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Worksheets

Giant Acid/Base Review

Total questions: 140

Worksheet time: 4hrs 43mins

Name
Class
Date
1.

Organize these options into the right categories.

Categorize the following

sour taste

bitter taste

pH = 8.2

pH = 1.8

turns blue litmus paper red

turns red litmus paper blue

slippery

increase hydroxide ions

increase hydrogen ions

pH = 5.4

Acid
Base
2.

What is pH based on?

a)

The pOH.

b)

The dissociation of water.

c)

The concentration of hydroxide ions.

d)

The formation of water.

3.

What equation will be used to solve the following problem?

What is the pH of solution with [H+] of 3.3 x 10–9 M?

a)

pH = −log⁡[H+]pH\ =\ -\log\left[H^+\right]

b)

pOH = −log⁡[OH−]pOH\ =\ -\log\left[OH^-\right]

c)

[H+]=10−pH \left[H^+\right]=10^{-pH}\

d)

[OH−]=10−pOH \left[OH^-\right]=10^{-pOH}\

e)

pH + pOH =14pH\ +\ pOH\ =14

4.

What is the pH of solution with [H+] of 3.3 x 10–9 M?

5.

What equation will be used to solve the following problem?

What is the [H+] for a solution with a pH of 12.05?

a)

pH = −log⁡[H+]pH\ =\ -\log\left[H^+\right]

b)

pOH = −log⁡[OH−]pOH\ =\ -\log\left[OH^-\right]

c)

[H+]=10−pH \left[H^+\right]=10^{-pH}\

d)

[OH−]=10−pOH \left[OH^-\right]=10^{-pOH}\

e)

pH + pOH =14pH\ +\ pOH\ =14

6.

What is the [H+] for a solution with a pH of 12.05?

7.

What equation will be used to solve the following problem?

What is the pOH of solution with [OH–] = 0.003 M?

a)

pH = −log⁡[H+]pH\ =\ -\log\left[H^+\right]

b)

pOH = −log⁡[OH−]pOH\ =\ -\log\left[OH^-\right]

c)

[H+]=10−pH \left[H^+\right]=10^{-pH}\

d)

[OH−]=10−pOH \left[OH^-\right]=10^{-pOH}\

e)

pH + pOH =14pH\ +\ pOH\ =14

8.

What is the pOH of solution with [OH–] = 0.003 M?

9.

What equation will be used to solve the following problem?

What is the [OH–] of a solution with a pOH of 4.90?

a)

pH = −log⁡[H+]pH\ =\ -\log\left[H^+\right]

b)

pOH = −log⁡[OH−]pOH\ =\ -\log\left[OH^-\right]

c)

[H+]=10−pH \left[H^+\right]=10^{-pH}\

d)

[OH−]=10−pOH \left[OH^-\right]=10^{-pOH}\

e)

pH + pOH =14pH\ +\ pOH\ =14

10.

What is the [OH–] of a solution with a pOH of 4.90?

11.

What equation will be used to solve the following problem?

What is the pH of a sodium hydroxide solution with a pOH of 2.11?

a)

pH = −log⁡[H+]pH\ =\ -\log\left[H^+\right]

b)

pOH = −log⁡[OH−]pOH\ =\ -\log\left[OH^-\right]

c)

[H+]=10−pH \left[H^+\right]=10^{-pH}\

d)

[OH−]=10−pOH \left[OH^-\right]=10^{-pOH}\

e)

pH + pOH =14pH\ +\ pOH\ =14

12.

What is the pH of a sodium hydroxide solution with a pOH of 2.11?

13.

What equation will be used to solve the following problem?

What is the pOH of a solution of a hydrochloric acid with a concentration of 0.0371 M?

(Hint: What does HCl produce when placed in water?)

a)

pH = −log⁡[H+]pH\ =\ -\log\left[H^+\right]

b)

pOH = −log⁡[OH−]pOH\ =\ -\log\left[OH^-\right]

c)

[H+]=10−pH \left[H^+\right]=10^{-pH}\

d)

[OH−]=10−pOH \left[OH^-\right]=10^{-pOH}\

e)

pH + pOH =14pH\ +\ pOH\ =14

14.

What is the pOH of a solution of a hydrochloric acid with a concentration of 0.0371 M?

15.

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

16.

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

a)

Acid

b)

Base

c)

Neutral

17.
A  pH and a pOH will add up to:
a)
0
b)
7
c)
14
d)
1.0 x 10-14
18.
If the pH of a solution is 5.6 the pOH is
a)
6.5
b)
12.4
c)
8.4
d)
5.6
19.
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
20.

What is the equation for calculating pH?

a)

pH = [H+]

b)

pH = log [H+]

c)

pH = -log[OH-]

d)

pH = -log [H+]

21.
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
22.
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
23.

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

24.

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

25.

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

26.

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

27.

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

28.
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
29.

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

30.

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

31.

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

a)

Acid

b)

Base

c)

Neutral

32.
A  pH and a pOH will add up to:
a)
0
b)
7
c)
14
d)
1.0 x 10-14
33.
If the pH of a solution is 5.6 the pOH is
a)
6.5
b)
12.4
c)
8.4
d)
5.6
34.
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
35.

What is the equation for calculating pH?

a)

pH = [H+]

b)

pH = log [H+]

c)

pH = -log[OH-]

d)

pH = -log [H+]

36.
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
37.
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
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 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

40.

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

41.

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

42.

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

43.
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
44.

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

45.

What is the pH of a solution that has a [H+] concentration of 1x10-4 ?

a)

10

b)

4

c)

.0001

d)

7

e)

[10-4]

46.

What is the pH of a solution that has a [OH-] of 1 x 10-5 ?

a)

9

b)

5

c)

.00005

d)

2.5

47.

What is the pH of a solution of KOH that has a Molarity of .00034?

a)

3

b)

3.4

c)

11

d)

10.53

48.
What does pH measure?
a)
Amount of Oxygen Ions
b)
Amount of Hydrogen Ions
c)
The amount of salt in a solution
d)
The density
49.
The following neutralization reaction occurs in the classroom.
HCl  +  KOH  -->  H2O  +  KCl
If a student uses 25.0 mL of a 0.5M solution of KOH, what is the molarity of the acid if 15.0mL of acid neutralized?
a)
0.8M
b)
1.2M
c)
12.5M
50.
Human blood has a pH between 7.35 and 7.45. Which of the following best describes human blood?
a)
strongly acidic
b)
slightly acidic
c)
strongly basic
d)
slightly basic
51.
I am titrating 1M HCl with 1M NaOH.  I have 25mL of HCl. How much NaOH will I need?
a)
2.5mL
b)
5mL
c)
25mL
d)
50mL
52.
How many moles of Ca(OH)2 are needed to neutralize three moles of HCl? 
a)
8
b)
1.5
c)
6
d)
3
53.
What is the [OH-] if the [H+] is 1.0 x 10-3M?
a)
1.0 x 10-3 M
b)
6.02 x 10-23 M
c)
1.0 x 10-14 M
d)
1.0 x 10-11 M
54.
What is the pOH of a solution that has a pH of 2?
a)
10
b)
12
c)
14
d)
1
55.
What is the [OH-] if the pH is 4.9?
a)
7.94 x 10-10 M
b)
1.0 x 10-4  M
c)
7.94 x 10-14 M
d)
4.9 x 10-10 M
56.

Which is the correct equation for calculating pH?

a)

pH = log[H+]

b)

pH = -log[H+]

c)

pH = 10-[H+]

d)

pH = In[H+]

57.
A solution with a pH of 3.6 would be...
a)
Acid
b)
Base
c)
Neutral
d)
Acid and Base
58.

In the reaction below, H2O is a(n):

H2SO3 + H2O --> H3O+ + HSO3-

a)

base

b)

acid

c)

conjugate acid

d)

conjugate base

59.
HSO4- + H2O → H3O++ SO42-
Identify the Acid in the above reaction.
a)
HSO4-
b)
H2O
c)
H3O+
d)
SO42-
60.
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-
61.

A solution of HCl has a [H+] = 7.2 x 10-9. Is this and acid or a base?

a)

Acid

b)

Base

62.

KOH has a pOH of 3.0, what is the [OH-]?

a)

0.01 M

b)

0.001 M

c)

0.0001 M

d)

0.1 M

63.

Which of the following is most acidic?

a)

H2CrO4

b)

Cr(OH)3

c)

Cr(OH)2

d)

Cr

64.

What is the concentration of hydronium, H3O+ ions in pure water?

a)

1.0 x 10–7 M

b)

Kw/[OH–]

c)

the same as [OH–

d)

All of the above

65.

As the [H3O+] of a solution increases, the value of

a)

log [H3O+] increases.

b)

–log [H3O+] decreases

c)

the solution’s pH decreases

d)

All of the above

66.

Which of the following is not a property of an acidic solution?

a)

[H3O+] greater than 1 x 10–7 M

b)

pH value below 7

c)

[OH–] greater than 1 x 10–7 M

d)

pOH value greater than 7

67.

A basic solution

a)

has a higher concentration of hydronium ions than hydroxide ions.

b)

has the same concentration of hydronium and hydroxide ions.

c)

has a lower concentration of hydronium ions than hydroxide ions.

d)

does not have hydronium ions.

68.

If the pH of a solution increases from 2.0 to 4.0, the H3O+ ion concentration

a)

decreases by a factor of 2.

b)

increases by a factor of 3

c)

decreases by a factor of 100.

d)

increases by a factor of 1000.

69.
According to the Arrhenius theory, acids increase the concentration of what in water?
a)
H+ ions
b)
hydrate ions
c)
hydroxide ions
d)
OH- ions
70.

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

71.
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
72.

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

a)

11

b)

-3

c)

3

d)

1

73.

​ (a)   react with metals. ​ (b)   are blue in bromothymol blue.​ A solution with a pH ​ (c)   will be yellow in bromothymol blue. A solution with a pH ​ (d)   will be pink in phenolphthalein.

Choose from the below words
Acids
Bases
below 7
above 8
74.

Identify the ion.

a)

Hydrogen

1.

H+

b)

Hydroxide

2.

OH-

c)

Hydronium

3.

H3O+

75.

Match the correct term with its definition

a)
Arrhenius Acid
1.

Produce H+ as the only positive ion

b)
Arrhenius Base
2.

Produce Oh- as the only negative ion

c)
Bronsted-Lowry Acid
3.

Proton donor

d)
Bronsted-Lowry Base
4.

Proton Acceptor

e)

Electrolyte

5.

Conducts electricity when dissolved

76.

Match the following

a)

H2SO3

1.

Sulfurous Acid

b)

NH3

2.

Ammonia

c)

HNO3

3.

Nitric Acid

d)

H2SO4

4.

Sulfuric Acid

e)

HClO

5.

Hypochlorous Acid

77.

A company produces a colorless vinegar that is 5.0% CH3COOH in water. Using thymol blue as an indicator, a student titrates a 15.0-milliliter sample of the vinegar with 43.1 milliliters of a 0.30 M NaOH(aq) solution until the acid is neutralized.

Determine the molarity of the CH3COOH in the vinegar sample, using the titration data. Round using significant figures.

78.

In a neutralization reaction...

potassium hydroxide reacts with hydrochloric acid to form ​water and potassium chloride

Write this reaction using the formulas:

1​ (a)   + 1​ (b)   → 1​ (c)   + ​ 1 (d)  

Choose from the below words
KOH
HCl
H2O
KCl
CO2
KH
HClO
79.

During a titration, 10.00 mL of acetic acid, HC2H3O2(aq), is completely neutralized by adding 12.50 mL of 0.64 M sodium hydroxide, NaOH(aq).

Determine the molarity of the acetic acid.

80.

30mL of NaOH is neutralized by 12.3mL of 0.2M HCl. What is the concentration of the NaOH.

a)

82 mol/l

b)

0.82 mol/l

c)

0.49 mol/l

d)

0.082 mol/l

81.

The reaction of perchloric acid (HClO4) with lithium hydroxide (KOH) is described by the equation

HClO4 + KOH → KClO4 + H2O

Suppose 100 mL of perchloric acid is neutralized by exactly 50.0 mL of 1.0 M of Potassium hydroxide. What is the concentration of the perchloric acid?

a)

0.5M

b)

50M

c)

2.0M

d)

1.0M

82.
What is the molarity of a NaOH solution if 11.6 mL of 3 M HCl was used to neutralize 25 mL of NaOH?
a)
1.392 M
b)
0.155 M
c)
0.718 M
83.

A titration works by using a ___________________________ reaction.

a)

Single Replacement

b)

Neutralization

c)

Combustion

d)

Synthesis

84.

If it takes 25 mL of 0.05 M HCl to neutralize 345 mL of NaOH solution, what is the concentration of the NaOH solution?

a)

0.0036 M NaOH

b)

0.00125 M NaOH

c)

3.62 M NaOH

d)

1.25 M NaOH

85.

Which of the following is the best definition of titration?

a)

An experimental way to determine the concentration of an unknown acid or a base

b)

An experimental way to create an effective buffered solution

c)

An experimental way of determining the type of salt that will be produced from a neutralization reaction

d)

An experimental way to determine whether an acid or base is strong or weak

86.

A titration curve is given below.

Which of the following statements is FALSE about this titration?

a)

The acid and base are neutralized at 50 mL

b)

Neutral salt is produced.

c)

A base is neutralized by an acid

d)

The indicator chosen should change color at pH 6-8

87.

What is the volume at the equivalence point.

a)

50 mL

b)

100 mL

c)

10 mL

d)

200 mL

88.

Label the parts of this titration curve

a)Equivalence Point
b)Base > Acid
c)Acid > Base
1
2
3
1)
2)
3)
89.

A 5.00 mL sample of household ammonia was analyzed by titration with hydrochloric acid according to the following reaction:   HCl  +  NH3  →  NH4 +   +  Cl −HCl\ \ +\ \ NH_3\ \ \rightarrow\ \ NH_4^{\ +}\ \ \ +\ \ Cl^{\ -}  
This titration required 19.5 mL of 0.750 M HCl. What is the molarity of the ammonia sample? 

a)

1.97 M

b)

2.19 M

c)

2.44 M

d)

2.92 M

90.

Which point on the titration curve corresponds to the point at which the moles of the added strong base are equal to the moles of the weak acid initially present?

a)

Q

b)

R

c)

S

d)

T

91.

At point P in the titration, which of the following species has the highest concentration?

a)

HA

b)

A–

c)

H3O+

d)

OH–

92.
what is the reading on this burette?
a)
4.40mL
b)
3.50mL
c)
3.60mL
d)
4.50mL
93.
What do acids do to red litmus paper?
a)
Turn it Red 
b)
Turn it Blue
c)
Turn it Yellow
d)
Turn it Green
94.
What do bases do to red litmus paper?
a)
Turn it Red 
b)
Turn it Blue
c)
Turn it Yellow
d)
Turn it Green
95.
Which food is the most acidic?
a)
bananas
b)
lemon juice
c)
orange juice
d)
fish
96.

Based on the results of testing colorless solutions with indicators, which solution is most acidic?

a)

solution where bromthymol blue is blue

b)

solution where bromcresol green is blue

c)

solution where phenolphthalein is pink

d)

solution where methyl orange is red

97.

In which solution will thymol blue indicator appear blue?

a)

0.1 M CH3COOH

b)

0.1 M KOH

c)

0.1 M HCl

d)

0.1 M H2SO4

98.

Three samples of the same solution are tested, each with a different indicator. All three indicators, bromthymol blue, thymol blue and bromcresol green appear blue if the pH of the solution is

a)

4.7

b)

6.0

c)

7.8

d)

9.9

99.

Which indicator is blue in a solution that has a pH of 5.6?

a)

bromcresol green

b)

bromthymol blue

c)

thymol blue

d)

methyl orange

100.

Which indicator is yellow in a solution with a pH of 9.8?

a)

methyl orange

b)

bromthymol blue

c)

bromcresol green

d)

thymol blue

101.

In which solution will thymol blue indicator appear blue?

a)

0.1 M CH3COOH

b)

0.1 M KOH

c)

0.1 M HCl

d)

0.1 M H2SO4

102.

According to reference table M, what is the color of the indicator methyl orange in a solution that has a pH of 2?

a)

blue

b)

yellow

c)

orange

d)

red

103.

A compound whose water solution conducts electricity and turns phenolphthalein pink is

a)

HCl

b)

HC2H3O2

c)

NaOH

d)

CH3OH

104.

An aqueous solution turns litmus red. The pH of this solution could be

a)

14

b)

11

c)

8

d)

5

105.

Three samples of the same solution are tested, each with a different indicator. All three indicators, bromthymol blue, thymol blue and bromcresol green appear blue if the pH of the solution is

a)

4.7

b)

6.0

c)

7.8

d)

9.9

106.

The pH of a strong acid would be:

a)

1-2

b)

5-6

c)

8-9

d)

12-13

107.

The pH of a strong base would be:

a)

1-2

b)

5-6

c)

8-9

d)

13-14

108.

Acid-Base indicators can tell the difference between an acid or base based on the change in ___________

a)

Smell

b)

Colour

c)

Taste

d)

Feel

109.

Litmus paper changes colour to ___________ in an acid.

a)

Blue

b)

Green

c)

Yellow

d)

Red

110.

Methyl Orange changes colour to ___________ in an acid.

a)

Green

b)

Blue

c)

Red

d)

Yellow

111.

What is the colour of phenolphthalein an acid?

a)

Pink

b)

Yellow

c)

Orange

d)

Colourless

112.
According to which theory is a base a substance which produces OH- ions in water?
a)
Arrhenius
b)
Bronsted-Lowry
c)
Lewis
113.
What is "neutralization"?
a)
Compound formed by a metal and a nonmetal
b)
The reaction between an acid and a base which produces a salt and water
c)
A chemical whose color changes in the presence of acids and bases
d)
To decrease the amount of solute as compared to the amount of solvent in a solution
114.

What is the [H+] in a solution with a pH of 11?

a)

1 x 10-1 M

b)

1 x 10-2 M

c)

1 x 1011 M

d)

1 x 10-11 M

115.

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

HCl + NH3 --> Cl- + NH4+

a)

HCl

b)

NH3

c)

Cl-

d)

NH4+

116.
The lower the pH, the greater the concentration of :
a)
OH-
b)
H+
117.
According to the pH range which substance is more acidic than lemon juice
a)
Hydrochloric acid
b)
cabbage
c)
milk
118.

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

119.
This piece of pH paper has been dipped into:
a)
An acid
b)
A base
c)
A pH-neutral substance
d)
A buffer
120.

If it takes 54 mL of 0.1 M NaOH to neutralize 125 mL of an HCl solution, what is the concentration of the HCl? (record you answer with the correct unit)

a)

0.043 M

b)

0.034 M

c)

0.065 M

d)

0.77 M

121.

A 25.0 mL sample of HCl was titrated to the endpoint with 15.0 mL of 2.0 M NaOH. What is the molarity of HCl?

a)

1.6 M HCl

b)

0.03 M HCl

c)

0.6 M HCl

d)

1.2 M HCl

122.

Write a balanced chemical equation for the reaction of the following acid and base:

___ NaOH + ___ HNO3 -->

4 lines
123.

Write a balanced chemical equation for the reaction of the following acid and base:

___ H2SO4 + ___KOH -->

4 lines
124.

A 0.025L solution of HCl is neutralized by 0.018L of a 1.0 M NaOH solution. What is the concentration of the HCl solution?

Use the steps in your notes to help you set up this problem!

a)

1.44 M

b)

4 M

c)

0.72 M

d)

None of the above

125.

A 0.050L solution of Ba(OH)2 is neutralized by 0.072L of a 0.55 M HNO3 solution. What is the concentration of the Ba(OH)2 solution?

a)

2 M

b)

0.40 M

c)

1.2 M

d)

None of the above

126.

A 0.125L solution of NaOH is neutralized by 0.0425L of a 0.65 M H2SO4 solution. What is the concentration of the NaOH solution?

a)

0.1 M

b)

1.6 M

c)

0.44 M

d)

None of the above

127.

A 0.0800L solution of Ca(OH)2 is neutralized by 0.0293L of a 3.58 M H2CrO4 solution. What is the concentration of the Ca(OH)2 solution?

a)

1.31 M

b)

0.49 M

c)

5.32 M

d)

None of the above

128.
What is the molarity of a NaOH solution if 11.6 mL of 3 M HCl was used to neutralize 25 mL of NaOH?
a)
1.392 M
b)
0.155 M
c)
0.718 M
129.

The reaction of perchloric acid (HClO4) with lithium hydroxide (KOH) is described by the equation

HClO4 + KOH → KClO4 + H2O

Suppose 100 mL of perchloric acid is neutralized by exactly 50.0 mL of 1.0 M of Potassium hydroxide. What is the concentration of the perchloric acid?

a)

0.5M

b)

50M

c)

2.0M

d)

1.0M

130.

If it takes 50 mL of 0.5 M Ca(OH)2 to neutralize 125 mL of hydrochloric acid (HCl), what is the concentration of the acid?

a)

0.2 M

b)

5 M

c)

0.5 M

d)

0.4 M

131.
A 50.0 mL sample of Ca(OH)2 is neutralized by 300.0 mL of HCl solution with a pH of 1.3. Calculate the molarity of the Ca(OH)2 solution.
a)
1.0 M
b)
0.50 M
c)
0.15 M 
d)
0.30 M
132.

How are acid equilibrium constants often expressed?

a)

Positive logarithms

b)

Negative logarithms

c)

Both positive and negative logarithms

d)

Neither positive or negative logarithms

133.

What is the name of this ion: [H3O+]?

a)

Hydroxide ion

b)

Hydronium ion

c)

Helium ion

d)

Helium oxide ion

134.
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.
135.

Which of the following would be a weak base?

a)
b)
c)
d)
136.

HA, a weak acid, is partially dissociated in water into hydrogen ions and A- . Which of the following equation represents dissociation of HA, a weak acid, in water?

a)

HA(aq) ⇌ H- (aq) + A+ (aq)

b)

H- (aq) + A+ (aq) ⇌ HA(aq)

c)

HA(aq) ⇌ H+ (aq) + A- (aq)

d)

H+ (aq) + A- (aq) ⇌ HA(aq)

137.

dissociation of weak acid, HA, is represented by following equation :


HA(aq) + H2O(l) ⇌ H3O+(aq) + A-(aq)


The equilibrium constant for this reaction is represented by Ka . Which of the following equation represents expression of equilibrium constant, Ka?

a)
b)
c)
d)
138.
Consider the general equation for an acid in water:
HA(aq) + H2O ↔ H3O+ + A-
If there is a lot of product, what does that tell you about the acid?
a)
Ka > 1  Strong acid
b)
Ka > 1  Weak acid
c)
Ka < 1  Strong acid
d)
Ka < 1  Weak acid
139.

Which of the following is the correct balanced equation showing the complete dissociation of sulfuric acid (a strong acid) into ions?

a)

H2SO4 (aq) → H+ (aq) + SO4–(aq)

b)

H2SO4 (aq) ⇌ 2H+ (aq) + SO42- (aq)

c)

HSO4 (aq) → H+(aq) + SO4–(aq)

d)

H2SO4 (aq) → 2H+ (aq) + SO42- (aq)

140.

Which of the following is the correct definition for a strong acid?

a)

Partially dissociates into ions when dissolved in water and the change is not reversible

b)

Fully dissociates into ions when dissolved in water and the change is not reversible

c)

Fully dissociates into ions when dissolved in water and the change is reversible

d)

Partially dissociates into ions when dissolved in water and the change is reversible

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