more present?
a)
H+
b)
K+
c)
OH-
d)
H-
6.

Which of the following will conduct electricity? Select all that apply

a)

Acidic solutions

b)

Basic solutions

c)

Ionic solutions

d)

Neutral covalent solutions

7.

Which of the following are properties of acids but not bases? Select all that apply.

a)

Changes the color of an indicator

b)

Sour taste

c)

Reacts with metals to produce hydrogen gas

d)

Feels slippery

8.

Neutralization is the process of an acid and a base reacting to form what? Select all that apply

a)

An ionic salt

b)

Hydronium ions

c)

NaCl

d)

Water

9.

Which of the following is a binary acid?

a)

H2SO4

b)

HNO3

c)

H2Se

d)

HC2H3O2

10.

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

a)

H+1

b)

OH-1

11.

Which substance below would be an Arrhenius Acid?

a)

CH4

b)

C2H6

c)

NaCl

d)

H3PO4

12.

Which substance below is an Arrhenius Base?

a)

CH3OH

b)

KOH

c)

HCl

d)

HF

13.

An Arrhenius acid:

a)

donates H+ to another substance

b)

accepts H+ from another substance

c)

produces H+

d)

produces OH-

14.

An Arrhenius base:

a)

donates H+

b)

accepts H+

c)

produces H+

d)

produces OH-

15.

NaOH is:

a)

an Arrhenius base

b)

an Arrhenius acid

c)

neither an acid nor a base

d)

both an acid and a base

16.

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

17.

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

18.

Which compound is an Arrhenius acid?

a)

CaO

b)

K2O

c)

HCl

d)

NH3

19.

A substance donates a proton, H+. It should be classified as a:

a)

Arrhenius base

b)

Bronsted-Lowry acid

c)

Bronsted-Lowry base

d)

Lewis acid

20.

What type of substance is Sr(OH)2?

a)

an Arrhenius acid

b)

an Arrhenius base

c)

neither

21.

Like most of the group 2 metal hydroxides, Sr(OH)2 is a strong base.

a)

TRUE

b)

FALSE

22.

What type of substances are LiBr & PCl3?

a)

Arrhenius acids

b)

Arrhenius bases

c)

neither

23.

Vinegar is a solution of CH3COOH(aq). It is:

a)

an Arrhenius acid

b)

an Arrhenius base

c)

neither

24.

What does a very large Ka value indicate?

a)

a strong acid

b)

a weak acid

25.

What does a very small Kb value indicate?

a)

a strong base

b)

a weak base

26.

The substance whose dissociation is shown in the graph above is likely a:

a)

a weak Arrhenius base

b)

a strong Arrhenius base

c)

a weak Arrhenius acid

d)

a strong Arrhenius acid

27.

Identify the TWO strong acids from the list below.

a)

HBr

b)

HF

c)

H3PO4

d)

HCN

e)

HNO3

28.

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)

29.
Forms a OH- hydroxide ion
a)
Lewis Base
b)
Arrhenius Base
c)
Bronsted Lowry Base
d)
Bronsted Lowry Acid
30.
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
31.

A Bronsted Lowry base:

a)

donates H+ to another substance

b)

accepts H+ from another substance

c)

produces H+

d)

produces OH-

32.

Which of the following does not describe an Arrhenius or Bronsted Lowry acid or base?

a)

Produces H+

b)

Produces OH-

c)

Donates H+ to another substance

d)

Donates OH- to another substance

33.
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
34.
What is the conjugate acid in the following equation?
a)
PO43- 
b)
HNO3 
c)
NO3- 
d)
HPO42-
35.
What is the conjugate base in the following reaction?
a)
HCO3- 
b)
HCl
c)
 H2CO3 
d)
Cl-
36.
What is the conjugate base of HCO3-?
a)
HCO3-
b)
H2CO3-
c)
H2CO3
d)
CO32-
37.
Which accepts protons?
a)
Brønsted-Lowry Acids
b)
Brønsted-Lowry Bases
c)
Arrhenius Acids
d)
Arrhenius Bases
38.
What substances increase H+ ion concentrations when dissolved in water?
a)
Brønsted-Lowry Acids
b)
Brønsted-Lowry Bases
c)
Arrhenius Acids
d)
Arrhenius Bases
39.
What substances increase OH- ion concentrations when dissolved in water?
a)
Brønsted-Lowry Acids
b)
Brønsted-Lowry Bases
c)
Arrhenius Acids
d)
Arrhenius Bases
40.
Which donates protons?
a)
Brønsted-Lowry Acids
b)
Brønsted-Lowry Bases
c)
Arrhenius Acids
d)
Arrhenius Bases
41.
When a hydrogen ion is released what does the solution become?
a)
Basic
b)
Acidic
c)
Amphoteric
d)
Proton
42.
When a hydroxide ion is released what does the solution become?
a)
Basic
b)
Acidic
c)
Amphoteric
d)
Proton
43.
Which of the following is not a strong acid?
a)
HCl
b)
HF
c)
HBr
d)
HNO3
44.
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.
45.
A chemist is working with a liquid substance that tastes bitter, feels slippery, and conducts an electric current. Which of the following is the chemist most likely working with? 
a)
a salt
b)
a base
c)
an acid
d)
distilled water
46.

Which of these is a weak base?

a)

NH3

b)

KOH

c)

HCOOH

d)

HBr

47.

Which of these is a strong acid?

a)

NH3

b)

CH3COOH

c)

HClO3

d)

HF

48.

Which of the following describes H2SO4

a)

Weak acid

b)

Strong base

c)

Strong acid

d)

Weak base

49.
I have a pOH have 4.23. Am I acidic or basic?
a)
Acidic
b)
Basic
c)
Neutral
50.

A solution contains 0.04 M of a weak acid. Calculate the pH of the solution knowing that the Ka for the acid is 1.6 x 10-7. The answer 4.1

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)

51.
Which of the following is an example of an acid anhydride.
a)
MgO
b)
Na2O
c)
CO2
d)
CaO
52.
WHen 200 mL of 2.0 M NaOH(aq) is added to 500 mL of 1.0 M HCl(aq), the pH of the resulting mixture is closest to 
a)
1.0
b)
3.0
c)
7.0
d)
13.0
53.
What is the pOH of a solution that has a pH of 2?
a)
10
b)
12
c)
14
d)
1
54.

Which chemical is a proton acceptor?

a)

Acid

b)

Base

55.

What is the pH of a 0.053 M solution of potassium hydroxide

a)

6.91

b)

12.72

c)

7.33

d)

1.28

56.

Of the following, which is the strongest acid

a)

HClO

b)

HClO2

c)

HClO3

d)

HClO4

57.

What is the conjugate acid of CO3-2?

a)

CO2-2

b)

HCO22-2

c)

H2CO3

d)

HCO3-1

58.
A compound that donates H+ ions is 
a)
A Bronsted-Lowry Acid
b)
An Arrhenius Acid
c)
A Bronsted-Lowry Base
d)
An Arrhenius Base
59.
Forms a OH- hydroxide ion
a)
Lewis Base
b)
Arrhenius Base
c)
Bronsted Lowry Base
d)
Bronsted Lowry Acid
60.

Water can act as both an acid and a base in an ionization reaction to form H+ and OH– ions. What is this phenomenon called?

a)

neutralization

b)

self-ionization

c)

base dissociation

d)

acid dissociation

61.

Hydrochloric acid (HCl) and acetic acid (HC2H3O2) are both acids. HCl completely dissociates in water, while HC2H3O2 does not. Which of the following statements best describes these two acids?

a)

HCl is a weak acid, HC2H3O2 is a weak acid.

b)

HCl is a strong acid, HC2H3O2 is a strong acid.

c)

HCl is a strong acid, HC2H3O2 is a weak acid.

d)

HCl is a weak acid, HC2H3O2 is a strong acid.

62.

Which of the following is a Brønsted-Lowry base but not an Arrhenius base?

a)

Ca(OH)2

b)

NH3

c)

NaOH

d)

KOH

63.
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
64.

If 25 mL of a Ca(OH)2 solution is needed to neutralize 15 mL of 0.18 M HC2H3O2, what is the concentration of the Ca(OH)2 solution? The answer is 0.054 M

a)

0.216 M

b)

0.108 M

c)

0.3 M

d)

0.054 M

65.

The Acid-Base classification system that defines an acid as any compound that contains hydrogen and ionizes to produce H+ and a base as any compound that contains hydroxide and ionizes to produce OH-

a)

Bronsted-Lowry

b)

Arrhenius acid-base

c)

Lewis acid-base

d)

Monoprotic and Polyprotic Acids

66.

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

67.

The Acid-Base classification system that defined an acid as any compound that can donate a proton (an H+ ion) to an appropriate acceptor. A base 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

68.

Accepts a pair of electrons

a)

Lewis Acid

b)

Lewis Base

c)

Bronsted Lowry Acid

d)

Arrhenius Base

69.

Lewis bases are defined as

a)

H+ acceptors

b)

electron pair acceptors

c)

H+ donors

d)

electron pair donors

70.

Classify the following molecule

a)

Lewis Acid

b)

Lewis Base

71.

Classify the following molecule

a)

Lewis Acid

b)

Lewis Base

72.

Classify this acid.

a)

Arrhenius Acid

b)

Bronsted Lowry Acid

c)

Lewis Acid

73.

True or False? All acids are Lewis acids.

a)

True

b)

False

74.

Which is the correct set of acid properties?

a)

sour taste, corrosive, change litmus from red to blue

b)

sour taste, corrosive, change litmus from blue to red

c)

sweet taste, slippery, change litmus from blue to red

d)

sour taste, slippery, change litmus from blue to red

75.

Classify this acid.

a)

Arrhenius Acid

b)

Bronsted Lowry Acid

c)

Lewis Acid

76.

Classify this acid.

a)

Arrhenius Acid

b)

Bronsted Lowry Acid

c)

Lewis Acid

77.
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
78.
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
79.
Accepts a pair of electrons
a)
Lewis Acid
b)
Arrhenius Acid 
c)
Bronsted Lowry Acid 
d)
Arrhenius Base
80.
An Arrhenius base increases the concentration of OH-.
a)
True
b)
False
81.
An Arrhenius base increases the concentration of OH-.
a)
True
b)
False
82.
HCl is an Arrhenius acid.
a)
True
b)
False
83.
NH3 is an Arrhenius base.
a)
True
b)
False
84.
A Bronsted-lowry base is a proton acceptor.
a)
True
b)
False
85.
NH3 is a Bronsted-Lowry base.
a)
True
b)
False
86.
NaOH is a Bronsted-Lowry base.
a)
True
b)
False
87.
A Lewis acid is an electron donor.
a)
True
b)
False
88.
A Lewis base is an electron donor.
a)
True
b)
False
89.
NaOH is a Lewis base.
a)
True
b)
False
90.
Fe3+ is a Lewis acid.
a)
True
b)
False
91.
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

92.
If you want to make a buffer with a pH of 9.47, what is the best choice to use?
a)

HF/NaF

b)

HCOOH/NaCOOH

c)

HCN/NaCN

93.
If you want your buffer to have a high capacity, you should:
a)
Make the concentration of the acid high and the conjugate base low.
b)
Make sure the concentration of both components is low.
c)
Make the concentration of the acid low and the conjugate base high.
d)
Make sure the concentration of both components is high.
94.
Accepts a pair of electrons
a)
Lewis Acid
b)
Arrhenius Acid 
c)
Bronsted Lowry Acid 
d)
Arrhenius Base
95.

The Acid-Base classification system that defines an acid as any compound that contains hydrogen and ionizes to produce H+ and a base as any compound that contains hydroxide and ionizes to produce OH-

a)

Bronsted-Lowry

b)

Arrhenius acid-base

c)

Lewis acid-base

d)

Monoprotic and Polyprotic Acids

96.

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

HCl + NH3 → Cl- + NH4+

a)

HCl

b)

NH3

c)

Cl-

d)

NH4+

97.

In the equation below, what is the Bronsted Lowry base (accepts H+)?

HCl + NH3 → Cl- + NH4+

a)

HCl

b)

NH3

c)

Cl-

d)

NH4+

98.

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

H2O + HCl → H3O+ + Cl-

a)

Water

b)

Hydrogen chloride

c)

Hydronium

d)

Chloride

99.

Which product in the following equation is a conjugate base?

H2O + HCl → H3O+ + Cl-

a)

Water

b)

Hydrogen chloride

c)

Hydronium

d)

Chloride

100.

What is the Bronsted Lowry base in the following equation?

PO4-3 + HNO3 → NO3- + HPO4-2

a)

PO43-

b)

HNO3

c)

NO3-

d)

HPO42-

101.

What is the conjugate acid in the following equation?

PO4-3 + HNO3 → NO3- + HPO4-2

a)

PO43-

b)

HNO3

c)

NO3-

d)

HPO42-

102.

What is the conjugate base in the following reaction?

HCO3- + HCl → H2CO3 + Cl-

a)

HCO3-

b)

HCl

c)

H2CO3

d)

Cl-

103.

HSO4- + H2O → H3O+ +SO42-

Identify the Bronsted Lowry Acid in the above reaction.

a)

HSO4-

b)

H2O

c)

H3O+

d)

SO42-

104.

CO32- + H2O → HCO3- + OH-

Using the above reaction, which compound is the conjugate base?

a)

CO32-

b)

H2O

c)

HCO3-

d)

OH-

105.

Match each term to the species which it describes for the reaction between hydrochloric acid and sodium hydroxide.

a)

Hydrochloric acid

1.

Bronsted-Lowry Acid

b)

Hydroxide ion

2.

Bronsted-Lowry Base

c)

Water

3.

Conjugate Acid

d)

Chloride ion

4.

Conjugate Base

e)

Sodium ion

5.

No term matches

106.
According to which theory is a base a substance which produces OH- ions in water?
a)
Arrhenius
b)
Bronsted-Lowry
c)
Lewis
107.
According to Bronsted-Lowry acid base theory, an acid is a.....
a)
Proton donor
b)
Proton acceptor
c)
Produces H+ when added to water
d)
Made of H+
108.
According to Lewis acid-base theory, a Lewis base is.....
a)
an electron pair acceptor
b)
an electron pair donor
c)
an oxidising agent
d)
a reducing agent
109.
According to Arrhenius acid-base theory, an acid is....
a)
an H+ acceptor
b)
a H+ donor
c)
a substance that produces H+ in water
d)
anything with an H+
110.
According to which acid-base theory is a base a proton acceptor?
a)
Arrhenius
b)
Bronsted-Lowry
c)
Lewis
111.
Which reactant in the following equation is a Bronsted acid?
a)
ammonium
b)
ammonia
c)
hydroxide
d)
water
112.
Which reactant in the following equation is a Bronsted acid?
a)
Water
b)
Hydrogen chloride
c)
Hydronium
d)
Chloride
113.
What might happen if you mixed a strong acid with an equally strong base?
a)
You would see an explosive chemical reaction.
b)
The acid would destroy the base.
c)
The base would destroy the acid.
d)
You'd wind up with a pH-neutral substance.
114.
What is the conjugate acid in the following equation?
a)
PO43- 
b)
HNO3 
c)
NO3- 
d)
HPO42-
115.
What is the conjugate base in the following reaction?
a)
HCO3- 
b)
HCl
c)
 H2CO3 
d)
Cl-
116.
HSO4-(aq)+H2O(l)      →       H3O+(aq)+SO42-(aq)
Identify the Acid in the above reaction.
a)
HSO4-
b)
H2O
c)
H3O+
d)
SO42-
117.
CO32-(aq)+H2O(l)      →              HCO3-(aq)+OH-(aq)
Using the above reaction, which compound is the conjugate base?
a)
CO32-
b)
H2O
c)
HCO3-
d)
OH-
118.
A compound that donates H+ ions is 
a)
A Bronsted-Lowry Acid
b)
An Arrhenius Acid
c)
A Bronsted-Lowry Base
d)
An Arrhenius Base
119.
A substance that remains when a base has accepted an H+ ion is
a)
An acid
b)
A Base
c)
A Conjugate Acid
d)
A Conjugate Base
120.

In the equation below, what is the Bronsted Lowry acid?

HCl + NH3 --> Cl- + NH4+

a)

HCl

b)

NH3

c)

Cl-

d)

NH4+

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