Acid/Base Study Guide Unit 11
Key terms and Concepts
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Arrhenius
o Arrhenius acid
 H3O+
o Arrhenius base
 OHBronsted-Lowry
o Bronsted- Lowry acid
o Bronsted- Lowry base
o Conjugate acid
o Conjugate base
Lewis
o Acid
o Base
Amphoteric
Polyprotic acid
Binary acids
Ternary acids
[H3O+] > [OH-]
[H3O+] = [OH-]
pH= -log [H+]
Questions you should be able to answer
1. What is the acid ion?
2. What is the base ion?
3. What does pH measure?
4. What does pOH measure?
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pOH = - log[OH-]
[H3O+] < [OH-]
𝐾𝑤
[H3O+] =
[OH−]
𝐾𝑤
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[OH-] = [𝐻 3𝑂+]
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Dissociation
Properties of Acids
Properties of Bases
Titrations
o Indicator
 Phenolthalein
o Equivalence point
Buffer
pH
pOH
Naming
o Acids and bases
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5. What is the pH scale?
a. On the scale, what range is acidic
b. What range is basic
c. What is neutral
Acid/ Base Pairs
Identify
1. In the equation below identify what is the acid, base, conjugate acid, and conjugate base.
H2CO3 + H2O  H3O+ + HCO3-
H2O + NH3   NH4+ + OHNaming Acids
Questions
1. Name the following acids:
a) HF
b) HBr
c) H2S
2. Name the following acids:
a) H2SO4
b) H2CO3
3. Name the following acids:
b) HNO2
c) H2SO3
4. Name the following bases:
a) Mg(OH)2
b) LiOH
Math: complete the following Math problems (show all work)
pH problems
1. What is the pH of the solution if the concentration is
a. [H+] = 0.0056 M
b. [OH-] = .000780 M
2. Identify if the solution in problem #1 is an acid or base.
a.
b.
Titration Problems M1V1 = M2V2
3. If it takes 54 mL of 0.1 M NaOH to neutralize 125 mL of an HCl solution, what is the
concentration of the HCl?
4. If it takes 25 mL of 0.05 M HCl to neutralize 345 mL of NaOH solution, what is the
concentration of the NaOH solution?