Chapter 16: Acids and Bases
Purpose
Acids and bases are special types of solutions. They react to neutralize one another. Acidity is measured on the
pH scale. Indicators show color changes at certain pH levels.
A and B
5/4 and 5/5
5/6 and 5/7
5/8
5/11 and 5/12
5/13 and 5/18
5/14 and 5/15
In-Class
 Chapter 16 Notes
 Go over Chapter 16
Worksheet #1
 Go over Practice SOL
 Lab – Soft Drink Titration
 Go over Chapter 16
Worksheet #2
 Lab – Acids and Bases
 Go over Chapter 16 Review
 Chapter 16 Test
 Chemistry SOL Test
HW Assignments
 Chapter 16 Worksheet #1
 Chapter 16 Worksheet #2
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 Chapter 16 Review
Worksheet
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Vocabulary
acid
base
electrolyte
indicator
end point
equivalence point
titration
neutralization
pH
pOH
Arrhenius
Bronsted Lowry
By the end of this Topic, you should be able to demonstrate proficiency in the following areas:
Essential Understandings
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Two important classes of compounds are acids and bases. Acids and bases are defined by several
theories. According to the Arrhenius theory, acids are characterized by their sour taste, low pH and
the fact that they turn litmus paper red. According to the Arrhenius theory, bases are characterized
by their bitter taste, slippery feel, high pH, and the fact that they turn litmus paper blue. According
to the Bronsted-Lowry theory, acids are proton donors, whereas bases are proton acceptors. Acids
and bases dissociate in varying degrees.
Strong electrolytes dissociate completely. Weak electrolytes dissociate partially. Non-electrolytes
do not dissociate.
pH is a number scale ranging from 0 to 14 that represents the acidity of a solution. The pH number
denotes hydrogen (hydronium) ion concentration. The pOH number denotes hydroxide ion
concentration. The higher the hydronium [H3O+] concentration, the lower the pH.
pH + pOH = 14.00
Strong acid-strong base titration is the process that measures [H+] and [OH-].
Indicators show color changes at certain pH levels.
Essential Knowledge, and Skills
In order to meet this standard, it is expected that students will
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differentiate between the defining characteristics of the Arrhenius theory of acids and bases and the
Bronsted-Lowry theory of acids and bases.
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identify common examples of acids and bases, including vinegar and ammonia.
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compare and contrast the differences between strong, weak, and non-electrolytes.
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relate the hydronium ion concentration to the pH scale.
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perform titrations in a laboratory setting using indicators.
SOL Standards
CH.4 The student will investigate and understand that chemical quantities are based on molar relationships.
Key concepts include
d) acid/base theory; strong electrolytes, weak electrolytes, and nonelectrolytes; dissociation and
ionization; pH and pOH; and the titration process.