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MR. SURRETTE
VAN NUYS HIGH SCHOOL
CHAPTER 12: ACIDS and BASES
WORKSHEET SOLUTIONS
1. The hydronium ion is:
1A. H3O+
2. Ammonia + water  _____ + hydroxide.
2A. NH4+
3. Kw =
3A. 10-14
4. Acids that have one hydrogen atom that dissociates in water are called:
4A. monoprotic
5. __________ defined acids as substances that donate protons.
5A. Bronsted-Lowry
6. The hydronium ion concentration is the same as the hydroxide ion concentration in __________
solutions.
6A. neutral
7. The hydronium ion concentration is less than the hydroxide ion concentration in __________
solutions.
7A. basic
8. Acid + base  salt + water. This reaction is an example of:
8A. neutralization
9. __________ defined acids as substances that produce H+ when dissolved in water.
9A. Arrhenius
10. A sample of pond water has a pH value of 5. This makes the pond water:
10A. acidic
11.
(A)
(B)
(C)
(D)
HNO3 is a __________ acid.
strong
monoprotic
single hydrogen
all of these
12.
(A)
(B)
(C)
(D)
All of the following are polyprotic acids except:
hydrochloric
phosphoric
sulfuric
carbonic
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CHEMISTRY
MR. SURRETTE
VAN NUYS HIGH SCHOOL
13. Sodium hydroxide is added to pure water. The water will become:
13A. basic
14. Complete the following reaction: sulfuric acid + potassium hydroxide 
14A.
(1) Identify the reactants
(2) Sulfuric acid = H2SO4
(3) Potassium hydroxide = KOH
(4) Identify the ions of the reactants
(5) H2SO4 = 2 H+ + SO4-2
(6) KOH = K+ + OH(7) Swap opposite charges:
(H+ + OH-) + (K+ + SO4-2)
(8) Determine the products: H2O + K2SO4
(9) Write a skeletal equation:
__ H2SO4 + __ KOH  __ K2SO4 + __ H2O
(10) Balance the skeletal equation:
H2SO4 + 2 KOH  K2SO4 + 2 H2O
(11) Determine if the K2SO4 product is soluble or insoluble.
(12) According to the solubility table: K2SO4 is soluble.
(13) Final Equation:
H2SO4(aq) + 2 KOH (aq)  K2SO4(aq) + 2 H2O (l)
15. Complete the following unbalanced reaction: HCl(g) + H2O(l) 
15A. HCl(g) + H2O(l)  H3O+(aq) + Cl-(aq)
16. Write the chemical equation that describes what happens when potassium hydroxide dissolves in
water.
16A. KOH(aq)  K+(aq) + HO-(aq)
17. Predict the chemical equation for ammonia dissolved in water.
17A. NH3(aq) + H2O(l)   NH4+(aq) + HO-(aq)
18. What is the concentration of hydronium ions in a solution if the concentration of hydroxide ions is
1.0 x 10-13 M?
18A.
(1) [H3O+] [HO-] = Kw
(2) [H3O+] = Kw / [HO-]
(3) [H3O+] = (1.0 x 10-14) / (1.0 x 10-13)
(4) [H3O+] = 1.0 x 10-1 M
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CHEMISTRY
MR. SURRETTE
VAN NUYS HIGH SCHOOL
19. What is the pH of a solution that contains 1.0 x 10-11 M hydronium ions?
19A.
(1) pH = - log[H3O+]
(2) pH = - log (1.0 x 10-11)
(3) pH = 11
20. Write chemical equations that describe the dissociation of sulfuric acid in water.
20A.
First hydrogen:
H2SO4(aq) + H2O(l)  H3O+(aq) + HSO4-(aq)
Second hydrogen:
HSO4-(aq) + H2O(l)   H3O+(aq) + SO42-(aq)
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CHEMISTRY
MR. SURRETTE
VAN NUYS HIGH SCHOOL
CHAPTER 12: ACIDS and BASES
QUIZ SOLUTIONS
1. __________ defined bases as substances that produce OH- when dissolved in water.
1A. Arrhenius
2. The hydronium ion is:
2A. H3O+
3. Acids that have one hydrogen atom that dissociates in water are called:
3A. monoprotic
4. HNO3 is a __________ acid.
(A) strong
(B) monoprotic
(C) single hydrogen
(D) all of these
5. All of the following are monoprotic acids except:
5A. Carbonic
6. __________ defined bases as substances that accept protons.
6A. Bronsted-Lowry
7. Kw =
7A. 10-14
8. The hydronium ion concentration is greater than the hydroxide ion concentration in __________
solutions.
8A. acidic
9. The hydronium ion concentration is less than the hydroxide ion concentration in __________
solutions.
9A. basic
10. A solution has a pH value of 12. This makes the solution:
10A. basic
11. Sodium hydroxide is added to pure water. The water will become:
11A. basic
12. HClO3 is added to pure water. The water will become:
12A. acidic
13. Pure H2O has a pH value of:
13A. 7
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CHEMISTRY
MR. SURRETTE
VAN NUYS HIGH SCHOOL
14. Complete the following reaction: sulfuric acid + sodium hydroxide 
14A.
(1) Identify the reactants
(2) Sulfuric acid = H2SO4
(3) Sodium hydroxide = NaOH
(4) Identify the ions of the reactants
(5) H2SO4 = 2 H+ + SO4-2
(6) NaOH = Na+ + OH(7) Swap opposite charges:
(H+ + OH-) + (Na+ + SO4-2)
(8) Determine the products: H2O + Na2SO4
(9) Write a skeletal equation:
__ H2SO4 + __ NaOH  __ Na2SO4 + __ H2O
(10) Balance the skeletal equation:
H2SO4 + 2 NaOH  Na2SO4 + 2 H2O
(11) Determine if the Na2SO4 product is soluble or insoluble.
(12) According to the solubility table: Na2SO4 is soluble.
(13) Final Equation:
H2SO4(aq) + 2 NaOH(aq)  Na2SO4(aq) + 2 H2O(l)
15. Complete the following unbalanced reaction: HNO3(aq) + H2O(l) 
15A. HNO3(aq) + H2O(l)  H3O+(aq) + NO3-(aq)
16. Write the chemical equation that describes what happens when sodium hydroxide is stirred into
water.
16A. NaOH(aq)  Na+(aq) + HO-(aq)
17. Predict the chemical equation for ammonia dissolved in water.
17A. NH3(aq) + H2O(l)   NH4+(aq) + HO- (aq)
18. What is the concentration of hydroxide ions in a solution if the concentration of hydronium ions is
1.0 x 10-11 M?
18A.
(1) [H3O+] [HO-] = Kw
(2) [OH-] = Kw / [H3O+]
(3) [OH-] = (1.0 x 10-14) / (1.0 x 10-11)
(4) [HO-] = 1.0 x 10-3 M
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CHEMISTRY
MR. SURRETTE
VAN NUYS HIGH SCHOOL
19. What is the pH of a solution that contains 1.0 x 10-4 M hydronium ions?
19A.
(1) pH = - log[H3O+]
(2) pH = - log (1.0 x 10-4)
(3) pH = 4
20. Write chemical equations that describe the dissociation of carbonic acid in water.
20A. Carbonic acid is a reaction intermediate: H2CO3(aq)  CO2(g) + H2O(l)
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CHEMISTRY