Ch. 19 Chemistry Exam Review
Ch. 19 Chemistry Exam Review
Ch. 19 Chemistry Exam Review
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<strong>Ch</strong>. <strong>19</strong> <strong>Ch</strong>emistry <strong>Exam</strong> <strong>Review</strong><br />
1. When an acid reacts with a base, what compounds are typically formed?<br />
2. What is the name of H3PO4?<br />
3. List the general properties of acids. List the three common strong acids.<br />
4. List the general properties of bases.<br />
5. What qualifies a base as an Arrhenius base?<br />
6. Explain the difference between monoprotic, diprotic, and triprotic acids.<br />
7. In the reaction CO + H O HCO + OH , water is acting as a(n) ____.<br />
a. Arrhenius base b. Arrhenius acid c. Brønsted-Lowry base d. Brønsted-Lowry acid<br />
8. What is amphoterism? What is a common substance that exhibits amphoterism?<br />
9. What are the bases in the following equilibrium reaction (according to Bronsted-Lowery)?<br />
CN + H O HCN + OH<br />
10. Will a solution with a hydroxide-ion concentration of 1 10 -9 M be acidic, basic or neutral?<br />
11. Which of these solutions is the most acidic?<br />
a. [H ] = 1 10 M b. [OH ] = 1 10 M c. [H ] = 1 10 M d. [OH ] = 1 10 M<br />
12. Acetic acid ionizes in water as follows:<br />
Fewer than 1% of acetic acid molecules are ionized at any instant. The acetic acid (CH COOH) is therefore<br />
____. The acetate ion (CH3COO - ) would be described as_______.<br />
a. a poor hydrogen-ion acceptor b. a good hydrogen-ion acceptor c. a poor hydrogen-ion donor d. a good<br />
hydrogen-ion donor<br />
13. A 0.12M solution of an acid that ionizes only slightly in solution would be termed ____.
14. Which of the following pairs consists of a strong acid and a weak base?<br />
a. sulfuric acid, sodium hydroxide b. acetic acid, ammonia c. acetic acid, sodium hydroxide d. nitric acid,<br />
ammonia<br />
15. How is Ka calculated? What is the significance of Ka?<br />
16. The K of carbonic acid is 4.3 10 .<br />
H CO H + HCO<br />
This means that H CO is a ____.<br />
a. good hydrogen-ion acceptor b. poor hydrogen-ion acceptor c. good hydrogen-ion donor d. poor<br />
hydrogen-ion donor<br />
17. How can a base be strong, but never concentrated?<br />
18. How many moles of H2SO4 are required to neutralize 2.4 mol NaOH?<br />
<strong>19</strong>. Calculate the molarity of an HCl solution if 45.0 mL of the solution is neutralized by 15.5 mL of 0.600 M<br />
NaOH.<br />
20. What is a buffer made from?<br />
21. What is the hydroxide ion concentration in a solution that has a pH of 6.52?<br />
22. What is the molarity of an H2SO4 solution if 55.0 mL of the solution reacts completely with 0.365 g CaCO3?<br />
23. What is the pH of a solution that has a hydroxide ion concentration of 2.5 x 10 -6 ?<br />
24. What will be produced when calcium hydroxide reacts with hydrochloric acid?<br />
25. The pH of a 0.500 M HNO2 solution is 3.25. What is the Ka of this acid?
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