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Unit 14 Review

Unit 14 Review. Acids & Bases. 1. In a titration, when the number of moles of hydrogen ions equals the number of moles of hydroxide ions , what is said to have happened?. A. The end point has been reached B. The equivalence point has been reached C. The titration is perfect

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Unit 14 Review

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  1. Unit 14 Review Acids & Bases

  2. 1. In a titration, when the number of moles of hydrogen ionsequals the number of moles of hydroxide ions, what is said to have happened? A. The end point has been reached B. The equivalence point has been reached C. The titration is perfect D. The equal point has been reached

  3. 2. Which of the following bases is strong? A. Sodium hydroxide B. Magnesium hydroxide C. Ammonia D. Vinegar

  4. 3. When an acid reacts with a base, what compounds are produced? • Acid • Base C. Salt and water D. Two elements

  5. 4. Which type of solution is one with a pH of 8? A. acidic B. basic C. neutral D. None of the above

  6. 5. With solutions of strong acids and strong bases, the word strong refers to ____. A. Molarity B. Molality C. Polarity D. Ionization

  7. 6. Which of the following represents a Bronsted-Lowry conjugate acid-base pair? A. SO32- and SO2 B. NH41+ and NH3 C. CO and COOH D. HCl and NaCl

  8. 7. Which compound can act as both a Bronsted-Lowry acid and a Bronsted-Lowry base? A. Hydrochloric acid B. Sodium hydroxide C. water D. vinegar

  9. 8. What type of acid is phosphoric acid? A. monoprotic B. diprotic C. triprotic D. quadprotic

  10. 9. What is an acid according to Arrhenius? A. A substance that releases H+ when placed in water. B. A substance that releases OH- when placed in water. C. A substance that can conduct electricity at any time. D. A substance that can act as a proton donor and acceptor.

  11. 10. Which of these is an Arrhenius base? A. CH3COOH B. LiOH C. NH3 D. HCl

  12. 11. In a neutral solution, the [H1+] is ____. A. 1 x 107 B. 1 x 10-14 C. 1 x 10-7 D. 1 x 10-1

  13. 12. The acid dissociation constant (Ka) for an acid dissolved in water is equal to the ____ x ____. A. [H+][OH-] B. [H3O+][OH-] C. [H+][HOH-] D. Both A and B

  14. 13. A 0.12 M solution of an acid that ionizes only slightly in solution would be termed ____. A. strong B. weak C. concentrated D. None of the above

  15. 14. What is transferred between a conjugate acid-base pair? A. An oxygen B. A proton C. An electron D. Nothing

  16. 15. What are the acids in the following: CN1- + H2O ↔ HCN + OH1-? A. H2O only B. CN- only C. H2O and HCN D. H2O, CN-, and OH

  17. 16. A Lewis acid is a substance that can ____. A. Accept an electron pair B. Donate an electron pair C. Donate a proton D. Releases H+

  18. 17. The process of adding a known amount of solution of known concentration to determine the concentration of another solution is called ____. A. neutralization B. equalization C. hydrolysis D. titration

  19. 18. If the hydroxide-ion concentration is 1 x 10-12 M, what is the pH of the solution? A. 12 B. 14 C. 2 D. None of the above

  20. 19. What is the hydrogen-ion concentration if the pH is 3.7? A. 1 x 10-4 B. 2 x 10-4 C. 5011 D. 2 x 10-3

  21. 20. What is the pH of a solution with a concentration of 0.01 M HCl? A. 2 B. 4 C. 6 D. 8

  22. 21. If [OH1-] = 1 x 10-4 M, what is the pH of the solution? A. 4 B. 10 C. 14 D. 1

  23. 22. A substance with a large Ka would be considered a A. Strong acid B. Weak acid C. Strong base D. Weak base

  24. 23. During a titration, the indicator changing color indicates that the _____________ has been reached. A. End point B. Equivalence point C. Neutralization point D. All of the above

  25. 24. Which of the following is a property of an acid? A. pH less than 7 B. Sour taste C. [H+] > [OH-] D. All of the above

  26. 25. Which of the following is a property of a base? A. Bitter B. Slippery feel C. [H+] < [OH-] D. All of the above

  27. Answers 1. B 9. A 17. D 2. A 10. B 18. C 3. C 11. C 19. B 4. B 12. D 20. A 5. D 13. B 21. B 6. B 14. B 22. A 7. C 15. C 23. A 8. C 16. A 24. D 25. D

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