Name ____________________________________________ Date _________________________ Period__
Sample Problems for Chapter 14: Acids and Bases
14.1 Acids and Bases
1.
(Read pgs. 442-446 in the chemistry textbook)
(a) What does it mean to say a solid substance has dissolved in water?
(b) What does it mean for a chemical to dissociate (ionize) in aqueous solution?
2.
(a) What is an electrolyte?
b) What are strong electrolytes?
(c) What are weak electrolytes?
(d) what is a nonelectrolyte?
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3.
(a) Fill in the following table of electrolytes:
Summary of Electrolytic Behavior of Common Soluble Ionic and Molecular Compounds
Compound
Strong Electrolyte
Weak Electrolyte
Nonelectrolyte
Ionic
Molecular
(b) What happens if an ionic substance is insoluble in water?
4. Identify each of the following as a strong, weak, or nonelectrolyte based on their chemical formulas.
i.
CO2
vi.
NH4CH3COOH
ii.
KNO3
vii.
LiBr
iii.
C2H6
viii.
XeF2
iv.
Mg(OH)2
ix.
PbSO4
v.
NaCl
x.
Ca3(PO4)2
5. Identify the non-, strong, and weak electrolytic solutions below. Explain your choices.
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6.
(a) What is the hydronium ion?
(b) What is the symbol for the hydronium ion?
7.
(a) What is the hydroxide ion?
(b) What is the symbol for the hydroxide ion?
8. What is an acid?
9. What is a base?
10. The table of electrolytes from Question 3(a) identifies strong acids as strong electrolytes. What are the
strong acids?
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11. Write a dissociation equation for the following strong and weak acids.
STRONG ACIDS:
(a) HCl(aq)
(b) HNO3(aq)
(c) H2SO4(aq)
WEAK ACIDS:
(a) HF(aq)
(b) HNO2(aq)
(c) H2SO3(aq)
12. All the strong bases are ionic compounds and, therefore, strong electrolytes. What are the strong bases?
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13. Write a dissociation equation for the following strong and weak Bases.
STRONG BASES:
(a) LiOH(s)
(b) Ca(OH)2(s)
WEAK BASES:
(a) Mg(OH)2(s)
(b) Sr(OH)3(s)
14. The ammonium polyatomic ion, NH4+(aq), dissociates weakly to increase the [H+] in aqueous solution.
Write an equation to show the dissociation of the ammonium polyatomic ion.
15. The ammonia molecule, NH3(aq), reacts in an equilibrium reaction with water to increase the [OH−] in
aqueous solution. Write an equation to show the dissociation of the ammonia molecule.
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ACID NOMENCLATURE
16.
(a) What is a binary acid?
(b) How are binary acids named?
17. What are the common binary acids?
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18.
(a) What is an oxy-acids?
(b) How are oxy-acids named?
19. What are the “trendsetter” oxy-acids?
Polyatomic
Anion
Polyatomic
Name
Acid
Name
Chemical
Formula
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20. How can the “Trendsetter” oxy-acids be changed?
EXAMPLE
Change Made
Change in Name
Name
Formula
21. Practice changing the name or formula of the trendsetters
Acid
Name
a)
Chemical
Formula
H3PO3
b) sulfurous acid
c) nitrous acid
d)
H3PO2
e)
H3CO2
f) pernitric acid
g) hyposulfurous acid
h)
i)
H2CrO3
Permanganous acid
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PRACTICE QUESTIONS
22. Identify each of the following compounds as either and acid (A) or a base (B).
a. NaOH
d. H3PO4
g. HNO3
j. Cu(OH)2
b. HCl
e. Al(OH)3
h. Ca(OH)2
k. Ba(OH)2
c. HCN
f. KOH
i. LiOH
l. HI
23. Write dissociation equations for each of the following acids or bases. Keep in mind whether or not it is a
strong or weak electrolyte.
a) barium hydroxide
b) nitrous acid
c) aluminum hydroxide
d) lead (IV) hydroxide
e) calcium hydroxide
f) lithium hydroxide
g) chloric acid
h) copper (II) hydroxide
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24. Name each of the following as an acid (A) or a base (B):
a. hydrochloric
e. sulfurous
j. potassium hydroxide
b. calcium hydroxide
f. lithium hydroxide
k. ammonium
c. carbonic
h. aluminum hydroxide
l. ammonia
d. nitric
i. hydrobromic
25. Write chemical formulas for each of the following and classify each as an acid (A) or a base (B):
Chemical
Formula
Acid/
Base
a) magnesium hydroxide
b) hydrofluoric
c) nitric acid
d) lithium hydroxide
e) ammonium hydroxide
f) chromic acid
g) barium hydroxide
26. Write the chemical formula for each of the following and then identify each of the following as a strong
electrolyte (SE), weak electrolyte (WE), or nonelecrtrolyte (NE). The solubility chart would be helpful!
Chemical
Formula
Electrolyte
(a) potassium hydroxide
(b) sodium carbonate
(c) silver chloride
(d) dinitrogen pentoxide
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