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Acids and Bases Review

Total questions: 77

Worksheet time: 1hrs 8mins

Name
Class
Date
1.

Which of the following indicator is most appropriate for determining the equivalence point in the titration of a weak acid with a strong base?

a)

Thymol blue : pH range of color change: 1.2 to 2.8

b)

Methyl orange: pH range of color change: 3.1 to 4.4

c)

Bromocresol blue: pH range of color change: 5.2 to 6.8

d)

m-cresol purple: pH range of color change: 7.6 to 9.2

2.

Which indicator would be effective for detecting the end point of this titration of a strong acid and a weak base.

a)

Methyl orange, with a range of 3.2-4.4

b)

phenolphthalein, with the range of 8.2 -10

c)

bromocresol green, with the range of 3.8-5.4

d)

thymol blue, with the range of 8.0-9.6

e)

Methyl orange, with a range of 3.2-4.4 or bromocresol green, with the range of 3.8-5.4

3.
What kind of acid does not completely dissociate?
a)
weak
b)
strong
c)
ionic
d)
pH
4.
pH is a measure of the ______________ of hydrogen ions
a)
concentration
b)
concatentation
c)
cations
d)
concentric
e)
salutations
5.
Water is ____, meaning it can be both and acid or a base
a)
Amphoteric
b)
Atmospheric
c)
Amphibious
d)
Aqueous
e)
Amplified
6.
Which of the following is an acid?
a)
CO2
b)
KOH
c)
NH3
d)
HBr
7.
Which of the following describes an acid?
a)
turns litmus blue
b)
low pH
c)
bitter
d)
high pH
8.
Solutions that identify an acid or base by a color change.
a)
weak acid
b)
weak base
c)
acidic anhydride
d)
indicator
9.
An acid that ionizes completely in an aqueous solution.
a)
weak acid
b)
weak base
c)
strong base
d)
strong acid
10.
Arrhenius acids begin with hydrogen.
a)
True
b)
False
11.
Which of the following is acid?
a)
pH = 9.1
b)
pOH = 3.11
c)
[H+] = 1.0 x 10-8 M
d)
pOH = 12.5
12.
Which of the following is basic?
a)
[OH-]= 3.44 x 10-2
b)
pH = 1.4
c)
pOH = 12.0
d)
[H+] = 9.8 x 10-3 M
13.

What is "end point" in a titration?

a)

The point where the color of an indicator begins to change

b)

The point where we take our final volume measurement

c)

The middle point on a titration curve

d)

The point where the volume of analyte has reached equilibrium with the volume of titrant

14.

When H2SO4 is titrated by RbOH, what is the pH at equivalence point?

a)

Exactly 7

b)

Below 7

c)

Above 7

d)

Unknown

15.

Which of the following is NOT a reason buffers are important?

a)

Buffers can prevent pH from changing

b)

Buffers can keep your blood pH at a specific level and prevent diseases

c)

Buffers can neutralize both acids and bases

d)

Buffers indicate pH change in titrations

16.

Which is NOT true of the species shown?

a)

It is called amphoteric

b)

It can act as both an acid and a base

c)

It can be used in a buffer

d)

It has a pH of 1

17.

If the pH of a solution is 3.2, what is the pOH of the solution?

a)

3.2

b)

-0.51

c)

10.8

d)

6.8

18.

If the pOH is 2.7, what is the pH?

a)

-0.43

b)

2.7

c)

7.3

d)

11.3

19.

If the concentration of H3O+ of a solution is 7.3 x 10-8, what is the pH?

a)

8

b)

7.1

c)

6.9

d)

14

20.

If the OH- concentration is 2.9 x 10-12, what is the pOH?

a)

12

b)

11.5

c)

2.5

d)

0

21.

If the hydronium ion concentration of a solution is 4.5 x 10-4, what is the pOH of the solution?

a)

3.35

b)

10.65

c)

14

d)

0

22.

If the hydroxide ion concentration of a solution is 1.8 x 10-1, what is the pH of the solution?

a)

0.74

b)

13.26

c)

0

d)

14

23.
According to ___________________, an acid is any substance that has an increased concentration of H+ (H3O+) is an acid. 
a)
Ahrrenius
b)
Bonsted-Lowry
c)
Lewis
d)
Newman-Wright
24.
According to ___________________, an acid is any substance that donates a proton. 
a)
Ahrrenius
b)
Bonsted-Lowry
c)
Lewis
d)
Newman-Wright
25.
According to ___________________, an acid is any substance that accepts a pair of valence electrons to form a covalent molecule. 
a)
Ahrrenius
b)
Bonsted-Lowry
c)
Lewis
d)
Newman-Wright
26.
According to ___________________, a base is any substance with an increased concentration of OH- ions. 
a)
Ahrrenius
b)
Bonsted-Lowry
c)
Lewis
d)
Newman-Wright
27.
According to ___________________, a base is any substance that accepts a proton. 
a)
Ahrrenius
b)
Bonsted-Lowry
c)
Lewis
d)
Newman-Wright
28.
According to ___________________, a base is any substance that donates a pair of valence electrons to form a covalent bond. 
a)
Ahrrenius
b)
Bonsted-Lowry
c)
Lewis
d)
Newman-Wright
29.
When you combine H+ and OH-, you get what molecule? 
a)
H2O
b)
H2O2
c)
OHH
d)
HHO
30.
A ________________ acid ionizes (dissociates) completely. 
a)
Strong
b)
Weak
c)
Medium
d)
Moderate
31.
A ________________ base ionizes (dissociates) completely. 
a)
Strong
b)
Weak
c)
Medium
d)
Moderate
32.
A ________________ base does not ionize (dissociate) completely, therefore it has a low concentration of OH- ions. 
a)
Strong
b)
Weak
c)
Medium
d)
Moderate
33.
A ______________ acid can only donate one proton. 
a)
Monoprotic
b)
Polyprotic 
c)
Diprotic
d)
Triprotic 
34.
A ______________ acid can donate 2 protons.
a)
Monoprotic
b)
Polyprotic 
c)
Diprotic
d)
Triprotic 
35.
A ______________ acid can donate 3 protons.
a)
Monoprotic
b)
Polyprotic 
c)
Diprotic
d)
Triprotic 
36.
A ______________ acid can donate more than one proton. 
a)
Monoprotic
b)
Polyprotic 
c)
Amphoteric
d)
Saturated
37.
The base that is formed when an acid or base is formed in a Bronsted-Lowry acid base reaction is called a? 
a)
Conjugate Acid
b)
Conjugate Base
c)
Base
d)
Acid
38.
A solution that can act as both an acid and a base is called? 
a)
Amphoteric
b)
Metomorphic
c)
Diabolic
d)
Might Morphin
39.
The acid that is formed when an acid or base is formed in a Bronsted-Lowry acid base reaction is called a? 
a)
Conjugate Acid
b)
Conjugate Base
c)
Base
d)
Acid
40.
A reaction in which H+ and OH- cancel each other out is known as a __________________ reaction. 
a)
Neutralization
b)
Combustion
c)
Single Replacement
d)
Synthetic 
41.
The remaining cation and anion from a neutralization reaction form a? 
a)
Salt
b)
Acid
c)
Base
d)
Pepper
42.
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
43.
The combined pH and pOH must equal: 
a)
14
b)
7
c)
10
d)
9
44.
To find the pH of a solution you take the _______________ of the H3O+ concentration. 
a)
-log
b)
log
c)
cos
d)
tan
45.
To find the pOH of a solution you take the _______________ of the OH- concentration. 
a)
-log
b)
log
c)
cos
d)
tan
46.
A _______________ is a substance changes color in the presence of an acid or base. 
a)
Amphoteric Solution
b)
Indicator Solution
c)
Inidcated Solution
d)
Super Saturated Solution 
47.
The point in which H+ and OH- are equal during the titration process is called? 
a)
End point
b)
Equivalence point
c)
Saturation point
d)
Unsaturation point
48.
The point in which an acid switches to a base or a base switches to an acid during titration is called the? 
a)
End point
b)
Equivalence point
c)
Saturation point
d)
Unsaturation point
49.
Which is not a strong acid?
a)
HF
b)
HI
c)
HCl
d)
HBr
50.
Which is not a strong base?
a)
LiOH
b)
NaOH
c)
NH4OH
d)
RbOH
51.
What does amphoteric mean?
a)
Acts as an amphibian does
b)
Acts as an acid most of the time
c)
Acts as a base most of the time
d)
Can acts as both an acid and a base
52.
Identify the conjugate acid-base pair.
a)
NH3 & NH4+
b)
NH3 & H2O
c)
NH4+ & OH-
d)
none of these
53.
Which molecule is donating the H+ ion?
a)
NH3
b)
OH-
c)
NH2-
d)
H2O
54.
Identify the molecule accepting the H+ ion?
a)
H2SO4
b)
H2O
c)
H3O+
d)
HSO4-
55.
Which molecule is amphoteric?
a)
H2O
b)
H3O+
c)
OH-
56.
Identify the reaction type:
KOH + H3PO4 --> K3PO4 + H2O
a)
Synthesis
b)
Decomposition
c)
Single replacement
d)
Double replacement
57.
Identify the reaction type:
Ca + AlCl3 --> CaCl2 + Al
a)
Synthesis
b)
Decomposition
c)
Single replacement
d)
Double replacement
58.
Balance this equation
_N2 + _H2 --> _NH3
a)
1,2,3
b)
1,3,2
c)
1,1,2
d)
2,1,1
59.
Balance this equation
_Al +_HCl --> _H2 +_AlCl3
a)
2, 6, 3, 2
b)
it is already balanced
c)
4, 12, 3, 4
d)
2, 1, 4, 5
60.
Balance this equation.
_CF4 + _Br2 -- _CBr4 + _F2
a)
2,1,2,1
b)
1,2,2,1
c)
1,2,1,2
d)
2,2,2,2
61.
HClO3
a)
strong acid
b)
weak acid
c)
strong base
d)
weak base
62.
H2SO4
a)
strong acid
b)
weak acid
c)
strong base
d)
weak base
63.
H2CO3
a)
strong acid
b)
weak acid
c)
strong base
d)
weak base
64.
Be(OH)2
a)
strong acid
b)
weak acid
c)
strong base
d)
weak base
65.
A solution that can act as both an acid and a base is called? 
a)
Amphoteric
b)
Metomorphic
c)
Diabolic
d)
Mighty Morphin
66.
Titration method is used to prepare salts from...
a)
Acid + Metal
b)
Acid + Alkali
c)
Base + Ammonium Salt
d)
Two Aqueous Solutions
67.
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
68.
The pH of a 0.001 M solution of HCl is 
a)
11
b)
3
c)
-3
d)
-11
69.
What is the pH of a solution if [H+] = 6.0 x 10-10 M?
a)
3.45
b)
6.25
c)
9.22
d)
11.34
70.
All bases have this in common
a)
Contain H+ ions
b)
Contain OH- ions
71.
What are the products to a neutralization reaction?
a)
H2 + Ionic Salt
b)
H2O + Ionic Salt
c)
H3O+ + Ionic Salt
d)
OH- + Ionic Salt
72.
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
73.
BASE + ACID ----> SALT +?
a)
water
b)
oxygen
c)
hydrogen ion
d)
hydroxide ion
74.

Which of the following species is amphoteric ?

a)

H+

b)

CO3-

c)

HCO3-

d)

H2CO3

e)

NO3 -

75.

Which of the following is a Bronsted-Lowry acid-base pair?

a)

H+ and Cl-

b)

HCl and NaOH

c)

H2SO4 and SO42-

d)

HCO3- and CO32-

76.

Which of the following is a Bronsted-Lowry acid-base pair?

a)

HClO2 and HNO2

b)

HIO and NO2-

c)

HCN and CLO2-

d)

H2PO4- and HPO42-

77.

Each of the following can act as a Bronsted-Lowry acid and a Bronsted-Lowry base, EXCEPT

a)

HCO3-

b)

H2PO4-

c)

NH4+

d)

H2O

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