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Worksheets

pH and pOH

Total questions: 160

Worksheet time: 8hrs 0mins

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.
A  pH and a pOH will add up to:
a)
0
b)
7
c)
14
d)
1.0 x 10-14
4.
If the pH of a solution is 5.6 the pOH is
a)
6.5
b)
12.4
c)
8.4
d)
5.6
5.
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
6.

What is the equation for calculating pH?

a)

pH = [H+]

b)

pH = log [H+]

c)

pH = -log[OH-]

d)

pH = -log [H+]

7.
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
8.
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
9.

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

10.

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

11.

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

12.

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

13.

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

14.
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
15.

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

16.

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

17.

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

a)

Acid

b)

Base

c)

Neutral

18.
A  pH and a pOH will add up to:
a)
0
b)
7
c)
14
d)
1.0 x 10-14
19.
If the pH of a solution is 5.6 the pOH is
a)
6.5
b)
12.4
c)
8.4
d)
5.6
20.
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
21.

What is the equation for calculating pH?

a)

pH = [H+]

b)

pH = log [H+]

c)

pH = -log[OH-]

d)

pH = -log [H+]

22.
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
23.
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
24.

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

25.

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

26.

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

27.

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

28.

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

29.
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
30.

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

31.

For a solution at 25oC, pH + pOH =

a)

7

b)

14

c)

1.0 x 10-14

d)

-log (1.0 x 10 -14)

32.

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

33.

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

a)

11

b)

-3

c)

3

d)

1

34.

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

35.

When the hydrogen ion concentration goes up, the pH ___

a)

gets lower

b)

stays the same

c)

gets higher

d)

goes toward 7

36.

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

37.

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

38.

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

39.

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

40.

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

41.

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

42.

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+

43.

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

44.

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

45.

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+

46.

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

47.

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

48.

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

49.

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

50.
If the pH of a solution is 5.6 the pOH is
a)
6.5
b)
12.4
c)
8.4
d)
5.6
51.

Acids have a ______ pH and a _________ pOH

a)

low, high

b)

high, low

c)

An acid will not have a pOH

52.
The pH scale is a range from:
a)
1-7
b)
0-14
c)
1-5
d)
1-20
53.
If the pH of a solution is 7 the solution is said to be
a)
Acidic
b)
Basic
c)
Neutral
d)
Tasty
54.

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

55.

Ammonia has a pOH of 2. Ammonia is __________.

a)

an acid

b)

a base

c)

an element

d)

a metal

56.

An acid

a)

is a substance that releases H+ ions when dissolved in water

b)

is a substance that does not release any ions when dissolved in water

c)

is a substance that releases OH- when dissolved in water

d)

releases an equal amount of OH- and H+ ions when dissolved in water

57.

The picture below shows the relative concentrations of H+ and OH- in a solution. Is the solution an acid or a base?

a)

acid

b)

base

58.
When dissolved in water, bases produce:
a)
acids
b)
salts
c)
hydrogen ions
d)
hydroxide ions
59.
A  pH and a pOH will add up to:
a)
0
b)
7
c)
14
d)
1.0 x 10-14
60.

Water has a neutral because

a)

it has more H+ ions than OH-

b)

it has more OH- ions than H+

c)

it does not produce any ions

d)

it has an equal amount of H+ and OH- in solution

61.
A solution has a pH of 7.0.  What would happen to the pH if H ions were added?
a)
pH would go up
b)
pH would go down
c)
pH would stay the same
d)
None of these
62.

A solution has a pH of 7.0. What would happen to the pH if OH- ions were added?

a)

pH would go up

b)

pH would go down

c)

pH would stay the same

d)

None of these

63.

If the [H+] of a solution is 1 x 10-2 M the pH is

a)

2

b)

12

c)

-2

d)

1

64.
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
65.
If the pH of a solution is 5.6 the pOH is
a)
6.5
b)
12.4
c)
8.4
d)
5.6
66.

If the [H3O+] of a solution is 1 x 10-8 M the [OH-] is

a)

1.0 x 10-6 M

b)

1.0 x 106 M

c)

1.0 x 10-8 M

d)

1.0 x 108 M

67.
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
68.
if a solution has a pOH of 5.2 the [OH-] of the solution is
a)
6 x 10 -6 M
b)
6.3 x 10 -6 M
c)
1.58 x 10-5 M
d)
2 x 10-5 M
69.
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
70.
A solution with a [H+] of 9.4 x 10-5 mol/L is said to be
a)
Acidic
b)
Basic
c)
Neutral
d)
negative number, no solution.
71.
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
72.

Find the pH of a 0.000841 M solution of sodium hydroxide

a)

3.07

b)

9.88

c)

10.92

d)

11.23

73.

What is the pOH of a 0.0124 M HCl solution?

a)

1.91

b)

12.09

c)

1.61

d)

12.39

74.

Find the pH of a solution that contains 4.17 g of H2SO4 dissolved in 1.75 liters of solution.

a)

1.31

b)

2.29

c)

3.45

d)

2.02

75.

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

76.

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

a)

Acid

b)

Base

c)

Neutral

77.
A  pH and a pOH will add up to:
a)
0
b)
7
c)
14
d)
1.0 x 10-14
78.
If the pH of a solution is 5.6 the pOH is
a)
6.5
b)
12.4
c)
8.4
d)
5.6
79.
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
80.

What is the equation for calculating pH?

a)

pH = [H+]

b)

pH = log [H+]

c)

pH = -log[OH-]

d)

pH = -log [H+]

81.
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
82.
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
83.

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

84.

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

85.

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

86.

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

87.

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

88.
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
89.

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

90.
If the [H+] of a solution is 1 x 10-2 mol/L the pH is
a)
2
b)
12
c)
-2
d)
1
91.
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
92.
If the pH of a solution is 5.6 the pOH is
a)
6.5
b)
12.4
c)
8.4
d)
5.6
93.
A  pH and a pOH will add up to:
a)
0
b)
7
c)
14
d)
1.0 x 10-14
94.
If the [H3O+] of a solution is 1 x 10-8 mol/L the [OH-] is
a)
1.0 x 10-6
b)
1.0 x 106
c)
1.0 x 10-8
d)
1.0 x 108
95.
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
96.
A solution with a [H+] of 9.4 x 10-5 mol/L is said to be
a)
Acidic
b)
Basic
c)
Neutral
d)
negative number, no solution.
97.
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
98.
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
99.
if a solution has a pOH of 5.2 the [OH-] of the solution is
a)
6 x 10 -6 M
b)
6.3 x 10 -6 M
c)
1.58 x 10-5 M
d)
2 x 10-5 M
100.
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
101.

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

102.

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

a)

acid

b)

base

c)

neutral

d)

metal

103.

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

104.

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

105.

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

106.

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

107.

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

108.

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

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.

Acids have a ______ pH and a _________ pOH

a)

low, high

b)

high, low

c)

An acid will not have a pOH

111.

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

112.

Which of the following pH values represents a basic pH?

a)

1

b)

5

c)

7

d)

9

e)

11

113.

Which of the following answer choices represents an acidic pH?

a)

1

b)

5

c)

7

d)

9

e)

11

114.

Which of the following pH values represents a neutral pH?

a)

1

b)

5

c)

7

d)

9

e)

11

115.

Which of the following pOH values represents an acidic pOH?

a)

1

b)

5

c)

7

d)

9

e)

11

116.

Which of the following pOH values represents a basic pOH?

a)

1

b)

5

c)

7

d)

9

e)

11

117.

What is the pOH of a neutral solution?

a)

1

b)

5

c)

7

d)

9

e)

11

118.

How are pH and pOH related?

a)

pH+pOH = 14pH+pOH\ =\ 14

b)

pH=pOHpH=pOH

c)

pH−pOH=14pH-pOH=14

d)

pH = 1pOHpH\ =\ \frac{1}{pOH}

119.

If the pH of an acid is 3, then it's pOH will be ...

a)

11

b)

3

c)

14

d)

12

120.

If the pOH of a base is 5, it's pH will be...

a)

2

b)

5

c)

14

d)

9

121.

If the [H+] of a solution is 1 x 10-2 M the pH is

a)

2

b)

12

c)

-2

d)

1

122.
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
123.

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

a)

8

b)

6

c)

7

d)

7.5

124.
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
125.
if a solution has a pOH of 5.2 the [OH-] of the solution is
a)
6 x 10 -6 M
b)
6.3 x 10 -6 M
c)
1.58 x 10-5 M
d)
2 x 10-5 M
126.

What is the pH of a solution with a hydrogen ion concentration of 1.0 x 10-8 M?

(HINT...pH = -log [H+] )

a)

-8

b)

6

c)

8

d)

14

127.

What is the pH of a 0.0001 M HCl solution

a)

1

b)

4

c)

7

d)

11

128.

Acids have a ______ pH and a _________ pOH

a)

low, high

b)

high, low

c)

An acid will not have a pOH

129.

Ammonia has a pOH of 2. Ammonia is __________.

a)

an acid

b)

a base

c)

an element

d)

a metal

130.

An acid

a)

is a substance that releases H+ ions when dissolved in water

b)

is a substance that does not release any ions when dissolved in water

c)

is a substance that releases OH- when dissolved in water

d)

releases an equal amount of OH- and H+ ions when dissolved in water

131.

The picture below shows the relative concentrations of H+ and OH- in a solution. Is the solution an acid or a base?

a)

acid

b)

base

132.
When dissolved in water, bases produce:
a)
acids
b)
salts
c)
hydrogen ions
d)
hydroxide ions
133.
A  pH and a pOH will add up to:
a)
0
b)
7
c)
14
d)
1.0 x 10-14
134.

Water is neutral because

a)

it has more H+ ions than OH-

b)

it has more OH- ions than H+

c)

it does not produce any ions

d)

it has an equal amount of H+ and OH- in solution

135.
A solution has a pH of 7.0.  What would happen to the pH if H ions were added?
a)
pH would go up
b)
pH would go down
c)
pH would stay the same
d)
None of these
136.

A solution has a pH of 7.0. What would happen to the pH if OH- ions were added?

a)

pH would go up

b)

pH would go down

c)

pH would stay the same

d)

None of these

137.
If the pH of a solution is 5.6 the pOH is
a)

6.5

b)

12.4

c)

8.4

d)

5.6

138.

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

a)

H+1

b)

OH-1

139.

When the hydrogen ion concentration goes up, the pH ___

a)

gets lower

b)

stays the same

c)

gets higher

d)

goes toward 7

140.

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+

141.

Acids which dissociate almost completely in aqueous solutions are known as:

a)

Dilute acids

b)

Strong acids

c)

Weak acids

d)

Concentrated acids

142.

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

143.

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+

144.

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

145.

Which is a property of a base?

a)

changes litmus from red to blue

b)

reacts with acid to form a salt

c)

feels slippery or soapy

d)

bitter taste

e)

All of the above

146.

A Bronsted Lowry acid:

a)

donates H+ to another substance

b)

accepts H+ from another substance

c)

produces H+

d)

produces OH-

147.

NaOH is:

a)

an Arrhenius base

b)

an Arrhenius acid

c)

neither an acid nor a base

d)

both an acid and a base

148.

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

149.
Acids produce _________ ions when they break down or dissocciate. 
a)
Hydroxide (OH-)
b)
Water
c)
Chlorine (Cl-)
d)
Hydrogen (H+)
150.
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

151.
Bases release ____________ ions when they break down or dissociate. 
a)
Hydrogen (H+)
b)
Hydroxide (OH-)
c)
Chlorine (Cl-)
d)
no
152.
A solution with a [H+] of 9.4 x 10-5 mol/L is said to be
a)

Acidic

b)

Basic

c)

Neutral

d)

negative number, no solution.

153.
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
154.

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

155.

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

156.

If the [H3O+] of a solution is 1 x 10-8 M the [OH-] is

a)

1.0 x 10-6 M

b)

1.0 x 106 M

c)

1.0 x 10-8 M

d)

1.0 x 108 M

157.

Find the pH of a 0.000841 M solution of sodium hydroxide

a)

3.07

b)

9.88

c)

10.92

d)

11.23

158.
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
159.

If the [H+] of a solution is 1 x 10-2 M the pH is

a)

2

b)

12

c)

-2

d)

1

160.

What is the pOH of a 0.0124 M HCl solution?

a)

1.91

b)

12.09

c)

1.61

d)

12.39

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