______ pts. out of 100 possible pts. = % = Name:

Advanced Chemistry: Test #7 (Acid/Base Chemistry)

Multiple Choice: Circle the letter of the best answer for each of the following.  (2 pts. each)

1. Which of the choices shown below is the conjugate base of a bicarbonate ion?

a. OH^-

b. H₂CO₃

c. Na⁺

d. CO₃^-2

e. None of the above; the bicarbonate ion cannot have a conjugate base

2. What is the pH of a 0.1 molar solution of NH₄OH?

a. 1

b. between 1 and 7

c. 7

d. between 7 and 13

e. 13

3. What is the pH of a 0.1 molar solution of C₂H₅OH?

a. 1

b. between 1 and 7

c. 7

d. between 7 and 13

e. 13

4. What is the pH of 0.1 molar KOH?

a. 1

b. between 1 and 7

c. 7

d. between 7 and 13

e. 13

5. What is the pH of 0.1 molar NaBr?

a. 1

b. between 1 and 7

c. 7

d. between 7 and 13

e. 13

6. What is the pH of 0.1 molar NaF?

a. 1

b. between 1 and 7

c. 7

d. between 7 and 13

e. 13

7. What is the pH of 0.1 molar HCOOH?

a. 1

b. between 1 and 7

c. 7

d. between 7 and 13

e. 13

8. What is the pH of 0.1 molar HF?

a. 1

b. between 1 and 7

c. 7

d. between 7 and 13

e. 13

9. What is the pH of 1.00 molar HCl?

a. -1

b. 0

c. 1

d. between 1 and 7

e. 7

10. What is the pH of 0.10 molar HCl?

a. -1

b. 0

c. 1

d. between 1 and 7

e. 7

11. When carbon dioxide reacts with water it forms a weakly acidic solution. The pH of that solution might be:

a. -1

b. 6

c. 7

d. 8

e. 14

12. A difference of how many pH unit(s) makes a one hundred fold difference in the hydrogen ion concentration?

a. 0.01

b. 0.1

c. 1

d. 2

e. 100

13. Complete the following acid/base reactions: (3 pts. each)

a. CO₃^-2 + HS^-

^b. CH₃COOH + BO₃^-3

14. Circle the conjugate base in each of the above reactions. (4 pts.)

15. Identify each of the following as a strong acid (SA), a weak acid (WA), a strong base (SB), a weak base (WB), or neutral (N): (2 pt. each)

a. HBr b. LiOH c. CH₃OH d. NH₄OH ______

e. KCl f. CHOOH g. H₂SO₄ h. HNO₂ ______

16. Write the formula for a hydronium ion. (2 pt.)

17. If a solution with a [H⁺] = 1.0 x 10^-10 M were tested with litmus paper and phenolphthalein, what would the tests show? (2 pt. each)

Litmus = Phenolphthalein =

18. List the following acids from strongest to weakest: phosphoric acid (H₃PO₄), sulfurous acid (H₂SO₃), hydrobromic acid (HBr), and hydroflouric acid (HF). (3 pts.)

19. What is the pH of a 0.050M solution of KOH? (3 pts.)

20. What is the pH of a 0.0020M solution of HNO₃? (3 pts.)

21. What is the pH of a 1.0M solution of NaCl? (3 pts.)

22. 45.7 ml of a 0.30M H₂SO₄ solution is required to neutralize 13.5 ml of a sodium hydroxide solution. What is the concentration of the NaOH solution? (5 pts.)

23. What is the pH of a solution that has been made by dissolving 4.0 g of NaOH into 100.0 ml of distilled water? (5 pts.)

24. What is the hydroxide ion concentration in a solution with a pH of 2.0? (4 pts.)

25. A 0.00150 M solution of Westtownous acid (WtH) has a pH of 6.5. What is the acidity constant for Westtownous acid? (10 pts.)

26. What is the pH of 0.250 M NaBrO (sodium hypobromite)? (8 pts.)