Holt Ch 14
Presentation
•
Chemistry
•
9th - 12th Grade
•
Practice Problem
•
Hard
Connie Schaef
FREE Resource
45 Slides • 25 Questions
1
2
3
Multiple Select
Which of the following are correct steps in naming a binary acid?
Begin with the prefix hydro-
End the name with the suffix -ic
Use the root of the second element's name
Add the prefix per-
4
Open Ended
Name a compound that is an acid under the Lewis definition but not under the Brønsted-Lowry definition.
5
Open Ended
Explain how Arrhenius acids behave in water and why all aqueous acids are considered electrolytes.
6
7
8
Multiple Choice
Which of the following best explains why two solutions can have different pH values?
They contain different amounts of water.
They are at different temperatures.
They have different concentrations of acids or bases.
They are in different types of containers.
9
10
Open Ended
Why is understanding the difference between acids and bases important in everyday life?
11
12
13
14
Multiple Choice
Which of the following is NOT a general property of aqueous acids?
They have a sour taste.
They change the color of acid-base indicators.
They react with bases to produce salts and water.
They are always solid at room temperature.
15
16
17
Fill in the Blanks
The acid with the formula HBr is called
Type answer...
18
19
20
Open Ended
Explain the difference between a binary acid and an oxyacid, providing an example of each.
21
22
23
Open Ended
Describe the pattern followed in naming the anions of oxyacids, using at least two examples from the provided table.
24
25
Multiple Choice
Which of the following acids has the anion sulfate?
Sulfuric acid
Nitric acid
Acetic acid
Phosphoric acid
26
27
28
29
30
31
32
Multiple Select
Which of the following are properties of bases?
Taste bitter
React with acids to produce salts and water
Feel slippery in dilute aqueous solutions
Release hydrogen ions in water
33
34
Multiple Choice
Which of the following statements best describes how ammonia (NH3) acts as a base in water?
It dissociates completely into ions.
It produces hydroxide ions by reacting with water molecules.
It forms a precipitate with water.
It does not interact with water at all.
35
36
Fill in the Blanks
An Arrhenius base increases the concentration of
Type answer...
37
38
Fill in the Blanks
The strength of a base depends on the extent to which it
Type answer...
39
40
Multiple Choice
Which of the following compounds is a strong base according to the table provided?
NH3
C6H5NH2
KOH
NH4Cl
41
42
Multiple Choice
Based on the information in the first two slides, what is the main difference between strong and weak bases?
Strong bases are molecular, weak bases are ionic.
Strong bases dissociate completely in water, weak bases do not.
Weak bases are always acids in disguise.
Strong bases do not contain hydroxide ions.
43
44
45
Open Ended
Explain how the concentrations of H3O+ and OH− ions determine whether a solution is acidic, neutral, or basic.
46
47
48
49
50
Multiple Choice
Which of the following best describes a Brønsted-Lowry acid?
A molecule or ion that is a proton donor
A molecule or ion that is a proton acceptor
A molecule or ion that produces OH- in water
A molecule or ion that produces H2O in a reaction
51
52
53
Multiple Choice
In the reaction HCl + NH3 → NH4+ + Cl-, which substance acts as the Brønsted-Lowry base?
NH3
HCl
NH4+
Cl-
54
55
56
Open Ended
Explain how protons are transferred in a Brønsted-Lowry acid-base reaction, using the reaction between HCl and NH3 as an example.
57
58
59
Fill in the Blanks
A monoprotic acid can donate only
Type answer...
60
61
62
63
Multiple Choice
Which of the following acids is polyprotic?
H2SO4
HCl
HNO3
HClO4
64
65
Multiple Select
Which of the following ions are present in a solution of sulfuric acid after both ionization steps?
H3O+
HSO4-
SO4^2-
Cl-
66
67
68
69
Open Ended
What questions do you still have about acids, bases, or the concept of pH after this lesson?
70
Multiple Choice
How does the difference in pH between two solutions help you determine whether they are acidic or basic?
A lower pH indicates a basic solution, and a higher pH indicates an acidic solution.
A lower pH indicates an acidic solution, and a higher pH indicates a basic solution.
Both acidic and basic solutions have the same pH.
pH does not help in determining if a solution is acidic or basic.
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