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Acids and Bases Review Quizizz

Total questions: 67

Worksheet time: 4hrs 14mins

Name
Class
Date
1.

Which solution can turn phenolphthalein pink?

a)

Sodium hydroxide

b)

Vinegar

c)

Tomato

d)

Hydrochloric acid

2.

Which solution would turn litmus red?

a)

Potassium hydroxide

b)

Sodium chloride

c)

HNO3

d)

Ammonia

3.

Which solution would turn litmus blue?

a)

HCl

b)

Citric fruits

c)

H2SO3

d)

NH3

4.

Which of the set of pH paper depicts that the dipped solution is highly acidic?

(compare with the pH scale and find out)

a)
b)
c)
5.
Litmus paper is an indicator of acids and bases, it turns red for bases.
a)
True
b)
false
6.
What is a substance that is one color in an acid and another color in a base? 
a)
Oxidizer
b)
Indicator
7.
The pH of a strong base would be:
a)
1-2
b)
5-6
c)
8-9
d)
13-14
8.
The pH of a weak base would be:
a)
1-2
b)
5-6
c)
8-9
d)
12-13
9.
The pH of a weak acid would be:
a)
1-2
b)
5-6
c)
8-9
d)
12-13
10.

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

a)

H+

b)

OH-1

11.

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

a)

H+1

b)

OH-1

12.

When using the Bronsted Lowry definition of acids and bases, the acid will ______________ a hydrogen proton.

a)

donate

b)

accept

13.

When using the Bronsted Lowry definition of acids and bases, the base will ______________ a hydrogen proton.

a)

donate

b)

accept

14.

In the following chemical equation, which compound is the acid?


HCl + NH3 → NH4+ + Cl−

a)

HCl

b)

NH3

c)

NH4+

d)

Cl−

15.
Neutralization reactions
a)
formed from joining positive and negative ions 
b)
increases OH ions
c)
froms a salt and water
d)
increases H2O ions
16.

What range of values on the pH scale represent solutions with a higher ratio of hydroxide (OH-) ions?

a)

below 7

b)

7

c)

above 7

d)

0-14

17.

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

18.

HCl is:

a)

an Arrhenius acid

b)

a Bronsted Lowry acid

c)

both an Arrhenius and Bronsted Lowry acid

d)

a base

19.

NaOH is:

a)

an Arrhenius base

b)

an Arrhenius acid

c)

neither an acid nor a base

d)

both an acid and a base

20.

NH3 is:

a)

a Bronsted Lowry base

b)

an Arrhenius base

c)

an acid

d)

both an Arrhenius and a Bronsted Lowry base

21.

pH is the measure of the concentration of ______.

a)

Acids

b)

H+ ion

c)

OH- ion

d)

Bases

22.

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+

23.

According to Bronsted-Lowry, what is the definition of an BASE?

a)

a substance that donates a hydrogen (H+) ion

b)

a substance that donates a hydroxide (OH-) ion

c)

a substance that accepts a hydrogen (H+) ion

d)

a substance that accepts a hydroxide (OH-) ion

24.

What is the conjugate base in the following reaction?

a)

HCO3-

b)

HCl

c)

H2CO3

d)

Cl-

25.
Which of the following shows the correct conjugate acid base pair?
a)
HCI (acid) / H3O+ (conjugate base)
b)
HCI (acid) / CI- (conjugate base)
c)
HCI (base) / CI- (conjugate acid)
d)
HCI (base) / H3O+ (conjugate acid)
26.
If a solution is basic which ion will be more present?
a)
H+
b)
K+
c)
OH-
d)
H-
27.

Which of the following are properties of acids but not bases? Select all that apply.

a)

Changes the color of an indicator

b)

Sour taste

c)

Reacts with metals to produce hydrogen gas

d)

Feels slippery

28.

Neutralization is the process of an acid and a base reacting to form what? Select all that apply

a)

An ionic salt

b)

Hydronium ions

c)

NaCl

d)

Water

29.

An arrhenius acid

a)

produces hydroxide ions in a solution

b)

is a proton donor

c)

produces hydrogen ions in a solution

d)

is a proton acceptor

30.

An arrhenius base

a)

produces hydroxide ions in a solution

b)

is a proton donor

c)

produces hydrogen ions in a solution

d)

is a proton acceptor

31.

A bronsted lowry acid

a)

produces hydroxide ions in a solution

b)

is a proton donor

c)

produces hydrogen ions in a solution

d)

is a proton acceptor

32.

Water can act as both an acid and a base according to the bronsted lowry model. This means water is

a)

neutral

b)

conjugate

c)

ionic

d)

amphoteric

33.

Acid-base conjugate pairs differ by a single

a)

Electron

b)

Proton

c)

Neutron

d)

Oxygen

34.

Which of the following show an acid and its conjugate base pair (in that order)

a)

H2SO4, SO42-

b)

OH-, H2O

c)

NH4+, H2O

d)

H2CO3, HCO3-

35.

Could C2H3O2- act as a base when placed in water?

a)

Yes, because it can accept a H+

b)

Yes, because it can donate a H+

c)

No, because it cannot donate a H+

d)

No, because it cannot accept a H+

36.

For a solution, pH + pOH =

a)

7

b)

1.0 x 10-14

c)

14

d)

-log (1.0 x 10-14)

37.

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

a)

4.0

b)

1.0 x 10-4

c)

10

d)

Cannot be determined from the information

38.

The pH of a solution is 8.43. What is the hydrogen ion H+ 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

39.

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

a)

2

b)

12

c)

-2

d)

1

40.

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

41.

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

a)

10.44

b)

3.56

c)

1.00

d)

-4.43

42.

If the [H+] of a solution is 6.8 x 10-9 M, the pH is

a)

8.17

b)

5.73

c)

9.99

d)

8.62

43.

if the [H+] of a solution is 8.4 x 10-3 M, the pOH of the solution will be

a)

2.08

b)

11.92

c)

1.02

d)

12.98

44.

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

45.

Limes have a [H+] of 1.3 x 10-2 M. Their pOH is

a)

1.89

b)

12.11

c)

1.03

d)

12.97

46.

Which of the following is true for a strong acid in aqueous solution?

a)

It partially ionizes in water

b)

It forms a weak base

c)

It completely ionizes in water

d)

It does not ionize in water

47.

What is the pH of a neutral solution at 25°C?

a)

0

b)

7

c)

14

d)

1

48.

Which of the following substances is amphoteric?

a)

NaCl

b)

NaOH

c)

HCl

d)

H2O

49.

Which of the following substances will increase the pH of a solution when added?

a)

CH3COOH

b)

NaOH

c)

NH4Cl

d)

HCl

50.

What is formed when an acid reacts with a base in a neutralization reaction?

a)

Only water

b)

Only salt

c)

Salt and water

d)

Hydrogen gas

51.

Which indicator turns blue in the presence of a base?

a)

Bromothymol blue

b)

Litmus paper

c)

Methyl orange

d)

Phenolphthalein

52.

Which of the following is a property of a strong acid?

a)

It does not react with water

b)

It partially dissociates in water

c)

It forms a weak base

d)

It completely dissociates in water

53.

What color does litmus paper turn in the presence of an acid?

a)

Green

b)

Blue

c)

Yellow

d)

Red

54.

Which of the following substances is considered a weak base?

a)

NaOH

b)

NH3

c)

HCl

d)

CH3COOH

55.
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
56.
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
57.
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
58.
Identify the products of the chemical equation
3 LiOH + H3PO4 →
a)
Li3PO4 + 3 H2O
b)
LiPO4 + 3 H2O
c)
Li(PO4)3 + 3 H2O
d)
BOY + La + N2
59.
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
60.
How many moles of Ca(OH)2 are needed to neutralize three moles of HCl? 
a)
8
b)
1.5
c)
6
d)
3
61.
For the acid-base titration combination of NaOH with 0.79 mol HCl, find the number of moles of NaOH that would be the chemically equivalent amount of HCl.
a)
0.79 mol
b)
1.6 mol
c)
0.38 mol
d)
3.2 mol
62.

What allows us to know when the end point has been reached?

a)

Bubbles

b)

Feels warm

c)

indicator changing color

d)

Turns to a solid

63.

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

64.
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
65.

A titration works by using a ___________________________ reaction.

a)

Single Replacement

b)

Neutralization

c)

Combustion

d)

Synthesis

66.

Indicators are used in a titration by changing ___________________ at different pH levels.

a)

Smell

b)

Shape

c)

Phase

d)

Color

67.

How many mL of 1.00 M H2SO4 is needed to neutralize 21.5 mL of 1.50 M KOH?

H2SO4 + 2KOH → K2SO4 + 2H2O

a)

16.1 mL

b)

1.10 mL

c)

5.65 mL

d)

0.900 mL

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