Pre CH18 HW for Silberberg
Followings are what you will find at the end of the chapter in your textbook.
For LEARNING OBJECTIVES: Highlight the main idea for EACH objective. Ready carefully so you
don’t highlight everything.
For MASTER THESE SKILLS: Highlight the main idea for each skill. Ready carefully so you don’t
highlight everything.
For KEY TERMS: Make sure you can define it and/or give an example of it. Pick TWO terms of your
choice and actually write the definition or an example.
For KEY EQUATIONS AND RELATIONSHIP: Next to EACH, define each term. Be very specific.
CHAPTER REVIEW GUIDE
Learning Objectives Relevant section (§) and/or sample problem (SP) numbers appear in parentheses.
Understand These Concepts
1.
2.
3.
4.
5.
6.
Why the proton is bonded to a water molecule, as H3O+, in all aqueous acid-base systems (§18.1)
The Arrhenius definitions of an acid and a base (§18.1)
Why all reactions of a strong acid and a strong base have the same
(§18.1)
How the strength of an acid (or base) relates to the extent of its dissociation into ions in water (§18.1)
How relative acid strength is expressed by the aciddissociation constant Ka (§18.1)
Why water is a very weak electrolyte and how its autoionization is expressed by Kw (§18.2)
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7. Why [H3O+] is inversely related to [OH–] in any aqueous solution (§18.2)
8. How the relative magnitudes of [H3O+] and [OH–] define whether a solution is acidic, basic, or neutral
(§18.2)
9. The Brønsted-Lowry definitions of an acid and a base and how an acid-base reaction can be viewed as a
proton-transfer process (§18.3)
10. How water acts as a base (or as an acid) when an acid (or a base) dissolves in it (§18.3)
11. How a conjugate acid-base pair differs by one proton (§18.3)
12. How a Brønsted-Lowry acid-base reaction involves two conjugate acid-base pairs (§18.3)
13. Why a stronger acid and base react (Kc > 1) to form a weaker base and acid (§18.3)
14. How the percent dissociation of a weak acid increases as its concentration decreases (§18.4)
15. How a polyprotic acid dissociates in two or more steps and why only the first step supplies significant
[H3O+] (§18.4)
16. The effects of electronegativity, bond polarity, and bond strength on acid strength (§18.5)
17. Why aqueous solutions of small, highly charged metal ions are acidic (§18.5)
18. How weak bases in water accept a proton rather than dissociate; the meaning of Kb and pKb (§18.6)
19. How ammonia, amines, and weak-acid anions act as weak bases in water (§18.6)
20. Why relative concentrations of HA and A– determine the acidity or basicity of their solution (§18.6)
21. The relationship of the Ka and Kb of a conjugate acid-base pair to Kw (§18.6)
22. The various combinations of cations and anions that lead to acidic, basic, or neutral salt solutions
(§18.7)
23. Why the strengths of strong acids are leveled in water but differentiated in a less basic solvent (§18.8)
24. The Lewis definitions of an acid and a base and how a Lewis acid-base reaction involves the donation
and acceptance of an electron pair to form a covalent bond (§18.9)
25. How molecules with electron-deficient atoms, molecules with polar multiple bonds, and metal cations
act as Lewis acids (§18.9)
Master These Skills
1. Classifying strong and weak acids and bases from their formulas (SP 18.1)
2. Using Kw to calculate [H3O+] or [OH–] in an aqueous solution (SP 18.2)
3. Using p-scales to express [H3O+], [OH–], and K (§18.2)
4. Calculating [H3O+], pH, [OH–], and pOH (SP 18.3)
5. Identifying conjugate acid-base pairs (SP 18.4)
6. Using relative acid strengths to predict the net direction of an acid-base reaction (SPs 18.5, 18.6)
7. Calculating Ka of a weak acid from pH (SP 18.7)
8. Calculating [H3O+] (and, thus, pH) from Ka and [HA]init (SP 18.8)
9. Applying the quadratic equation to find a concentration (Follow-up Problem 18.8A)
10. Calculating the percent dissociation of a weak acid (§18.4 and SP 18.9)
11. Calculating [H3O+] and other concentrations for a polyprotic acid (SP 18.10)
12. Predicting relative acid strengths of nonmetal hydrides and oxoacids (§18.5)
13. Calculating pH from Kb and [B]init (SP 18.11)
14. Finding Kb of A– from Ka of HA and Kw (§18.6 and SP 18.12)
15. Calculating pH from Kb of A– and [A–]init (SP 18.12)
16. Predicting the relative acidity of a salt solution from the nature of the cation and anion (SPs 18.13,
18.14)
17. Identifying Lewis acids and bases (SP 18.15)
Key Terms Page numbers appear in parentheses.
Section 18.1
hydronium ion, H3O+ (778)
Arrhenius acid-base definition (778)
neutralization (778)
acid-dissociation (acid-ionization) constant (Ka) (780)
Section 18.2
autoionization (782)
ion-product constant for water (Kw) (783)
pH (784) = -log [H3O+]
acid-base indicator (786)
Section 18.3
Brønsted-Lowry acid-base definition (787)
proton donor (787)
proton acceptor (787)
conjugate acid-base pair (788)
Section 18.4
polyprotic acid (797)
Section 18.6
base-dissociation (base-ionization) constant (Kb) (802)
Section 18.8
leveling effect (811)
Section 18.9
Lewis acid-base definition (811)
adduct (811)
Key Equations and Relationships Page numbers appear in parentheses.

18.1 Defining the acid-dissociation constant (780):
Ka = eq constant to acid, [ ] = concentration in M

18.2 Defining the ion-product constant for water (783):

18.3 Defining pH (784):

18.4 Relating pKw to pH and pOH (785):

18.5 Finding the percent dissociation of HA (795):

18.6 Defining the base-dissociation constant (802):

18.7 Expressing the relationship among Ka, Kb, and Kw (805):
Answer the following questions. Show your work.
a. Look up the list of strong acids and list them here.
b. What is the conjugate acid of HCO3-1 ?
c. What is the conjugate base of HCO3-1 ?
d. What is a salt? Give two examples.
e. Define leveling effect.
f. Write chemical equation showing auto-ionization of water.
g. Write chemical equation showing acid-dissociation of HF (aq).
h. Write K expression for the equation for equation above.