# ATOMIC PHYSICS WORKSHEET - DOC

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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.   HNO3 is a __________ acid.
(A)   strong
(B)   monoprotic
(C)   single hydrogen
(D)   all of these

CHEMISTRY                                                                                   PAGE 1
MR. SURRETTE                                                           VAN NUYS HIGH SCHOOL

12.   All of the following are polyprotic acids except:
(A)   hydrochloric
(B)   phosphoric
(C)   sulfuric
(D)   carbonic

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)

CHEMISTRY                                                                                   PAGE 2
MR. SURRETTE                                                               VAN NUYS HIGH SCHOOL

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

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)

CHEMISTRY                                                                                       PAGE 3
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:
basic

12. HClO3 is added to pure water. The water will become:
acidic

CHEMISTRY                                                                                   PAGE 4
MR. SURRETTE                                                              VAN NUYS HIGH SCHOOL

13. Pure H2O has a pH value of:
7

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-
(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

CHEMISTRY                                                                                       PAGE 5
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)

CHEMISTRY                                                                                PAGE 6

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