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WorksheetsAcid/Base Review
Total questions: 42
Worksheet time: 33mins
Name
Class
Date
1.
What is a solution that has an excess of hydroxide (OH-) ions?
a)
pH
b)
acid
c)
neutral
d)
base
2.
Acids are found on the pH scale between which numbers?
a)
0-7
b)
7
c)
7-14
d)
19-42
3.
A solution that is _____ has a pH of 7.
a)
acidic
b)
basic
c)
neutral
d)
none of the above
4.
What is a solution that has an excess of Hydrogen (H+) Ions?
a)
pH
b)
acid
c)
neutral
d)
base
5.
hydrochloric acid
a)
strong acid
b)
weak acid
c)
strong base
d)
weak base
6.
sodium hydroxide
a)
strong acid
b)
weak acid
c)
strong base
d)
weak base
7.
Be(OH)2
a)
strong acid
b)
weak acid
c)
strong base
d)
weak base
8.
H2SO4
a)
strong acid
b)
weak acid
c)
strong base
d)
weak base
9.
HCN
a)
strong acid
b)
weak acid
c)
strong base
d)
weak base
10.
magnesium hydroxide
a)
strong acid
b)
weak acid
c)
strong base
d)
weak base
11.
The [H+] is orange juice is 0.00020 M. FInd the pH of orange juice.
a)
1
b)
3.7
c)
10.3
d)
13
12.
The hydroxide ion is a soft drink is 5.00 x 10-12 M. Find the pH.
a)
0.002
b)
2.7
c)
11.3
d)
14
13.
The pOH of sea water is 5.9. What is its pH?
a)
0.0000000083
b)
0.0000013
c)
5.9
d)
8.1
14.
What is the hydrogen ion concentration in a solution with pOH = 3.3?
a)
10.7 M
b)
0.00050 M
c)
0.000025 M
d)
2.0 x 10-11 M
15.
What is the pH of a 0.13 M solution of H2SO4?
a)
0.13
b)
0.58
c)
0.89
d)
13.4
16.
What is the pH of a solution that has an [H3O+] =1x10-4?
a)
4
b)
-4
c)
2
d)
3
17.
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
18.
The pH of a 0.001 M solution of HCl is
a)
11
b)
3
c)
-3
d)
-11
19.
The pH of a solution at 25ₒC in which [OH-] = 3.9 x 10-5M is:
a)
4.41
b)
3.90
c)
9.59
d)
4.80
20.
Calculate the pH of a 0.47M NH3 (Kb = 1.8 x 10-5) solution.
a)
2.54
b)
8.93
c)
5.07
d)
11.46
21.
Calculate the [H+] in a solution that has a pH of 2.73.
a)
5.4 x 10-12 M
b)
1.9 x 10-3 M
c)
2.7 M
d)
11.3 M
22.
In the Bronsted Lowry theory, an acid is :
a)
a proton donor
b)
a proton acceptor
c)
an H donor
an electron acceptor
an electron acceptor
23.
An acid/base reaction always produces:
a)
H2
b)
H2O
c)
NaCl
d)
H3O+
24.
HNO2 has a Ka = 4.6x10-4 and HOCl has a Ka = 3.5 x10-8. Which is a stronger acid?
a)
HNO2
b)
HOCl
25.
A 1.0 M solution of HC2H3O2 has a pH
a)
= 1
b)
less than 1
c)
greater than 1
d)
=7
26.
Identify [OH−] = 1.0 × 10−6M as being true of acidic or basic solutions at 25◦C and then determine the pH.
a)
basic; pH = 6
b)
acidic; pH = 6
c)
basic; pH = 8
d)
acidic; pH = 8
27.
Calculate the [H+] in a solution which shows a pH of 11.70.
a)
11.7 M
b)
2.0 × 10−12 M
c)
5.0 × 10−3 M
d)
2.3 M
28.
A solution contains 0.00100M HCl. Determine the [OH−].
a)
1.00x10-3M [OH−]
b)
1.00x10-14M [OH−]
c)
1.00x10-7M [OH−]
d)
1.00x10-11M [OH−]
29.
A solution has a
[OH-]=2.4x10-4M.
Does this correspond to a pOH greater than or less than 4? Is the solution acidic or basic?
[OH-]=2.4x10-4M.
Does this correspond to a pOH greater than or less than 4? Is the solution acidic or basic?
a)
pOH < 4; acidic
b)
pOH > 4; acidic
c)
pOH < 4; basic
d)
pOH > 4; acidic
30.
If you add 0.001 moles of HCl to 1 liter of water, the pH of the solution will be
a)
2.0
b)
5.0
c)
3.0
d)
1.0
31.
A sample of pure water is neutral because it contains
a)
some hydronium ions.
b)
equal amounts of hydroxide and hydronium ions.
c)
some hydroxide ions.
d)
only H2O molecules.
32.
This is one way to show a neutral substance:
a)
[H+]=[OH-]
b)
[H+]~~[OH-]
c)
[H+]<[OH-]
d)
[H+]>[OH-]
33.
This indicates an acidic substance:
a)
[H+]<[OH-]
b)
[H+]>[OH-]
c)
[H+]:[OH-]
34.
This indicates a basic substance:
a)
[H+]>[OH-]
b)
[H+]:[OH-]
c)
[H+]<[OH-]
35.
This uses a log function to describe the concentration of OH- ions in solution:
a)
pOH
b)
pH
c)
acid
d)
base
36.
This uses a log function to describe the concentration of hydronium ions in a solution:
a)
pOH
b)
pH
c)
acid
d)
base
37.
What is the ion responsible for acidity in water called?
a)
hydrogen ion
b)
hydronium ion
c)
ionic product
d)
hydroxide ion
38.
If a solution of Ca(OH)2 has a molarity of 0.001, what is the OH- concentration?
a)
10-3
b)
10-6
c)
0.002
d)
10-11
39.
What is the concentration of H3O+ ions in a 0.02M solution of HNO3?
a)
0.02
b)
0.04
c)
10-12
d)
3 x 0.002
40.
What is the concentration of OH- ions in a 0,01M solution of HCl?
a)
0.01
b)
0.02
c)
10-2
d)
10-12
41.
BASE + ACID ----> SALT +?
a)
water
b)
oxygen
c)
hydrogen ion
d)
hydroxide ion
42.
A solution with [H+] = 1.0 x 1013
a)
is acidic
b)
is basic
c)
is neutral
d)
unable to determine
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