Basic Chemistry, 4/e Chapter 14: Acids and Bases

1. Basic Chemistry, 4/eChapter 14: Acids and Bases Karen Timberlake

2. Chapter 14 – Acids and Bases 1. All of the following are strong acids except A. sulfuric acid. B. nitric acid. C. hydrochloric acid. D. acetic acid.

3. Chapter 14 – Acids and Bases 1. All of the following are strong acids except A. sulfuric acid. B. nitric acid. C. hydrochloric acid. D. acetic acid.

4. Chapter 14 – Acids and Bases 2. All of the following are strong bases except A. sodium hydroxide. B. calcium hydroxide. C. aluminum hydroxide. D. potassium hydroxide.

5. Chapter 14 – Acids and Bases 2. All of the following are strong bases except A. sodium hydroxide. B. calcium hydroxide. C. aluminum hydroxide. D. potassium hydroxide.

6. Chapter 14 – Acids and Bases 3. Which of the following juices is least acidic? A. Tomato B. Apple C. Orange D. Lemon

7. Chapter 14 – Acids and Bases 3. Which of the following juices is least acidic? A. Tomato B. Apple C. Orange D. Lemon

8. Chapter 14 – Acids and Bases 4. Which of the following metals does not react with an acid? A. Calcium B. Copper C. Magnesium D. Zinc

9. Chapter 14 – Acids and Bases 4. Which of the following metals does not react with an acid? A. Calcium B. Copper C. Magnesium D. Zinc

10. Chapter 14 – Acids and Bases 5. Determine the Ka for an acid HX if the pH of a 0.100 M solution of HX is 4.5. A. 1.0 × 10–8 B. 3.0 × 10–7 C. 2.5 × 10–8 D. 4.5 × 10–9

11. Chapter 14 – Acids and Bases 5. Determine the Ka for an acid HX if the pH of a 0.100 M solution of HX is 4.5. A. 1.0 × 10–8 B. 3.0 × 10–7 C. 2.5 × 10–8 D. 4.5 × 10–9

12. Chapter 14 – Acids and Bases 6. Determine the Ka for an acid HX if the [H+] of a 0.200 M solution of HX is 0.00003 M. A. 3.0 × 10–9 B. 4.5 × 10–9 C. 3.0 × 10–7 D. 2.5 × 10–7

13. Chapter 14 – Acids and Bases 6. Determine the Ka for an acid HX if the [H+] of a 0.200 M solution of HX is 0.00003 M. A. 3.0 × 10–9 B. 4.5 × 10–9 C. 3.0 × 10–7 D. 2.5 × 10–7

14. Chapter 14 – Acids and Bases 7. The [H+] of a 1.0 M acetic acid (Ka = 1.8 × 10–5) solution is A. 1.0 M. B. 0.3 M. C. 0.0042 M. D. 1.8 × 10–5 M.

15. Chapter 14 – Acids and Bases 7. The [H+] of a 1.0 M acetic acid (Ka = 1.8 × 10–5) solution is A. 1.0 M. B. 0.3 M. C. 0.0042 M. D. 1.8 × 10–5 M.

16. Chapter 14 – Acids and Bases 8. What is the pH of a 0.00167 M HCl solution? A. 0.60 B. 1.67 C. 2.78 D. 3.0

17. Chapter 14 – Acids and Bases 8. What is the pH of a 0.00167 M HCl solution? A. 0.60 B. 1.67 C. 2.78 D. 3.0

18. Chapter 14 – Acids and Bases 9. What is the pH of a 0.04 M KOH solution? A. 9.6 B. 10.4 C. 11.7 D. 12.6

19. Chapter 14 – Acids and Bases 9. What is the pH of a 0.04 M KOH solution? A. 9.6 B. 10.4 C. 11.7 D. 12.6

20. Chapter 14 – Acids and Bases 10. What is the [H+] of a solution at pH 3.5? A. 5.3 × 10–5 B. 6.0 × 10–4 C. 3.16 × 10–4 D. 8.84 × 10–3

21. Chapter 14 – Acids and Bases 10. What is the [H+] of a solution at pH 3.5? A. 5.3 × 10–5 B. 6.0 × 10–4 C. 3.16 × 10-4 D. 8.84 × 10–3

22. Chapter 14 – Acids and Bases 11. What is the [OH–] concentration of a solution at pH 4.0? A. 4 M B. 10–4 M C. 10 M D. 10–10 M

23. Chapter 14 – Acids and Bases 11. What is the [OH–] concentration of a solution at pH 4.0? A. 4 M B. 10–4 M C. 10 M D. 10–10 M

24. Chapter 14 – Acids and Bases 12. A student titrated 15.0 mL of an unknown acid solution with 25.0 mL of a 0.100 M KOH solution. What is the molarity of the unknown acid? A. 0.115 M B. 0.126 M C. 0.150 M D. 0.167 M

25. Chapter 14 – Acids and Bases 12. A student titrated 15.0 mL of an unknown acid solution with 25.0 mL of a 0.100 M KOH solution. What is the molarity of the unknown acid? A. 0.115 M B. 0.126 M C. 0.150 M D. 0.167 M

26. Chapter 14 – Acids and Bases 13. A student titrated 20.0 mL of an unknown acid solution with 32.4 mL of a 0.115 M KOH solution. What is the molarity of the unknown acid? A. 0.153 M B. 0.186 M C. 0.224 M D. 0.347 M

27. Chapter 14 – Acids and Bases 13. A student titrated 20.0 mL of an unknown acid solution with 32.4 mL of a 0.115 M KOH solution. What is the molarity of the unknown acid? A. 0.153 M B. 0.186 M C. 0.224 M D. 0.347 M

28. Chapter 14 – Acids and Bases 14. Which of the following statements best describes a buffer? A. An acid on the product side of an equation describing an acid–base reaction. B. A solution that contains substantial amounts of both a weak acid and its conjugate base and resists changes in pH. C. A base on the product side of an equation describing an acid–base reaction. D. Any substance that can act as an acid or base, depending on the nature of the solution.

29. Chapter 14 – Acids and Bases 14. Which of the following statements best describes a buffer? A. An acid on the product side of an equation describing an acid–base reaction. B. A solution that contains substantial amounts of both a weak acid and its conjugate base and resists changes in pH. C. A base on the product side of an equation describing an acid–base reaction. D. Any substance that can act as an acid or base, depending on the nature of the solution.

30. Chapter 14 – Acids and Bases 15. Which of these buffers, according to your text, plays an important role in stabilizing the pH of the blood? A. CH3COOH/CH3COO– B. H2PO4–/HPO42– C. H2SO4/HSO4– D. H2CO3/HCO3–

31. Chapter 14 – Acids and Bases 15. Which of these buffers, according to your text, plays an important role in stabilizing the pH of the blood? A. CH3COOH/CH3COO– B. H2PO4–/HPO42– C. H2SO4/HSO4– D. H2CO3/HCO3–