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Acids and Bases review Honors

Total questions: 51

Worksheet time: 57mins

Name
Class
Date
1.

A(n) ______ is a substance with a pH less than 7.

a)

acid

b)

alkaline

c)

base

d)

buffer

2.
The pH of a solution is tested, and it is found to be a basic solution. Of the following choices, what could the pH have been?
a)
3
b)
9
c)
7
d)
5
3.
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
4.

Which of the following are the conjugate bases of HSO4–, CH3OH, and H3O+, respectively?

a)

SO42–, CH2OH–, and OH–

b)

CH3O–, SO42–, and H2O

c)

SO42–, CH3O–, and H2O

d)

SO42–, CH2OH–, and H2O

5.

Which molecule is acting as a base in the following reaction?

OH– + NH4+ → H2O + NH3

a)

OH–

b)

NH4+

c)

H2O

d)

NH3

6.

Which pH would correspond to the weakest base?

a)

8

b)

14

c)

7.8

d)

11.6

7.

Which of the following compounds is a strong acid?

I. HClO4 (aq)

II. H2SO4 (aq)

III. HNO3 (aq)

a)

I only

b)

II only

c)

II and III only

d)

I, II, and III

8.

Which of the following is not a strong base?

a)

Ca(OH)2

b)

Fe(OH)3

c)

KOH

d)

NaOH

9.

What is the pH of a solution that has an [H+] of 2.5 × 10–5?

a)

4.60

b)

5.0

c)

2.5

d)

7

10.

What is the [H+] if the pH is 4.0?

a)

1.0 × 10–10 M

b)

1.0 × 10–4 M

c)

1.0 × 10–14 M

d)

1.0 × 10–7 M

11.

What is the pOH of a solution where the [OH–] is 7.3 × 10–2 M?

a)

-1.14

b)

2.0

c)

1.14

d)

7.3

12.
What is the pOH of a solution that has a pH of 2?
a)
10
b)
12
c)
14
d)
1
13.

What is the pOH of a solution where the [H+] is 2.5 × 10–12 M?

a)

11.6

b)

2.40

c)

12

d)

2.5

14.

If [H3O+] in an aqueous solution is 7.5 × 10–9 M, what is the [OH–]?

a)

6.4 × 10–5 M

b)

3.8 × 10–5 M

c)

7.5 × 10–5 M

d)

1.3 × 10–5 M

15.

Arhenius Acids

a)

Create/increase concentration of H+ ions

b)

Create/increase concentration of OH- ions

c)

Form H+ and OH- from water

d)

Create/increase concentration of H20 molecules

16.

Arrhenius Bases

a)

Create/increase concentration of H+ ions

b)

Create/increase concentration of OH- ions

c)

Create/increase concentration of H20 Molecules

d)

Form H+ and OH- from water

17.

Which of these compounds is an Arhenius Base

a)

LiOH

b)

NH3

c)

H2PO4

d)

CH3COO-

18.

What is transferred between a conjugate acid-base pair

a)

An electron

b)

A proton

c)

A hydroxide ion

d)

A hydronium ion

19.

Water is

a)

Amphoteric

b)

An acid and a base

c)

H30

d)

An acid

20.

Acids ____ a proton(H+)

a)

give away

b)

recieve

c)

steal

d)

bond with

21.

Bases ____ a proton (H+)

a)

give away

b)

lose

c)

recieve

d)

release

22.

An Acid who gives away a proton is now

a)

a conjugate acid

b)

a conjugate base

c)

an acid

d)

a base

23.

What is pH

a)

the negative logarithm of the hydrogen ion concentration

b)

the positive logarithm of the hydrogen ion concentration

c)

the positive logarithm of the hydroxide ion concentration

d)

the negative logarithm of the hydroxide ion concentration

24.

Bases are _____ on the pH scale

a)

7 - 14

b)

0- 14

c)

0 -7

d)

5 - 9

25.

Acids are _____ on the pH scale

a)

7 - 14

b)

0- 14

c)

0 -7

d)

5 - 9

26.

A base has a pOH of

a)

0-7

b)

0-14

c)

7-14

d)

4-9

27.

An acid has a pOH of

a)

0-7

b)

0-14

c)

7-14

d)

4-9

28.

What characterizes a strong acid or base

a)

polar covalent bonding

b)

complete ionization in water

c)

ionic bonding

d)

presence of an ion

29.

Hydronium atoms are

a)

H30+

b)

H+

c)

OH-

d)

H20

30.

Salts that are formed from nuetralization can be

a)

Acid

b)

Base

c)

Neutral

d)

HCl

e)

NaOH

31.

A bronsted Lowry acid

a)

donates protons

b)

receives protons

c)

donates electrons

d)

receives electrons

32.

A bronsted Lowry bas

a)

donates protons

b)

receives protons

c)

donates electrons

d)

receives electrons

33.

Ammonium ((NH4)+) is a

a)

Strong Base

b)

Weak base

c)

Strong Acid

d)

Weak acid

34.

Bases turn the litmus paper

(a)  

35.

acids turn the litmus paper

(a)  

36.

acid + base -->

a)

salt + hydrogen

b)

salt + water

c)

salt + carbon dioxide + water

d)

salt

37.
HCl + NaOH → 
a)
NaH + ClOH
b)
NaCl + H2
c)
NaCl + H2O
d)
NaCl + Cl2
38.
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
39.
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
40.
what is the reading on this burette?
a)
4.40mL
b)
3.50mL
c)
3.60mL
d)
4.50mL
41.
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
42.
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
43.
What acid and what base would you choose to prepare the salt potassium chlorate?
a)
KOH and HClO3
b)
KOH and HClO2
c)
HK and OHClO3
d)
HK and OHClO2
44.
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
45.
How many moles of Ca(OH)2 are needed to neutralize three moles of HCl? 
a)
8
b)
1.5
c)
6
d)
3
46.
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
47.
Changes the color of indicators.
a)
Acids
b)
Bases
c)
All
48.
If phenolphthalein turns bright pink, it indicates
a)
an acid 
b)
a base
c)
a neutral
49.
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
50.
Which of the following is a conjugate acid/base pair?
a)
HCl/OCl-
b)
H2SO4/SO42-
c)
NH4+/NH3
d)
H3O+/OH-
51.

Feels slippery

a)

Acids

b)

Bases

c)

All

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