wayground logo

Free Printable Worksheets

Font size

S
M
L
XL
Worksheets

Calculating pH

Total questions: 132

Worksheet time: 2hrs 41mins

Name
Class
Date
1.

If a solution has a [H+] of 9.3x10-11, what is the pH?

a)

10.0

b)

4.0

c)

3.5

d)

8.2

2.

If a solution has a [OH-] of 2.3x10-4, it must be a(n)...

a)

Acid

b)

Base

c)

Neutral

3.
If the pH of a solution is 5.6 the pOH is
a)
6.5
b)
12.4
c)
8.4
d)
5.6
4.
A  pH and a pOH will add up to:
a)
0
b)
7
c)
14
d)
1.0 x 10-14
5.

If a solution has a [H+] of 9.3x10-11, what is the pH?

a)

10.0

b)

4.0

c)

3.5

d)

8.2

6.

If a solution has a [OH-] of 2.3x10-4, it must be a(n)...

a)

Acid

b)

Base

c)

Neutral

7.
If the pH of a solution is 5.6 the pOH is
a)
6.5
b)
12.4
c)
8.4
d)
5.6
8.
A  pH and a pOH will add up to:
a)
0
b)
7
c)
14
d)
1.0 x 10-14
9.
If the [OH-] of a solution is 2.7 x 10-4 mol/L the pOH of the solution is
a)
10.44
b)
3.56
c)
1.00
d)
-4.43
10.

What is the equation for calculating pH?

a)

pH = [H+]

b)

pH = log [H+]

c)

pH = -log[OH-]

d)

pH = -log [H+]

11.

If we dissolve 20.0 grams of HCl in 1.2 L of water, what is the pH of that solution?

a)

0.34

b)

4.21

c)

7.20

d)

10.34

12.
If the [H+] of a solution is 6.8 x 10-9 mol/L the pH is
a)
8.17
b)
8.2
c)
9.99
d)
8.62
13.
if the [H+] of a solution is 8.4 x 10-3 mol/L the pOH of the solution will be
a)
2.08
b)
11.92
c)
1.02
d)
12.98
14.

The Kw at room temperature (25 degrees C) is equal to 1.0 x 10-14.  It can also be defined as:

a)

the pH and pOH of a solution

b)

the product of the hydronium ion and the hydroxide ion concentrations

c)

-log [hydronium ion]

d)

antilog -pH

15.

If the hydronium ion H3O+ concentration is equal to the hydroxide ion OH- concentration, the solution is a(n)

a)

acid

b)

base

c)

salt

d)

neutral solution

16.

The pH of a solution is 8.43. What is the hydronium ion H3O+ concentration?

a)

3.7 x 10-9 M

b)

2.7 x 10-6 M

c)

1.0 x 10-8.43 M

d)

1.0 x 10-14

17.

The pH of a solution is 8.43. What is the hydroxide ion OH- concentration?

a)

3.7 x 10-9 M

b)

2.7 x 10-6 M

c)

antilog (-pH)

d)

1.0 x 10-14/-pH

18.

How do you enter antilog on your calculator?

a)

push -log

b)

push ln (natural log)

c)

push 10^

d)

push second log

19.

A solution of Ca(OH)2 is 1.0 x 10-5 M. What is the hydronium ion concentration?

a)

1.0 x 10-5 M

b)

1.0 x 10-9 M

c)

5.0 x 10-10 M

d)

2.0 x 10-5 M

20.

What is the hydronium ion concentration of 4.0 M H2SO4?

a)

4.0 M

b)

8.0 M

c)

1.0 x 10-4 M

d)

2.5 x 10-15 M

21.

A solution has 1.0 x 10-8 M hydronium ions. Another solution has 1.0 x 10-3 M hydronium ions. Which solution has a larger number of hydronium ions? Hint this solution is an acid.

a)

1.0 x 10-3 M hydronium ion solution

b)

1.0 x 10-8 M hydronium ion solution

c)

Neither solution is an acid

22.
Limes have a [H3O+] of 1.3 x 10-2 mol/L.  Their pOH is
a)
1.89
b)
12.11
c)
1.03
d)
12.97
23.

Kw = [OH- ][H3O+]

a)

Kw = 14

b)

Kw = 1 x 10-14

c)

Kw = 1 x 1014

d)

Kw = 0

24.

What is the [OH-] if the pH is 4.900?

a)

7.94 x 10-10 M

b)

1.00 x 10-4 M

c)

7.94 x 10-14 M

d)

4.90 x 10-10 M

25.

What is the pH of a solution with a hydrogen ion concentration of 6.2 x 10-5?

a)

5

b)

4.2

c)

1.6

d)

10.9

26.

Hydrogen ion concentration is also written as:

a)

[H2O]

b)

[H3O+]

c)

[OH-]

d)

[H+]

27.

A sample of fruit juice is found to have a hydrogen ion concentration of 2.87 x 10-4. What would the pH be?

a)

1.76

b)

3.54

c)

8.29

d)

13.22

28.

What is the concentration of H+ in a solution with a pH of 3?

a)

1.0 x 10-3

b)

3.0 M

c)

10.3 M

d)

103 M

29.

What is the pH of a solution when [H+] = 7.9 x 10-11?

a)

2.4

b)

10.1

c)

7.5

d)

4.8

30.

Calculate the pH of a solution with a hydrogen ion concentration of 6.5 x 10-9.

a)

8.2

b)

3.4

c)

5.5

d)

9.1

31.

Which of the following is the hydrogen ion concentration of an acid?

a)

9.2 x 10-14

b)

2.4 x 10-7

c)

1.0 x 10-8

d)

5.7 x 10-11

32.

Which of the following is the [H+] concentration of a base?

a)

9.2 x 10-3

b)

8.3 x 10-6

c)

3.4 x 10-9

d)

1.7 x 10-7

33.

A solution with a hydrogen ion concentration of 5.1 x 10-7 will turn litmus paper:

a)

red

b)

blue

c)

green

d)

purple

34.

A solution with a [H+] concentration of 3.6 x 10-13 will turn litmus paper what color?

a)

purple

b)

green

c)

red

d)

blue

35.

If a solution has a [H+] of 9.3x10-11, what is the pH?

a)

10.0

b)

4.0

c)

3.5

d)

8.2

36.

What is the equation for calculating pH?

a)

pH = [H+]

b)

pH = log [H+]

c)

pH = -log[OH-]

d)

pH = -log [H+]

37.
If the [H+] of a solution is 6.8 x 10-9 mol/L the pH is
a)
8.17
b)
8.2
c)
9.99
d)
8.62
38.

If the hydronium ion H3O+ concentration is equal to the hydroxide ion OH- concentration, the solution is a(n)

a)

acid

b)

base

c)

salt

d)

neutral solution

39.
The pH scale is a range from:
a)
1-7
b)
0-14
c)
1-5
d)
1-20
40.
if the [H+] of a solution is 1.0 x 10-2 mol/L the pH is
a)
2
b)
-2
c)
1
d)
12
41.
Ammonia has a pH of 12.  Ammonia is __________.
a)
an acid
b)
a base
c)
an element
d)
a metal
42.
Which of these solutions is an acid?
a)
Dish Soap: pH of 12
b)
Tomato Soup: pH of 4
c)
Baking Soda: pH of 9
d)
Drain Cleaner: pH of 14
43.
What is the pH of a 4.3 x 10-7 M solution of H2CO3?
a)
7
b)
6.4
c)
7.6
d)
4.3
44.
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
45.

If a solution has a [H+] of 9.3x10-11, what is the pH?

a)

10.0

b)

4.0

c)

3.5

d)

8.2

46.

If a solution has a [OH-] of 2.3x10-4, it must be a(n)...

a)

Acid

b)

Base

c)

Neutral

47.
A  pH and a pOH will add up to:
a)
0
b)
7
c)
14
d)
1.0 x 10-14
48.
If the pH of a solution is 5.6 the pOH is
a)
6.5
b)
12.4
c)
8.4
d)
5.6
49.
If the [OH-] of a solution is 2.7 x 10-4 mol/L the pOH of the solution is
a)
10.44
b)
3.56
c)
1.00
d)
-4.43
50.

What is the equation for calculating pH?

a)

pH = [H+]

b)

pH = log [H+]

c)

pH = -log[OH-]

d)

pH = -log [H+]

51.
If the [H+] of a solution is 6.8 x 10-9 mol/L the pH is
a)
8.17
b)
8.2
c)
9.99
d)
8.62
52.
if the [H+] of a solution is 8.4 x 10-3 mol/L the pOH of the solution will be
a)
2.08
b)
11.92
c)
1.02
d)
12.98
53.

If the hydronium ion H3O+ concentration is equal to the hydroxide ion OH- concentration, the solution is a(n)

a)

acid

b)

base

c)

salt

d)

neutral solution

54.

The pH of a solution is 8.43. What is the hydronium ion H3O+ concentration?

a)

3.7 x 10-9 M

b)

2.7 x 10-6 M

c)

1.0 x 10-8.43 M

d)

1.0 x 10-14

55.

The pH of a solution is 8.43. What is the hydroxide ion OH- concentration?

a)

3.7 x 10-9 M

b)

2.7 x 10-6 M

c)

antilog (-pH)

d)

1.0 x 10-14/-pH

56.

What is the hydronium ion concentration of 4.0 M H2SO4?

a)

4.0 M

b)

8.0 M

c)

1.0 x 10-4 M

d)

2.5 x 10-15 M

57.

A solution has 1.0 x 10-8 M hydronium ions. Another solution has 1.0 x 10-3 M hydronium ions. Which solution has a larger number of hydronium ions? Hint this solution is an acid.

a)

1.0 x 10-3 M hydronium ion solution

b)

1.0 x 10-8 M hydronium ion solution

c)

Neither solution is an acid

58.
Limes have a [H3O+] of 1.3 x 10-2 mol/L.  Their pOH is
a)
1.89
b)
12.11
c)
1.03
d)
12.97
59.

What is the [OH-] if the pH is 4.900?

a)

7.94 x 10-10 M

b)

1.00 x 10-4 M

c)

7.94 x 10-14 M

d)

4.90 x 10-10 M

60.

If a solution has a [H+] of 9.3x10-11, what is the pH?

a)

10.0

b)

4.0

c)

3.5

d)

8.2

61.
If the pH of a solution is 5.6 the pOH is
a)
6.5
b)
12.4
c)
8.4
d)
5.6
62.
A  pH and a pOH will add up to:
a)
0
b)
7
c)
14
d)
1.0 x 10-14
63.

What is the equation for calculating pH?

a)

pH = [H+]

b)

pH = log [H+]

c)

pH = -log[OH-]

d)

pH = -log [H+]

64.

If the hydronium ion H3O+ concentration is equal to the hydroxide ion OH- concentration, the solution is a(n)

a)

acid

b)

base

c)

salt

d)

neutral solution

65.

What does pH measure?

a)

the amount of hydrogen (H+) ions

b)

the amount of hydroxide (OH-) ions

c)

amount of water

d)

all of the above

66.

Which of the following is the strongest acid?

a)

1

b)

5

c)

3

d)

8

67.

Which of the following is the strongest base?

a)

4

b)

14

c)

7

d)

15

68.

A pH of 3 is how many times more acidic than a pH of 5?

a)

2

b)

20

c)

10

d)

100

69.
If the pH of a solution is 5 the [H+] is
a)
1.0 x 105  M
b)
1.0 x 109  M
c)
5.0 x 101  M
d)
1.0 x 10-5  M
70.

For a solution, pH + pOH =

a)

7

b)

14

c)

1.0 x 10-14

d)

-log (1.0 x 10 -14)

71.

If the pH of a solution is 4.0, what is the pOH?

a)

4.0

b)

10.0

c)

1.0 x 10 -4

d)

cannot be determined from the information

72.

The pH of a solution is 8.43. What is the [H3O+]concentration?

a)

3.7 x 10 -9

b)

1.0 x 10-8.43

c)

2.7 x 10-6

d)

1.0 x 10-14

73.

If the [H3O+] of a solution is 1 x 10-3 M, the pH is

a)

11

b)

-3

c)

3

d)

1

74.

If the pH of a solution is 8 the [H3O+] is

a)

1.0 x 106 M

b)

8.0 x 101 M

c)

1.0 x 108 M

d)

1.0 x 10-8 M

75.

If the [OH-] of a solution is 2.7 x 10-4 M, the pOH of the solution is

a)

10.44

b)

1.00

c)

3.57

d)

-4.43

76.

If the [H3O+] of a solution is 6.8 x 10-8 M, the pH is

a)

7.17

b)

3.2 x 10-5

c)

7.2

d)

7.62

77.

If the [H3O+] of a solution is 9.3 x 10-3 M, the pOH of the solution will be

a)

2.03

b)

1.02

c)

11.97

d)

12.98

78.

If a solution has a pOH of 3.7 the [OH-] of the solution is

a)

5.0 x 10-11

b)

2.0 x 10-4

c)

10.3

d)

14

79.

Oranges have a [H3O+] of 1.7 x 10-2 M. Their pOH is

a)

1.77

b)

12.23

c)

10.91

d)

3.09

80.

Ammonia has a pOH of 2. Ammonia is a(n) __________.

a)

acid

b)

base

c)

neutral

d)

metal

81.

Find the pH of a solution with [OH-] = 8.41 x 10-4.

a)

3.08

b)

10.92

c)

9.88

d)

11.23

82.

What is the pOH of a solution with [H+] = 1.24 x 10 -2?

a)

1.91

b)

1.61

c)

12.09

d)

12.39

83.

What is the pH of a solution that has a [H+] of 2.5 x 10-5?

a)

4.60

b)

2.5

c)

5.0

d)

7

84.

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

a)

1.0 x 10-10 M

b)

1.0 x 10-14 M

c)

1.0 x 10-4 M

d)

1.0 x 10-7 M

85.

What is the pOH of a solution where the [OH-] is 7.3 x 10-2 M?

a)

-1.14

b)

1.14

c)

2.01

d)

11.99

86.

What is the [OH-] if the [H+] is 1.0 x 10-3M?

a)

1.0 x 10-3 M

b)

1.0 x 10-14 M

c)

6.02 x 10-23 M

d)

1.0 x 10-11 M

87.

What is the [OH-] if the pH is 4.9?

a)

4.9 x 10-10 M

b)

1.0 x 10-4 M

c)

1.25 x 10-5 M

d)

7.94 x 10-10 M

88.

A 1.0 x 10-4 M solution of HNO3 has a [H+] concentration of: (Notice HNO3 has one H+.)

a)

1.0 x 10-14

b)

log 1.0 x 10-4

c)

1.0 x 10-10

d)

1.0 x 10-4

89.

A solution of KOH is 2.5 x 10-5 M. What is the [H+] concentration? (Hint: Find pOH, then pH, then [H+].)

a)

4.60

b)

9.40

c)

3.98 x 10-10

d)

1.0 x 10-4.60

90.

For a solution, pH + pOH =

a)

7

b)

14

c)

1.0 x 10-14

d)

-log (1.0 x 10 -14)

91.

If the pH of a solution is 4.0, what is the pOH?

a)

4.0

b)

10.0

c)

1.0 x 10 -4

d)

cannot be determined from the information

92.

The pH of a solution is 8.43. What is the [H3O+]concentration?

a)

3.7 x 10 -9

b)

1.0 x 10-8.43

c)

2.7 x 10-6

d)

1.0 x 10-14

93.

If the [H3O+] of a solution is 1 x 10-3 M, the pH is

a)

11

b)

-3

c)

3

d)

1

94.

If the pH of a solution is 8 the [H3O+] is

a)

1.0 x 106 M

b)

8.0 x 101 M

c)

1.0 x 108 M

d)

1.0 x 10-8 M

95.

If the [OH-] of a solution is 2.7 x 10-4 M, the pOH of the solution is

a)

10.44

b)

1.00

c)

3.57

d)

-4.43

96.

If the [H3O+] of a solution is 6.8 x 10-8 M, the pH is

a)

7.17

b)

3.2 x 10-5

c)

7.2

d)

7.62

97.

If the [H3O+] of a solution is 9.3 x 10-3 M, the pOH of the solution will be

a)

2.03

b)

1.02

c)

11.97

d)

12.98

98.

If a solution has a pOH of 3.7 the [OH-] of the solution is

a)

5.0 x 10-11

b)

2.0 x 10-4

c)

10.3

d)

14

99.

Oranges have a [H3O+] of 1.7 x 10-2 M. Their pOH is

a)

1.77

b)

12.23

c)

10.91

d)

3.09

100.

Ammonia has a pOH of 2. Ammonia is a(n) __________.

a)

acid

b)

base

c)

neutral

d)

metal

101.

Find the pH of a solution with [OH-] = 8.41 x 10-4.

a)

3.08

b)

10.92

c)

9.88

d)

11.23

102.

What is the pOH of a solution with [H+] = 1.24 x 10 -2?

a)

1.91

b)

1.61

c)

12.09

d)

12.39

103.

What is the pH of a solution that has a [H+] of 2.5 x 10-5?

a)

4.60

b)

2.5

c)

5.0

d)

7

104.

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

a)

1.0 x 10-10 M

b)

1.0 x 10-14 M

c)

1.0 x 10-4 M

d)

1.0 x 10-7 M

105.

What is the pOH of a solution where the [OH-] is 7.3 x 10-2 M?

a)

-1.14

b)

1.14

c)

2.01

d)

11.99

106.

What is the [OH-] if the [H+] is 1.0 x 10-3M?

a)

1.0 x 10-3 M

b)

1.0 x 10-14 M

c)

6.02 x 10-23 M

d)

1.0 x 10-11 M

107.

What is the [OH-] if the pH is 4.9?

a)

4.9 x 10-10 M

b)

1.0 x 10-4 M

c)

1.25 x 10-5 M

d)

7.94 x 10-10 M

108.

A 1.0 x 10-4 M solution of HNO3 has a [H+] concentration of: (Notice HNO3 has one H+.)

a)

1.0 x 10-14

b)

log 1.0 x 10-4

c)

1.0 x 10-10

d)

1.0 x 10-4

109.

A solution of KOH is 2.5 x 10-5 M. What is the [H+] concentration? (Hint: Find pOH, then pH, then [H+].)

a)

4.60

b)

9.40

c)

3.98 x 10-10

d)

1.0 x 10-4.60

110.

For a solution, pH + pOH =

a)

7

b)

14

c)

1.0 x 10-14

d)

-log (1.0 x 10 -14)

111.

For a solution, pH + pOH =

a)

7

b)

14

c)

1.0 x 10-14

d)

-log (1.0 x 10 -14)

112.

What is the equation for calculating pH?

a)

pH = [H+]

b)

pH = log [H+]

c)

pH = -log[OH-]

d)

pH = -log [H+]

113.

For a solution at 25oC, pH + pOH =

a)

7

b)

14

c)

1.0 x 10-14

d)

-log (1.0 x 10 -14)

114.

If the pH of a solution is 4.0, what is the pOH?

a)

4.0

b)

10.0

c)

1.0 x 10 -4

d)

cannot be determined from the information

115.

If the [H3O+] of a solution is 1 x 10-3 M, the pH is

a)

11

b)

-3

c)

3

d)

1

116.

If the pH of a solution is 8 the [H3O+] is

a)

1.0 x 106 M

b)

8.0 x 101 M

c)

1.0 x 108 M

d)

1.0 x 10-8 M

117.

When the hydrogen ion concentration goes up, the pH ___

a)

gets lower

b)

stays the same

c)

gets higher

d)

goes toward 7

118.

If the [OH-] of a solution is 2.7 x 10-4 M, the pOH of the solution is

a)

10.44

b)

1.00

c)

3.57

d)

-4.43

119.

The pH of a solution is 8.43. What is the [H3O+] concentration?

a)

3.7 x 10 -9

b)

1.0 x 10-8.43

c)

2.7 x 10-6

d)

1.0 x 10-14

120.

What is the numerical value of Kw, the water dissociation constant?

a)

14.0 x 10-1

b)

7.0 x 10-2

c)

2.0 x 10-7

d)

1.0 x 10-14

121.

If a solution has a pOH of 1 what is the pH? Is it an acid or base? (pick 2)

a)

acid

b)

base

c)

13

d)

1

e)

neutral

122.

If the [H3O+] of a solution is 6.8 x 10-8 M, the pH is

a)

7.17

b)

3.2 x 10-5

c)

7.2

d)

7.62

123.

If the [H3O+] of a solution is 9.3 x 10-3 M, the pOH of the solution will be

a)

2.03

b)

1.02

c)

11.97

d)

12.98

124.

When a water molecule loses a hydrogen ion, or proton, it becomes ___

a)

a hydronium ion, H3O+

b)

a hydroxide ion, OH-

c)

a hydronium ion, OH-

d)

a hydroxide ion, H3O+

125.

If a solution has a pH of 1 what is the pOH? Is it an acid or base? (pick 2)

a)

acid

b)

base

c)

13

d)

15

e)

neutral

126.

If a solution has a pOH of 3.7, the [OH-] of the solution is

a)

5.0 x 10-11

b)

2.0 x 10-4

c)

10.3

d)

14

127.

When a hydrogen ion, or proton, attaches to a water molecule it forms ___

a)

a hydronium ion, H3O+

b)

a hydroxide ion, OH-

c)

a hydronium ion, OH-

d)

a hydroxide ion, H3O+

128.

Oranges have a [H3O+] of 1.7 x 10-2 M. Their pOH is

a)

1.77

b)

12.23

c)

10.91

d)

3.09

129.

Find the pH of a solution with [OH-] = 8.41 x 10-4.

a)

3.08

b)

10.92

c)

9.88

d)

11.23

130.

What is the pOH of a solution where the [OH-] is 7.3 x 10-2 M?

a)

-1.14

b)

1.14

c)

2.01

d)

11.99

131.

A solution of KOH is 2.5 x 10-5 M. What is the [H+] concentration? (Hint: Find pOH, then pH, then [H+].)

a)

4.60

b)

9.40

c)

3.98 x 10-10

d)

1.0 x 10-4.60

132.
If the pH of a solution is 5.6 the pOH is
a)
6.5
b)
12.4
c)
8.4
d)
5.6

Similar Resources on Wayground

Ions and isotopes

132 questions

Ions and isotopes

quiz

Worksheet

•

10th - 12th Grade

PS Final Exam Review

131 questions

PS Final Exam Review

quiz

Worksheet

•

10th Grade

CCR Chem A Final Review (Units 1-5)

128 questions

CCR Chem A Final Review (Units 1-5)

quiz

Worksheet

•

9th - 12th Grade

IGCSE Chemistry Revision

137 questions

IGCSE Chemistry Revision

quiz

Worksheet

•

10th - 11th Grade

Unit Review: Thermochemistry

127 questions

Unit Review: Thermochemistry

quiz

Worksheet

•

9th - 12th Grade

2.4 Chemistry NCEA

135 questions

2.4 Chemistry NCEA

quiz

Worksheet

•

11th - 12th Grade

Atomic Radius, Ionization Energy, & Electronegativity

127 questions

Atomic Radius, Ionization Energy, & Electronegativity

quiz

Worksheet

•

12th Grade

Semester 2 FINAL

132 questions

Semester 2 FINAL

quiz

Worksheet

•

10th Grade