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Chemistry 121 – Chemistry in the Modern World
Weekly Worksheet 5
Directions: Answer the following questions using your textbook. Remember, these are the types of questions that will be on the proctored exam. Create a separate Word document listing the correct answers and submit it in the Assignments folder. Use as a title your name and the week number. For example, I would call this assignment Matton5. Each question is worth 1 or 2 points, for a total of 40 points.
1. Chapter 6, Question 7c (2 points)
2. Chapter 6, Question 9b (2 points)
3. Chapter 6, Question 10a
4. Chapter 6, Question 10b
5. Chapter 6, Question 11a (2 points)
6. Chapter 6, Question 12b (2 points)
7. Chapter 6, Question13b
8. Chapter 6, Question 13c
9. Chapter 6, Question 14a
10. Chapter 6, Question 14b
11. Chapter 6, Question 14c
12. Chapter 6, Question 14d
13. Chapter 6, Question 14e
14. Chapter 6, Question 14f
15. Chapter 6, Question 14g
16. Chapter 6, Question 28
1. Which is NOT a characteristic of acids?
a. taste bitter
b. turn litmus red
c. react with bases to form salts
d. react with metal to form hydrogen gas
2. Lemon juice has a sour taste and turns litmus to red. Lemon juice is,
a. basic.
b. acidic.
c. neutral.
d. caustic.
3. Many medicines have a bitter taste which manufacturers attempt to disguise. These medicines are probably,
a. acids.
b. bases.
c. salts.
d. neutral.
4. A hydrogen ion, H+, is the same as a(n),
a. hydronium ion.
b. proton.
c. electron.
d. hydrate.
5. Which one of the following is a hydroxide ion?
a. OH-
b. H+
c. H3O+
d. H2O-
6. The same number of moles of acetic acid and hydrogen chloride are placed in beakers containing water. After this addition, the beaker with the HCl has more hydronium ions than the beaker with added acetic acid. HCl is classified as,
a. a weaker acid than acetic acid.
b. a stronger acid than acetic acid.
c. equal in acid strength to acetic acid.
d. a base.
7. HCN is classified as a very weak acid in water. This means that it produces,
a. no hydronium ions.
b. a relatively small fraction of the maximum number of possible hydronium ions.
c. a relatively large fraction of the maximum number of possible hydronium ions.
d. 100% of the maximum number of possible hydronium ions.
8. When an aqueous solution containing hydrochloric acid is just neutralized with an aqueous solution containing sodium hydroxide, the solution would taste (don’t try this at home!),
a. sour.
b. bitter.
c. salty.
d. sweet.
9. Which of the following is the correct balanced equation for the neutralization of potassium hydroxide with hydrochloric acid?
a. KOH + HCl ( KCl + H2O
b. KOH + HCl ( ClOH + H2O
c. KOH ( HCl + KCl + H2O
d. KCl + H2O ( HCl + KOH
10. Which of the following is the correct balanced equation for the reaction in water of sulfuric acid, H2SO4, a strong acid?
a. H2SO4 ( H+ + HSO4-
b. H2SO4 ( OH- + HSO4-
c. H+ + HSO4- ( H2SO4
d. OH- + H+ ( H2O
11. Which of the following is the correct balanced equation for the reaction in water of LiOH, a strong base found in alkaline storage batteries?
a. LiOH ( H+ + O- + Li+
b. LiOH ( H2O + Li+
c. LiOH ( Li+ + OH-
d. Li+ + OH- ( LiOH
12. A sample of rainwater has a pH of 3.5. What ion is sure to be present in relatively large concentration in this rain sample?
a. H3O+
b. SO42-
c. OH-
d. HSO4-
13. A solution with a pH of 10 has a hydronium ion concentration of,
a. 10-10 mol/L.
b. 1010 mol/L.
c. 10 mol/L
d. -10 mol/L
14. A solution of toilet bowl cleaner has a pH of 10. The solution is,
a. strongly acidic.
b. weakly acidic.
c. strongly basic.
d. weakly basic.
15. Which substance has the lowest pH?
a. blood
b. lemon juice
c. unpolluted rainwater
d. a concentrated solution of NaOH, sodium hydroxide
16. If the concentration of hydronium ions in a dilute solution of nitric acid is 0.0001M, what is the pH of that solution?
a. 7
b. 14
c. 4
d. 5
17. Which of the following does NOT contribute to acid rain?
a. coal-burning power plants
b. lightning
c. volcanic eruptions
d. none – they all contribute to acid rain.
18. By definition, acid rain has a pH,
a. below 4
b. below 5.6
c. below 7
d. above 8.5
19. All antacids are,
a. acids.
b. bases.
c. neutral.
d. salts.
20. In general, when aqueous solutions of an acid and a base are mixed,
a. a new acid and a salt are formed.
b. a new base and a salt are formed.
c. No reaction occurs.
d. a salt and water are formed.
Week 5:
10. Describe the reactions of nitrogen oxides in the atmosphere. How does this contribute to acid rain? What are the main sources of nitrogen emissions?
And choose one:
1. Consider This 6.23 (page 269) – Reexamine Figure 6.22. Although it may be tempting to blame acid rain for the damage, other agents may be at work. View possible other culprits for yourself by taking a photo tour of our nation’s capitol, courtesy of a website on acid rain provided by the United States Geological Survey. A link is provided at the textbook’s website. What kinds of damage do the photos show? What promotes damage by acid rain? What else has caused the deterioration?
2. Consider This 6.24 (page 270) – The concerns of acid rain vary across the globe. Many countries in North America and Europe have websites dealing with acid rain. Search to locate one or use the links provided at the textbook’s website. What are the issues in the country you selected? Does the acid deposition originate outside the borders of the country?
3. Chapter 6, Question 25 (page 278) – Assuming the ocean continues to acidify at the same rate that it has been over the past 200 years, how long will it take before the ocean actually becomes acidic? What are some possible affects of this? What do you think is the appropriate response?
4. Chapter 6, Question 49 (page 280) – Discuss the validity of the statement, “Photochemical smog is a local issue, acid rain is a regional one, and the enhanced greenhouse effect is a global one.” Briefly describe the chemistry behind each issue. Do you agree that the magnitudes of the problem are really so different in scope? What do you think are the appropriate responses to each issue?
