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Acid-Base Chemistry

Total questions: 36

Worksheet time: 41mins

Name
Class
Date
1.
What is the Molarity for a solution with the concentration of 60 moles in 20 liters of water?
a)
120 M
b)
3 M
c)
30 M
d)
2 M
2.

What is the conjugate acid for the base NH3?

a)

NH4+

b)

NH2-

c)

NH52+

d)

HCl

3.

What is the H+ concentration of a solution with a pH of 2?

a)

.01 moles/L

b)

.1 moles/L

c)

.0001 moles/L

d)

.000001 moles/L

4.

What is the pH of a solution with .0001 moles per L of H+?

a)

4

b)

3

c)

10

d)

13

5.

What is the conjugate base of HCl?

a)

Cl-

b)

H2Cl+

c)

HCl

d)

H2O

6.

An acid that consists of hydrogen plus one other element is known as a ________________ ?

a)

Binary Acid

b)

Trinary Acid

c)

Tertiary Acid

d)

Binary Base

7.
Which of the following is NOT a property of a base? 
a)
Conduct electricity
b)
Change the color of an indicator solution
c)
Taste sour
d)
Are slippery when mixed with water
8.

According to ___________________, a base is any substance that donates OH- ions in aqueous solutions.

a)

Arrhenius

b)

Bronsted-Lowry

c)

Lewis

d)

Newman-Wright

9.

According to ___________________, a base is any substance that accepts a proton.

a)

Arrhenius

b)

Bronsted-Lowry

c)

Lewis

d)

Newman-Wright

10.
A ________________ acid ionizes (dissociates) completely. 
a)
Strong
b)
Weak
c)
Medium
d)
Moderate
11.
A ______________ acid can only donate one proton. 
a)
Monoprotic
b)
Polyprotic 
c)
Diprotic
d)
Triprotic 
12.
A ______________ acid can donate 2 protons.
a)
Monoprotic
b)
Polyprotic 
c)
Diprotic
d)
Triprotic 
13.
A reaction in which H+ and OH- cancel each other out is known as a __________________ reaction. 
a)
Neutralization
b)
Combustion
c)
Single Replacement
d)
Synthetic 
14.

The Kw constant is ____________ at 25oC.

a)

1.0 x 10-14

b)

1.0 x 1014

c)

6.022 x 1023

d)

6.0634 x 10-34

15.

pH + pOH = ________ at 25oC

a)

14

b)

7

c)

10

d)

9

16.
To find the pH of a solution you take the _______________ of the H3O+ concentration. 
a)
-log
b)
log
c)
cos
d)
tan
17.
What is the conjugate base in the following reaction?
a)
HCO3- 
b)
HCl
c)
 H2CO3 
d)
Cl-
18.
Which of the following is not a strong acid?
a)
HCl
b)
HF
c)
HBr
d)
HNO3
19.
What is the conjugate base of HCO3-?
a)
HCO3-
b)
H2CO3-
c)
H2CO3
d)
CO32-
20.
If a solution has a [H+] of 1.2 x 10-4M what is the [OH-]?
a)
8.3 x 10-4M 
b)
8.3 x 10-11M 
c)
1.2 x 1010M 
d)
1.2 x 10-4M 
21.
What is the [OH-] if the pH is 4.9?
a)
7.94 x 10-10 M
b)
1.0 x 10-4  M
c)
7.94 x 10-14 M
d)
4.9 x 10-10 M
22.
What is the pOH of a solution that has a pH of 2?
a)
10
b)
12
c)
14
d)
1
23.
Tastes Sour
a)
Acids
b)
Bases
c)
Salts
d)
All
24.
Tastes bitter.
a)
Acids
b)
Bases
c)
Salts
d)
All
25.

sodium hydroxide (NaOH)

a)

strong acid

b)

weak acid

c)

strong base

d)

weak base

26.

BASE + ACID ----> SALT + ???

a)

water

b)

oxygen

c)

hydrogen ion

d)

hydroxide ion

27.
If 25 mL of a Ca(OH)2 solution is needed to neutralize 15 mL of 0.18 M HC2H3O2, what is the concentration of the Ca(OH)2 solution?
a)
0.216 M
b)
0.108 M
c)
0.3 M
d)
0.054 M
28.
Classify the following solution:
15 M  HCl
a)
dilute, strong acid
b)
concentrated, strong acid
c)
dilute, weak acid
29.
Classify the following compound:
0.1 M  NaOH
a)
dilute, weak base
b)
dilute, strong base
c)
concentrated, strong base
30.

A weak acid titrated to the equivalence point with a strong base will produce a _____________?

a)

neutral solution

b)

acidic solution

c)

basic solution

31.

If a strong acid is titrated with a strong base to its equivalence point, the resulting solution will be ___________.

a)

neutral

b)

acidic

c)

basic

32.

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

a)

vinegar

b)

milk

c)

water

d)

bleach

33.

An organic substance that changes color as the pH of the solution changes is called a(n) ______________.

a)

indicator

b)

inhibitor

c)

catalyst

d)

salt

34.

What is the main purpose of acid-base titrations?

a)

To test if reactants react.

b)

To calculate the concentration of unknown analyte.

c)

To calculate the concentration of known analyte.

d)

To test quality of reactants.

35.

What is an equivalence point?

a)

It is the point when enough analyte has been added.

b)

It is the point when the amount of added titrant is equal to the amount of analyte in the solution.

c)

It is the point when the volume of titrant is equivalent the volume of analyte.

d)

It is the point when the concentration of titrant added is equivalent to the volume of analyte.

36.
what is the reading on this burette?
a)
4.40mL
b)
3.50mL
c)
3.60mL
d)
4.50mL

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