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Unit 15 : Acids and Bases Review

Total questions: 39

Worksheet time: 45mins

Name
Class
Date
1.

Which acid is nitric acid?

a)

HNO3

b)

NH3

c)

HN-3

d)

HNO2

2.

Which of the following is named using the prefix hydro- and the suffic -ic?

a)

HBr

b)

HNO2

c)

H2CO3

d)

H3PO4

3.

What is the name of the base, NaOH?

a)

sodium hydroxide

b)

monsodium hydroxide

c)

sodium (I) hydroxide

d)

sodium oxide

4.

What is an acid capable of donating or releasing in water?

a)

a proton, H+

b)

an electron, e-

c)

a neutron, n0

d)

oxygen ions

5.

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

6.

Bases have a pH of

a)

7

b)

Less than 7

c)

More than 7

7.

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

8.

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

9.

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

10.

A bronsted lowry 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

11.

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

12.

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

13.

Identify the true statement about the following reaction:

F- + H2O --> HF +OH-

a)

H2O is a bronsted lowry base

b)

H2O is not an acid or base according to either model

c)

H2O is a bronsted lowry acid

d)

H2O is an arrhenius acid

14.

Acid-base conjugate pairs differ by a single

a)

Electron

b)

Proton

c)

Neutron

d)

Oxygen

15.

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-

16.

Which of the following statements is true concerning acids and bases?

a)

acids and bases don't react with each other

b)

acids mixed with bases neutralize each other

c)

acids mixed with bases make stronger bases

d)

acids mixed with bases make stronger acids

17.

Neutral solutions have a pH of:

a)

0

b)

1

c)

7

d)

14

18.

Which is true?

a)

pH of less than 7 is basic; pH of more than 7 is acidic

b)

pH of less than 7 is acidic; pH of more than 7 is basic

19.

A sour taste is a characteristic of:

a)

acids

b)

bases

c)

neutral

d)

pH scale

20.

Which is a characteristic of a base?

a)

tastes sour

b)

found mostly in foods

c)

feels slippery

d)

turn litmus paper red

21.

pH is the measure of the concentration of ______.

a)

Acids

b)

H+ ion

c)

OH- ion

d)

Bases

22.

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

23.

What is being donated/accepted between conjugate acid-base pairs?

a)

a hydrogen (H+) ion

b)

a hydroxide (OH-) ion

c)

water

d)

a neutron

24.

What is the conjugate base in the following reaction?

a)

HCO3-

b)

HCl

c)

H2CO3

d)

Cl-

25.

Which of the following correctly identifies an Acid-Base Pair?

a)

HH4+ , OH-

b)

H2O , OH-

c)

CaCO3 ,CaCl2

d)

HNO3 , H2SO4

26.
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)
27.
What methods can you use to measure the pH of a solution?
a)
Observing color or clarity
b)
Measuring mass or volume
c)
Measuring density or electrical conductivity
d)
Using acid base-indicators or pH meters
28.
Which is the stronger acid?
a)
pH 1
b)
pH 4
c)
pH 8
d)
pH 13
29.

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

30.

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

a)

Acid

b)

Base

c)

Neutral

31.
If the pH of a solution is 5.6 the pOH is
a)
6.5
b)
12.4
c)
8.4
d)
5.6
32.
A  pH and a pOH will add up to:
a)
0
b)
7
c)
14
d)
1.0 x 10-14
33.

What is the equation for calculating pH?

a)

pH = [H+]

b)

pH = log [H+]

c)

pH = -log[OH-]

d)

pH = -log [H+]

34.
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
35.
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
36.

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

37.
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
38.

Kw = [OH- ][H3O+]

a)

Kw = 14

b)

Kw = 1 x 10-14

c)

Kw = 1 x 1014

d)

Kw = 0

39.

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

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