| 1. What is the pH of a 0.01 M HCl solution?
a. -1
b. 0
c. 1
d. 2
e. 3
2. What is the OH- concentration (molarity) of a solution that contains 5 x 10-3 mole of H+ per liter?
a. 7.00 x 10-14 M
b. 1.00 x 10-12 M
c. 2.00 x 10-12 M
d. 1.00 x 10-11 M
e. 2.00 x 10-11 M
3. Which of the following names is not associated with acid-base theory
a. Dalton
b. Arrhenius
c. Bronsted
d. Lowry
e. Lewis
4. Given the following equation, identify the conjugate acidNH3(g) + H2O (l) → NH4+ (aq) + OH-(aq)
a. NH3
b. H2O
c. NH4+
d. OH-
e. H+
5. The process of determining the concentration of an acid by adding a base is called which of the following?
a. endothermy
b. titration
c. neutralization
d. equivalence
e. none of the above
6. You must have which of the following to reach the equivalence point in the reaction between hydrochloric acid and magnesium hydroxide?
a. 1 mol HCl and 1 mol Mg(OH}2
b. 2 mol HCl and 2 mol Mg(OH)2
c. 2 mol HCl and 1 mol Mg(OH)2
d. 1 mol HCl and 2 mol Mg(OH)2
e. none of the above
7. Which of the following metals will not form a strong base?
a. Sodium
b. Lithium
c. Rubidium
d. Cesium
e. Scandium
8. Which of the following would not be considered a strong acid?
a. sulfuric acid
b. acetic acid
c. nitric acid
d. hydrochloric acid
e. perchloric acid
9. Titrating a solution of 25 mL NaOH requires 42.5 mL of a 0.225M HCl solution. What is the molarity of the basic solution?
a. 0.5882 M
b. 0.1324 M
c. 2.6140 M
d. 0.3825 M
e. none of the above
10. Which of the following is not an acid?
a. battery acid
b. lemon juice
c. Draino
d. tomato juice
e. orange juice
11. Calculate the pH of a 0.70 M solution of HF. (HF has a Ka of 7.2 x 10-4)
a. 4.87
b. 3.14
c. 2.33
d. 1.65
e. 1.57
12. Which of the following is true about the pH of a solution of sulfuric acid?
a. If the solution is dilute the pH is not able to be calculated.
b. If the solution is dilute the pH is completely controlled py the first dissociation.
c. If the solution is dilute the pH is completely controlled Py the second dissociation.
d. If the solution is concentrated the pH is partially controlled Py the second dissociation.
e. If the solution is dilute the pH is partially controlled Py the second dissociation.
13. What is the pH of a 0.45 M KCl solution?
a. 10.5
b. 7.0
c. 9.2
d. 1.4
e. 4.5
14. Which of the following is not true for a solution at 25°C that has a hydroxide concentration of 2.5 x 10-6 M?
a. Kw = 1 x 10-14
b. The solution is acidic
c. The solution is basic
d. The [H+] is 4 x 10-9 M
e. The Kw is independent of what the solution contains
15. A solution is made that is 1.2 x 10-3 M NaOH. What is the pH of this solution?
a. 1.66
b. 2.92
c. 3.12
d. 11.08
e. 12.34
16. Which of the following is the [H+] of a solution which has a pH of 9.7?
a. 2.0 x 10-10 M
b. 5.0 x 10-5 M
c. 3.6 x 10-9 M
d. 9.7 x 10-9 M
e. 6.3 x 10-10 M
17. Calculate the pH of 0.250 M HN03 (aq).
a. 0.60
b. 2.50
c. 12.0
d. 1.20
e. 13.4
18. Acetic acid (HC2H3O2) is a weak acid (Ka = 1.8 x 10-5). Calculate the pH of a 17.6 M HC2H3O2 solution.
a. 4.3
b. 6.4
c. 1.7
d. 0.97
e. 7.4
19. Determine the molarity of a solution of the weak acid HClO2 (Ka = 1.10 x 10-2) if it has a pH of 1.25.
a. 0.287 M
b. 1.23 M
c. 0.819 M
d. 3.17 M
e. 1.52 M
20. Name the conjugate base in the following reaction: HC2H502 + H20 → H30+ + C2H502-
a. acetic acid
b. water
c. hydronium ion
d. acetate ion
e. none of the above
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