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Honors Chemistry Acids and Bases Review 23-24

Total questions: 75

Worksheet time: 2hrs 30mins

Name
Class
Date
1.

What is an Arrhenius acid?

a)

A substance that produces H+ in water.

b)

A substance that produces OH- in water.

2.

What is an Arrhenius base?

a)

A substance that produces H+ ion in water

b)

A substance that produces OH- ion in water.

c)

A substance that produces OH+ ion in water

d)

A substance that produces H- ion in water.

3.

A student tests an unknown aqueous solution and finds it conducts electricity and turns litmus paper red. What can the student infer?

a)

The solution contains an acid.

b)

The solution contains a base.

c)

The solutions is neutral.

4.

A student tests an unknown aqueous solution and finds it conducts electricity and turns litmus paper blue. What can the student infer?

a)

The solution contains an acid.

b)

The solution contains a base.

c)

The solutions is neutral.

5.

​ (a)   conduct electricity and turn litmus paper red.

Choose from the below words
Acids
Bases
Neutral solutions
Salts
6.

Label the acid, base, conjugate acid and conjugate base.

a)acid
b)base
c)conjugate acid
d)conjugate base
1
2
3
4
1)
2)
3)
4)
7.

Click on the acid.

A
B
C
D
8.

Click on the base.

A
B
C
D
9.

Click on the conjugate base.

A
B
C
D
10.

Click on the conjugate acid.

A
B
C
D
11.

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

a)

HCl and NaOH

b)

H3O+ and OH-

c)

H2SO4 and HSO4-

d)

H2S and S2-

12.

According to Bronsted-Lowry, what does an acid do?

a)

It donates a proton (H+).

b)

It accepts a proton (H+)

c)

It produces H+ in water.

d)

It produces OH- in water.

13.

According to Bronsted-Lowry, what does a base do?

a)

It donates a proton (H+).

b)

It accepts a proton (H+)

c)

It produces H+ in water.

d)

It produces OH- in water.

14.

What happens to acids when they react to metals?

a)

Produce Oxygen gas

b)

Helium Gas

c)

Hydrogen gas

15.

Which are slippery when touched?

a)

Acids

b)

Bases

16.

What would the expected pH of a cola be?

a)

2.5 - 3.5

b)

7

c)

8-9

17.

Examine the results (color change) of the pH paper shown in the picture. What type of substance was tested?

a)

an acid

b)

a base

c)

a neutral substance

d)

none of the above

18.
An indicator will ______________ when it is in contact with an acid or base
a)
Bubble
b)
Form a new substance
c)
Change color
d)
Stay the same color
19.

If the substance is neutral, what would the pH be?11

a)

3

b)

5

c)

7

d)

9

e)

11

20.

Ocean water is only slightly basic. What might its pH value be?

a)

5

b)

8

c)

12

d)

2

21.

The strongest bases have pH values close to

a)

0

b)

14

c)

7

d)

5

22.

Which of the following pH values represents a base?

a)

2.1

b)

4.6

c)

6.8

d)

8.1

23.

Which of the following is a property of a base?

a)

bitter taste

b)

reacts with metals

c)

salty

d)

sour taste

24.

Milk is a very weak acid. What might its pH value be?

a)

6.5

b)

7.8

c)

4.2

d)

12.2

25.

Which pH has the most hydrogen ions (H+)?

a)

2

b)

7

c)

10

d)

13

26.

A substance with a pH of 7 is which of the following?

a)

acid

b)

base

c)

neutral

27.

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

28.

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

a)

8

b)

6

c)

7

d)

9

29.
What is the pOH of a solution that has a pH of 2?
a)
10
b)
12
c)
14
d)
1
30.

What is a titration?

a)

when the moles of hydrogen ions is equal to the moles of hydroxide ions

b)

adding a known amount of solution of known concentration to determine the concentration of an unknown

c)

reaction in which an acid and a base react in an aqueous solution to produce a salt and water

d)

the extent of ionization of an acid or base

31.

Phenolophalein turns from clear to pink when the pH turns

a)

acidic

b)

basic

c)

saline

d)

ionic

32.

What completely ionizes in solution?

a)

Weak acids

b)

Strong acids

c)

Strong Salts

d)

Neutral salts

33.

The table shows the pH of several solutions. Which solution is the most acidic?

a)

vinegar

b)

milk

c)

water

d)

bleach

34.

Zn(OH)2 is an example of a...

a)

acid

b)

base

c)

salt

d)

water

35.

H3PO4 is an example of a ...

a)

acid

b)

base

c)

salt

d)

non-electrolyte

36.

The table shows the pH of several solutions. Which solution has the greatest concentration (amount) of H+ ions?

a)

vinegar

b)

milk

c)

water

d)

bleach

37.

The table shows the pH of several solutions. Which solution has the greatest concentration (amount) of OH- ions?

a)

vinegar

b)

milk

c)

water

d)

bleach

38.

For a solution, pH + pOH =

a)

7

b)

14

c)

1.0 x 10-14

d)

-log (1.0 x 10 -14)

39.

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

40.

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

41.

For a solution, pH + pOH =

a)

7

b)

14

c)

1.0 x 10-14

d)

-log (1.0 x 10 -14)

42.

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

43.

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

44.

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

a)

11

b)

-3

c)

3

d)

1

45.

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

46.

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

47.

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

48.

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

a)

acid

b)

base

c)

neutral

d)

metal

49.

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

50.

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

51.

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

52.

A solution has a pH of 6.9. This solution is _____.

a)

an acid

b)

a base

c)

neutral

53.

If a solution has a very low pH, the hydroxide concentration is _______.

a)

very high

b)

very low

c)

zero

54.

If a solution has a very high pH, the hydroxide concentration is _______.

a)

very high

b)

very low

c)

zero

55.

If a solution has a very high hydrogen ion concentration, the hydroxide concentration is _______.

a)

very high

b)

very low

c)

zero

56.

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

57.

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

58.
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
59.
What is the conjugate base in the following reaction?
a)
HCO3- 
b)
HCl
c)
 H2CO3 
d)
Cl-
60.
What is the conjugate acid in the following equation?
a)
PO43- 
b)
HNO3 
c)
NO3- 
d)
HPO42-
61.
The conjugate acid of HCO3- is ___ and the conjugate base of HCO3- is ___.  (remember that H+ ion? well, follow it!!)
a)
H2CO3; CO3-2
b)
CO3-2; CO3-2
c)
H2CO3; H2O
d)
H2O; H2CO3
62.

What is this piece of apparatus called

a)

Pipette

b)

Burette

c)

Janette

d)

Cuvette

63.

Why do we perform a titration?

a)

To determine the concentration of an unknown solution

b)

To see if a reaction will occur between an acid and base

c)

To find the mass of an unknown acid

d)

To find the molar mass of an unknown solution

e)

To calculate the viscosity of the solution

64.

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

65.

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

66.

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

67.
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
68.
I have 25mL of 1M HCl which neutralises 20mL of NaOH. What is the concentration of the NaOH?
a)
0.8 M
b)
1 M
c)
1.25 M
69.
What is the endpoint of a titration
a)
Where the amount of acid and base are balanced according to the equation
b)
Where there is no base
c)
At the end
70.
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
71.
what is the reading on this burette?
a)
4.40mL
b)
3.50mL
c)
3.60mL
d)
4.50mL
72.
acid + base ₋>
a)
salt + hydrogen
b)
salt + water
c)
salt + carbon dioxide + water
d)
salt
73.
HCl + NaOH → 
a)
NaH + ClOH
b)
NaCl + H2
c)
NaCl + H2O
d)
NaCl + Cl2
74.

A 10.00 mL sample of H2SO4 was neutralized by 13.5 mL of 1.00 M KOH by the following reaction: H2SO4 +  2KOH  →  K2SO4  +  2H2OH_2SO_4\ +\ \ 2KOH\ \ \rightarrow\ \ K_2SO_4\ \ +\ \ 2H_2O  
What is the molarity of H2SO4?

a)

0.675 M

b)

0.910 M

c)

1.05 M

d)

1.20 M

75.

A 25.00 mL sample of HCl was titrated to the end point with 15.00 mL of 2.00 M NaOH. The following neutralization reaction occured: HCl  +  NaOH  →  NaCl  +  H2OHCl\ \ +\ \ NaOH\ \ \rightarrow\ \ NaCl\ \ +\ \ H_2O  
What is the molarity of the HCl? 

a)

0.650 M

b)

1.05 M

c)

1.20 M

d)

1.50 M

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