practice test acids and bases2 by W5wI9I

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									Acid Base Practice Test
____     1. Acids taste
             a. sweet.                                               c.   bitter.
             b. sour.                                                d.   salty.
____     2. Acids generally release H2 gas when they react with
             a. nonmetals.                                           c.   active metals.
             b. semimetals.                                          d.   inactive metals.
____     3. Acids make litmus paper turn
             a. red.                                                 c.   blue.
             b. yellow.                                              d.   black.
____     4. Bases feel
             a. rough.                                               c.   slippery.
             b. moist.                                               d.   dry.
____     5. Bases react with
             a. acids to produce salts and water.                    c.   water to produce acids and salts.
             b. salts to produce acids and water.                    d.   neither acids, salts, nor water.

____     6. Which of the following is a binary acid?
             a. H2SO4                                                  c. HBr
             b. CH3COOH                                                d. NaOH
____     7. Which of the following is chloric acid?
             a. HClO                                                   c. HClO3
             b. HClO2                                                  d. HClO4
_____    8. Which type of solution is one with a pH of 8?
             a. acidic           b. basic            c. neutral
_____    9. What is the pH when the hydrogen ion concentration is 2 x 10 –3 M
             a. 2       b. 2.7 c. 3        d. ) 3.3 e. 4
_____   10. A solution with a pH of 5.0 _____.
             a. is basic
             b. has a hydrogen-ion concentration of 5.0M
             c. is neutral
             d. has a hydroxide-ion concentration of 1 x 10 –9 M

____    11. The traditional definition of acids is based on the observations of
            a. Brønsted and Lowry.                                       c. Arrhenius.
            b. Lewis.                                                    d. Faraday.
____    12. What is an Arrhenius acid?
            a. a chemical compound that increases the concentration of hydrogen ions in aqueous solution
            b. a chemical compound that increases the concentration of hydroxide ions in aqueous solution
            c. a chemical compound that decreases the concentration of hydrogen ions in aqueous solution
            d. a chemical compound that decreases the concentration of hydroxide ions in aqueous solution
____    13. Which statement about Arrhenius acids is FALSE?
            a. Their water solutions are called aqueous acids.
            b. They are molecular compounds with ionizable hydrogen atoms.
            c. Their pure aqueous solutions are electrolytes.
            d. They increase the concentration of hydroxide ions in aqueous solution.
____    14. A substance that ionizes nearly completely in aqueous solutions and produces H3O+ is a
            a. weak base.                                                c. weak acid.
            b. strong base.                                              d. strong acid.
____    15. Which of the following is a strong acid?
            a. HSO4–                                                     c. CH3COOH
            b. H2SO4                                                     d. H3PO4

____    16. Which of the following is a triprotic acid?
            a. H2SO4                                                  c. HCl
            b. CH3COOH                                                d. H3PO4
____    17. Strong bases are
            a. strong electrolytes.                                   c. nonelectrolytes.
            b. weak electrolytes.                                     d. also strong acids.
____    18. Hydroxides of Group 1 metals
            a. are all strong bases.                                  c. are all acids.
            b. are all weak bases.                                    d. might be either strong or weak bases.
____    19. Whose definition of acids and bases emphasizes the role of protons?
            a. Brønsted and Lowry                                     c. Arrhenius
            b. Lewis                                                  d. Faraday
____    20. A Lewis base is a(n)
            a. producer of OH– ions.                                  c. electron-pair donor.
            b. proton acceptor.                                       d. electron-pair acceptor.
____   21. An electron-pair acceptor is a
           a. Brønsted-Lowry base.                                    c. Lewis base.
           b. Lewis acid.                                             d. traditional acid.
____   22. A species that remains when an acid has lost a proton is a
           a. conjugate base.                                         c. strong base.
           b. conjugate acid.                                         d. strong acid.
____   23. In the reaction HF + H2O H3O+ + F–, a conjugate acid-base pair is
           a. HF and H2O.                                             c. H3O+ and H2O.
                            +
           b. F– and H3O .                                            d. HF and H3O+.
                                                                  –
____   24. In the reaction CH3COOH + H2O            +
                                               H3O + CH3COO , the conjugate base of H3O+ is
           a. H2O.                                                    c. CH3COO–.
           b. CH3COOH.                                                d. not shown.
____   25. In the reaction HSO4– + H2O H3O+ + SO42–, the ion HSO4– acts as a(n)
           a. acid.                                                   c. spectator species.
           b. base.                                                   d. salt.

____   26. In the reaction H3PO4 + H2O H3O+ + H2PO4–, the molecule H2O acts as a(n)
           a. acid.                                                  c. spectator species.
           b. base.                                                  d. salt.
____   27. What is neutralization?
           a. an acid-base reaction that does not include dissocation of ions
           b. a reaction of hydronium ions and hydroxide ions to form a salt
           c. a reaction of hydronium ions and hydroxide ions to form water molecules
           d. a reaction of hydronium ions and hydroxide ions to form water molecules and a salt
____   28. Which compound is produced by a neutralization?
           a. H2O(l)                                                 c. Ca(OH)2(s)
           b. HNO3(aq)                                               d. H3PO4(aq)
____   29. Which of the following gases does NOT dissolve in atmospheric water to produce acidic solutions?
           a. NO                                                     c. O2
           b. NO2                                                    d. CO2
____   30. What is the concentration of H3O+ in pure water?
           a. 10–7 M                                                 c. 55.4 M
           b. 0.7 M                                                  d. 107 M

____   31. If [H3O+] of a solution is less than [OH–], the solution
           a. is always acidic.                                       c. is always neutral.
           b. is always basic.                                        d. might be acidic, basic, or neutral.
____   32. What is the pH of a 10–4 M HCl solution?
           a. 4                                                       c. 8
           b. 6                                                       d. 10
____   33. What is the pH of a 10–5 M KOH solution?
           a. 3                                                       c. 9
           b. 5                                                       d. 11
____   34. If [H3O+] = 8.26  10–5 M, what is the pH of the solution?
           a. 2.161                                                   c. 4.083
           b. 3.912                                                   d. 8.024
____   35. What is the hydroxide ion concentration of a solution whose pH is 12.40?
           a. 2.5  10–2 M                                            c. 8.9  10–2 M
                         –2
           b. 4.4  10 M                                              d. 1.0  10–1 M

____   36. An acid-base titration involves a
           a. composition reaction.                                   c. single-replacement reaction.
           b. neutralization reaction.                                d. decomposition reaction.
____   37. What unknown quantity can be calculated after performing a titration?
           a. volume                                                  c. mass
           b. concentration                                           d. density
____   38. What is the molarity of an HCl solution if 50.0 mL is neutralized in a titration by 40.0 mL of 0.400 M NaOH?
           a. 0.200 M                                                 c. 0.320 M
           b. 0.280 M                                                 d. 0.500 M
____   39. What is the molarity of an H2SO4 solution if 49.0 mL is completely titrated by 68.4 mL of an NaOH solution whose concentration is
           0.333 M?
           a. 0.116 M                                                 c. 0.465 M
           b. 0.232 M                                                 d. 0.880 M
____   40. What is the molarity of a Ba(OH)2 solution if 93.9 mL is completely titrated by 15.3 mL of 0.247 M H 2SO4?
           a. 0.0101 M                                                c. 0.0402 M
           b. 0.0201 M                                                d. 0.0805 M
Acid Base Practice Test
Answer Section

MULTIPLE CHOICE

         1. ANS:      B   DIF:   I     OBJ:   15-1.1

         2. ANS:      C   DIF:   I     OBJ:   15-1.1

         3. ANS:      A   DIF:   I     OBJ:   15-1.1

         4. ANS:      C   DIF:   I     OBJ:   15-1.1

         5. ANS:      A   DIF:   I     OBJ:   15-1.1

         6. ANS:      C   DIF:   II    OBJ:   15-1.2

         7. ANS:      C   DIF:   II    OBJ:   15-1.2

         8. ANS:      B   DIF:   I     OBJ:   15-1.3

         9. ANS:      B   DIF:   I     OBJ:   15-1.3

        10. ANS:      D   DIF:   I     OBJ:   15-1.3

        11. ANS:      C   DIF:   I     OBJ:   15-1.4

        12. ANS:      A   DIF:   I     OBJ:   15-1.4

        13. ANS:      D   DIF:   I     OBJ:   15-1.4

        14. ANS:      D   DIF:   I     OBJ:   15-1.5

        15. ANS:      B   DIF:   II    OBJ:   15-1.5

        16. ANS:      D   DIF:   II    OBJ:   15-1.5

        17. ANS:      A   DIF:   I     OBJ:   15-1.5

        18. ANS:      A   DIF:   I     OBJ:   15-1.5

        19. ANS:      A   DIF:   I     OBJ:   15-2.1

        20. ANS:      C   DIF:   I     OBJ:   15-2.2

        21. ANS:      B   DIF:   I     OBJ:   15-2.2

        22. ANS:      A   DIF:   I     OBJ:   15-3.1

        23. ANS:      C   DIF:   II    OBJ:   15-3.1

        24. ANS:      A   DIF:   II    OBJ:   15-3.1

        25. ANS:      A   DIF:   II    OBJ:   15-3.1

        26. ANS:      B   DIF:   II    OBJ:   15-3.1

        27. ANS:      C   DIF:   I     OBJ:   15-3.2

        28. ANS:      A   DIF:   I     OBJ:   15-3.2

        29. ANS:      C   DIF:   I     OBJ:   15-3.3

        30. ANS:      A   DIF:   I     OBJ:   16-1.1

        31. ANS:      B   DIF:   I     OBJ:   16-1.2

        32. ANS:      A   DIF:   III   OBJ:   16-1.4
33. ANS:   C   DIF:   III   OBJ:   16-1.4

34. ANS:   C   DIF:   III   OBJ:   16-1.4

35. ANS:   A   DIF:   III   OBJ:   16-1.5

36. ANS:   B   DIF:   I     OBJ:   16-2.2

37. ANS:   B   DIF:   I     OBJ:   16-2.2

38. ANS:   C   DIF:   III   OBJ:   16-2.3

39. ANS:   B   DIF:   III   OBJ:   16-2.3

40. ANS:   C   DIF:   III   OBJ:   16-2.3

								
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