Name__________________________________________________#____________ Honors Chemistry Reading Guide
Carpenito/Dinota/Ingoglia
Acids and Bases
(Chapters 14 and 15)
Chapter 14
Section 1: Properties of Acids and Bases
Define the following terms:
binary acid:
oxyacid:
Arrhenius acid:
Arrhenius base:
strong acid:
weak acid:
Compare the general properties of acids with the general properties of bases.
Distinguish between binary and oxyacids in terms of their components and the way that they are named.
What acid is the most commonly produced industrial chemical in the world? What is it used for?
Name three other acids and summarize their uses.
Explain HOW acids produce ions when in aqueous solution.
What is the difference between a strong acid and a weak acid?
Organic acids contain what functional acid group? What hydrogen atom is ionizable in organic acids such
as acetic acid?
How can substances (such as ammonia) form hydroxide ions in aqueous solution when there is no
hydroxide ion in their molecular formula?
What is the difference between a strong base and a weak base?
Section 2: Acid-Base Theories
Define the following terms:
Bronsted-Lowry acid:
Bronsted-Lowry base:
monoprotic acid:
polyprotic acid:
Lewis acid:
Lewis base:
Write Bronsted-Lowry acid-base reactions to show how carbonic acid (H2CO3)ionizes completely in
water:
Which of the three acid-base theories has the broadest scope (covers the greatest number of
compounds)?
Is it possible for a compound to be an acid or base according to all three theories? Explain your answer.
Section 3: Acid-Base Reactions:
Define the following terms:
conjugate base:
conjugate acid:
amphoteric:
neutralization:
salt:
What is the relationship between the strength of an acid and the strength of its conjugate base?
What trend is favored in the direction of proton-transfer reactions?
What characteristics do most amphoteric species have in common?
How does the number of oxygens in a molecule affect the strength of an acid?
Why are reactions between and acid and a base referred to as “neutralization” reactions?
Use Figure 3.1 to identify the strongest base:
strongest acid:
weakest base:
weakest acid:
Chapter 15
Section 1: Aqueous Solutions and the Concept of pH
Define the following terms:
self-ionization of water:
Kw:
pH:
Why is pure water an extremely weak electrolyte?
What is true about the relationship between [H3O+] and [OH-] in acidic solutions? in basic solutions?
Find the [OH-] in a solution whose [H3O+]= 3.0 x 10-4 Show your work!
What do the letters “pH” stand for?
Arrange the following in terms of increasing pH using Figure 1.6.
blood, bread, tomatoes apples sea water, saliva
How are significant figures determined in pH values?
How is the [H3O+] determined for a strong acid or base? for a weak acid or base?
Section 1: Aqueous Solutions and the Concept of pH
Define the following terms:
acid-base indicators:
transition interval:
titration:
equivalence point:
end point:
standard solution:
Explain how indicators can be used to estimate the pH of a solution. Why can indicators NOT be used to
measure the exact pH of a solution?
What happens to the pH of an acid solution as the equivalence point in a titration is approached?
How is a specific indicator chosen based on the relative acid and base strengths in a titration?
Look at Figure 2.7 and describe three main differences between a strong acid-strong base titration and a
weak acid-strong base titration.
Read through the titration techniques in Figure 2.8. Why is it not necessary to refill burets to the 0 mark
when completing sequential titrations?
How can you determine from your data that your titration results are sufficiently precise?