Honors Chemistry – Unit 9 Test

1. Acids tastea. bitter b. sour c. sweet d. salty

2. The process of adding a known amount of solution of known concentration to determine the concentration of another solution is calleda. hydrolysis b. titration c. buffer capacity d. neutralization

3. In the reaction represented by the equation H2SO4 + H2O ↔ H3O+ + HSO-4, the ion HSO-

4 acts as a(n)a. spectator species c. conjugate acidb. salt d. conjugate base

4. What is the best description for a solution with a hydroxide-ion concentration of 1 x 10-4M?a. neutral b. basic c. acidic d. the answer can’t be determined

5. In the reaction represented by the equation NH3 + H2O→ NH+4 + OH-, H2O is a(n)

a. Bronsted-Lowry acid c. Arrheniusb. Lewis base d. Bronsted-Lowry base

6. Which expression represents the concentration of H3O+ ions in solution?a. 10-14 – [OH-] c. 10-14 x [OH-]b. 10-14 ÷ [OH-] d. [OH-] ÷ 10-14

7. The substances produced when KOH(aq) neutralizes HCl (aq) area. H3O+ (aq) and KCl (aq) c. KH2O+ (aq) and Cl- (aq)b. H2O (l) and KCl (aq) d. HClO (aq) and KH (aq)

8. What is the pH of a solution whose hydronium ion concentration is 5.03 x 10-1 Ma. 0.5133 b. 0.2984 c. 1.542 d. 5.031

9. The pH of a basic solution isa. < 7 b. > 14 c. > 7 d. < 0

10. Which compound would most likely be produced by a neutralization reactions?a. Ca(OH)2 (s) c. HNO3(aq)b. H3PO4 (aq) d. H2O (l)

11. An amphoteric species is one that reacts as a(n)a. acid only b. base only c. acid or base d. none of these

12. What is the pH of a 10-4 m HCl solution?a. 8 b. 6 c. 4 d. 10

13. If [H3O+] of a solution is greater than [OH-], the solution a. is always basic c. is always acidicb. might be acidic, basic or neutral d. is always neutral

14. An acid ending with the suffix –ic produces an ion with thea. suffix – ate c. suffix – ousb. suffix – ite d. prefix – hydro-

15. In the reaction represented by the equation HClO3 + NH3 ↔ NH+4 + ClO-

3, the conjugate acid of NH3 isa. NH+

4 b. ClO-3 c. not shown d. HClO3

16. What is the acid-ionization expression for the ionization of acetic acid shown in the reaction represented by the equation: CH3COOH (aq) + H2O (l) ↔ H3O+ (aq) + CH3COOH- (aq)a. [CH3COOH] c. [H3O + ] [CH 3COO - ] [H3O+] [CH3COO-] [CH3COOH]

b. [H3O+] [CH3COOH-] d. . [H3O + ] [CH 3COO - ] [CH3COOH] [H2O]

17. Which is a Lewis acid but not a Bronsted Lowry acid?a. HCl b. NH3 c. BF3 d. none of these

18. When titrating a strong acid with a strong base, the equivalence point a. will be above a pH of 7.0 c. will be below a pH of 7.0b. will be either a above or below a pH of 7.0 d. will be at a pH of 7.0

19. Which of the following is a triprotic acid?a. H2SO4 b. CH3COOH c. HCl d. H3PO4

20. In a titration, when the number of moles of hydrogen ions equals the number of moles of a hydroxide ions, what is said to have happened a. the titration has failed c. the equivalence point has been reachedb. the ionization constant has reached a value of 1 d. the end point has been reached

21. Which quantity is directly measured in titration?a. density b. concentration c. volume d. mass

22. Bases react witha. salts to produce acids and water c. water to produce acids and saltsb. acids to produce salts and water d. neither acids, salts nor water

23. A Lewis acid isa. a proton acceptor c. an electron-pair acceptorb. a proton donor d. an electron-pair donor

24. A Bronsted Lowry base isa. electron-pair donor c. electron-pair acceptorb. hydrogen ion acceptor d. producer of OH- ions

25.