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Acids, Bases, and Equilibrium

Total questions: 35

Worksheet time: 1hrs 8mins

Name
Class
Date
1.

HSO4¯ + H2O ↔ H3O+ + SO4 2¯ In the equilibrium represented above, the species that act as bases include which of the following?

a)

HSO4-

b)

H2O

c)

SO4 2¯

d)

H2O and SO4 2¯

2.

Which of the following values would represent the pH of a strong base?

a)

1

b)

8

c)

7

d)

13

3.

Which of the following values would represent the pH of a strong acid?

a)

1

b)

6

c)

7

d)

13

4.

What range of values on the pH scale represent solutions with a higher ratio of hydronium (H3O+) ions?

a)

0-14

b)

below 7

c)

7

d)

above 7

5.

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

6.

Pure water (H2O) has a pH of 7 and would be classified as...

a)

a base

b)

a neutral substance

c)

both an acid and a base

d)

an acid

7.

The products of a neutralization reaction are usually...

a)

salt and water

b)

an acid and a base

c)

a neutral solution

d)

carbon dioxide and oxygen

8.

The reactants in a neutralization reaction are always...

a)

salt and water

b)

an acid and a base

c)

a neutral solution

d)

carbon dioxide and oxygen

9.
What is the pH of a solution if [H+] = 6.0 x 10-10 M?
a)
3.45
b)
6.25
c)
9.22
d)
11.34
10.
What is the pH of a solution if [OH-] = 1.0 x 10-5M?
a)
5.00
b)
7.00
c)
9.00
d)
11.00
11.
Which one of the following solutions is the most acidic?
a)
[H+] = 2.4 x 10-6 M
b)
[OH-] = 9.8 x 10-4 M
c)
[H+] = 4.2 x 10-7 M
d)
[OH-] = 1.7 x 10-12 M
12.

Identify the Bronsted Lowry Acid (A) and Base (B) in the given reaction.

a)

A

b)

B

c)

C

d)

D

13.
An equilibrium constant with a large magnitude indicates…
a)
A very fast reaction
b)
Higher concentration of products at equilibrium
c)
Higher concentration of reactants at equilibrium
d)
Nothing, without considering the stoichiometry of the reaction
14.

What is the [H+] when [OH-] = 8.1 x 10-5?

a)

8.1 x 10-5 M

b)

1.0 x 10-7 M

c)

1.2 x 10-10 M

d)

3.6 x 10-6 M

15.

In this rxn: HBr + NH3 --> NH4+ + Br- the acid and its conjugate base, respectively are...

a)

NH3 and NH4+

b)

NH3 and Br-

c)

HBr and NH4+

d)

HBr and Br-

16.
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
17.

A chemical has a pH = 6. It would be best described as

a)

Strong acid

b)

Strong base

c)

Weak acid

d)

Weak base

18.
If an acid is combined with a base of equal strength, the result will most likely be
a)
a neutral solution.
b)
a stronger acid.
c)
impossible to tell without testing the pH.
d)
a stronger base
19.
Which of the following do NOT represent a conjugate acid/base pair?
a)
H3O+/H2O
b)
H2O/OH-
c)
H2CO3/CO3-2
d)
all are conjugate pairs
20.
What is the pH of a 5.0 x 10-3 M KOH solution?
a)
10.10
b)
6.70
c)
2.30
d)
11.70
21.
Calculate the [H+] in a solution that has a pH of 2.73.
a)
5.4 x 10-12 M
b)
1.9 x 10-3 M
c)
2.7 M
d)
11.3 M
22.
What is the conjugate acid in the following equation?
a)
PO43- 
b)
HNO3 
c)
NO3- 
d)
HPO42-
23.

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

a)

Acid

b)

Base

24.
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
25.

The Bronsted Lowry definition of acids is

a)

Acids donate electrons

b)

Acids are proton donors

c)

Acids are proton acceptors

d)

Acids accept electrons

26.
The Bronsted Lowry definition of a base:
a)
Bases contain OH-
b)
Bases are proton donors
c)
Bases are proton acceptors
d)
Bases have a pH less than 7
27.

HBr

a)

strong acid

b)

weak acid

c)

strong base

d)

weak base

28.

What is the conjugate base in the following reaction?

HCO3- + HCl → H2CO3 + Cl-

a)

HCO3-

b)

HCl

c)

H2CO3

d)

Cl-

29.

SiO2(s)+ 4HBr(g) ↔ SiBr4(g) + 2H2O(g)

ΔH = +143.5 kJ


Which way will the reaction shift if water vapor is added?

a)

shift left

b)

shift right

c)

no shift

30.
For the reaction...
SO2 + O2  <=>  SO3
If the concentration of SO2 is increased, the equilibrium position of the reaction will shift ___________.
a)
to the left
b)
to the right
c)
to the left and right 
d)
neither left nor right
31.
For the reaction...
SO2 + O2 <=>  SO3
If the equilibrium position shifts to the right, the concentration of O2 will ___________.
a)
increase
b)
decrease
c)
remain the same
d)
double
32.
What is the Kc expression for this reaction?
   2 NO(g)  +  O2(g) ⇌  2 NO2(g)
a)
Kc = [NO2]2 / [NO]2 [O2]
b)
Kc =  [NO]2 [O2] / [NO2]2
c)
Kc = [NO]2 [O2] [NO2]2
d)
Kc = [NO2]2 / [NO]2 +  [O2]
33.
Le Chatelier's Principle states that.... 
If a (dynamic) equilibrium is disturbed by changing the conditions, the position of equilibrium................
a)
moves to increase the change
b)
moves to counteract the change
c)
does not change
34.
Changes in pressure will only affect substances that are in the __________ state.
a)
gaseous
b)
liquid
c)
solid
35.
What are the products to a neutralization reaction?
a)
H2 + Ionic Salt
b)
H2O + Ionic Salt
c)
H3O+ + Ionic Salt
d)
OH- + Ionic Salt

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