ACIDS and BASES PRACTICE TEST
Acids and Bases Practice Test - page 1
1. For a solution to be classified as acidic, the hydrogen-ion concentration must be greater than ______.
2. A solution in which the hydroxide-ion concentration is 1 x 10-4Mis (acidic, basic or neutral).
3. In the reaction CO32-+ H2O ↔ HCO3- + OH- the carbonate ion is acting as a Bronsted-Lowry (acid or base).
4. A 0.12 M solution of an acid that ionizes only slightly in solution would be termed (concentrated or dilute) and (weak or strong).
5. A solution in which the hydroxide-ion concentration is 1 x 10-8M is (acidic, basic or neutral).
6. The products of the self-ionization of water are _____.
7. Rain is called acid rain when the pH is less than ______.
8. In a neutral solution, what is the concentration (molarity) of H+?
9. During an acid-base titration, a very rapid change in pH will take place at the _____ point.
10. List the 6 strong acids.
11. In NH4+ + H2O ↔NH3 + H3O+, water is acting as a Bronsted-Lowry (acid or base).
12. With solutions of “strong” acids and “strong” bases, the word “strong” refers to _____.
13. According to the Bronsted-Lowry theory, an acid is a _____ donor.
14. An acid-base titration is carried out by monitoring the _____.
15. What is a monoprotic acid?
16. A 12.0 M solution of an acid that ionizes completely in solution would be termed (concentrated or dilute) and (weak or strong).
17. What is the Bronsted-Lowry acid in the reaction? CN- + H2O ↔ HCN + OH-
18. Acids taste _____.
19. Acids generally release H2 gas when they react with _____.
20. Acids make pH paper turn ______.
21. Acids react with bases to produce _____ and _____.
22. Hydroxides of Group 1 metals are (weak or strong) bases.
23. Name the following ternary acids:
a) H2SO4b) HC2H3O2
c) HClO3d) HClO4
24. A binary acid contains hydrogen and an anion whose name ends in ______.
25. What is the basic assumption in the Arrhenius theory in terms of conducting electricity?
26. A substance that ionizes nearly completely in aqueous solutions and produces H3O+ is a (weak or strong) acid.
27. Name the following binary acids.
a) HClb) H2Sec) HFd) HCN
28. Bases feel _____.
29. What is the most common weak base that is used in household cleaning?
30. Define Arrhenius base.
31. Acid rain is caused by which of the oxides?
Acids and Bases Practice Test - page 1
Figure AFigure B
32.Use Figure A above to answer the following question. Which indicator is best to show an equivalence point pH of 4?
33. Use Figure B above to answer the following question. The titration curve above represents a ______titrated with a ______.
a) weak acid, strong baseb) strong base, strong acid
c) strong base, weak acidd) strong acid, strong base
Acids and Bases Practice Test - page 1
Please show work for the following.
34. What is [H3O+] of a solution whose pH is 4.00?
35. What is the pH of each solution?
a) [OH-] = 1.0 x 10-10 M
b) [H+] = 1.00 x 10-9M c) pOH = 13.4
36. If the [H+] in a solution is 1.34 x 10-1M then calculate [OH-].
37. If 114 mL of 0.00804 M NaOH titrates 118 mL of H3PO4 solution, what is the molarity of the H3PO4 solution?
3NaOH + H3PO4 Na3PO4 + 3H2O
38. Calculate the moles of a Ba(OH)2 solution if it is completely titrated by
261 mL of 0.505 M HNO3.
Ba(OH)2 + 2HNO3 Ba(NO3)2 + 2H2O
39. Calculate the moles of a HClO3solution if it is completely titrated with 0.0582 moles of Ba(OH)2.
Ba(OH)2 + 2HClO3 Ba(ClO3)2 + 2H2O
40. How many mL of 1.20 M HCl can you make from 350. mL of 6.00 M HCl?
41. What is the hydroxide ion concentration of a solution whose pH is 8.25?
42. What is the pOH of a solution in which
a) [OH-] = 3.65 x 10-11M?
b) [H+] = 5.00 x 10-4 M?c) pH = 3.33
43. If [OH-] =3.88 x 10-3 Mcalculate [H+].
44. If 34.2 mL of 0.850 M Ca(OH)2 completely titrates a 57.0 mL solution of HNO3 solution, what is the molarity of the HNO3 solution?
Ca(OH)2 + 2HNO3 Ca(NO3)2 + 2H2O
45. You have 270. mL of 8.00 M NaOH. How many milliliters of 3.20 M NaOH can be made?
46. How many milliliters of water must be added to 12.5 mL of a 3.00 M solution in order to dilute it to 2.00 M?
Acids and Bases Practice Test - page 1