Honors Chapter 19 Review

Honors Chapter 19 Review
Acids and Bases
1. Determine the pH of the following solutions:
a. A 4.5 x 10-3 M HBr solution.
b. A 3.67 x 10-5 M KOH solution.
c. A solution made by diluting 25 mL of 6.0M HCl until the final volume of the solution is 1.75 L.
d. 5 L of an aqueous solution that contains 1.0 grams of HBr and 1.0 grams of nitric acid.
2. What are the pOHs for the solutions in problem 1?
a. ____________________________
b. ____________________________
c. ____________________________
d. ____________________________
3. Which of the following pHs would be the strongest acid?
a. pH 6
b. pH 8
c. pH 13
4. A neutralization reaction forms:
5. Pure water is neutral because:
6. The Arrhenius Model states:
7. The Bronsted-Lowry Model states:
8. What is the molarity of 100 mL of an unknown base if it can be titrated and neutralized with 85 mL of 2M
9. What is the molarity of 71 g of Ca3(PO4)2 dissolved in 925 mL of water?
For questions 10-17, identify each of the solutions as ACIDIC, BASIC, or NEUTRAL:
10. HCl
11. pH=4.3
12. Orange juice
13. pOH = 8.7
14. NaOH
15. Distilled water
16. [H+] = 1x10-4 M
17. H3O+
18. In a titration/neutralization experiment, the indicator is used to:
For questions 19-25, write either the correct name or the correct formula of the acids/bases listed:
19. HNO3
23. NaOH
20. HF
24. Hydrochloric acid
21. HBr
25. Sulfurous acid
22. H2SO4
26. What is the pH of a solution where the pOH = 7.6?
27. In a titration/neutralization experiment, 15 mL of 0.25 M HCl was neutralized by 22.5 mL of a sodium
hydroxide solution of unknown concentration. The concentration of the NaOH was:
28. What is the conjugate acid of HPO4-2?
29. What volume of 0.500M KOH is needed to neutralize 33.3 mL of 0.113M HCl?
30. It takes 43 mL of 2.95M HCl to neutralize 45.7 mL of Ba(OH)2. What is the concentration of the base?
31. Classify the following as Bronsted acids, bases, or both.
a. H2O
b. OH-
c. NH3
d. NH4+
e. NH-2
f. CO3-2
32. What is the conjugate base of the following acids?
a. HClO4
b. NH4+
c. H2O
d. HCO3-
33. What is the conjugate acid of the following bases?
a. CN-
b. SO4-2
c. H2O
d. HCO3-
34. Calculate the pH of the solution formed when 100 mL of 1.00 M HCl is added to 1.00 L of water.
35. Calculate the pH of the following solution of strong acids and bases:
a. 0.001M HCl
b. 0.76 M KOH
c. 2.8 x 10-4M Ba(OH)2