Perk Learning Lab, MGCCC

Created by Tara L. Moore

 

GENERAL CHEMISTRY,  5th ed., Whitten, Davis & Peck

 

Chapter 4 Review Quiz

 

MATCHING

  1. Electrolytes
  2. Acids
  3. Bases
  4. Salts
  5. Oxidation
  6. Reduction
  7. Spectator ions

 

    1. A compound that contains a cation other than H+ and an anion other than OH- of O-2
    2. A substance whose aqueous solutions conducts electricity
    3. Gain of electrons
    4. Lose of electrons
    5. A substance whose aqueous solutions do not conduct electricity
    6. In aqueous solutions, the process in which a molecular compound separates to form ions
    7. A substance that produces OH- ions in aqueous solution
    8. Ions in solution that do not participate in a chemical reaction
    9. A substance that produces H+ ions in aqueous solution

 

 

  1. Name the three classes of electrolytes.

 

 

  1. Write the ionization equation for perchloric acid.

 

 

  1. Strong electrolytes
    1. Are a metal hydroxide that is soluble in water and dissociates completely in dilute aqueous solution
    2. Are a molecular substance that ionizes only slightly in water to produce an alkaline solution
    3. Are a substance that conducts electricity well in dilute aqueous solution
    4. Are a substance that conducts electricity poorly in dilute aqueous solution
    5. Are a substance that does not conduct electricity at low temperatures but does so at higher temperatures

 

 

  1. Strong soluble bases
    1. Are a metal hydroxide that is soluble in water and dissociates completely in dilute aqueous solution
    2. Are a molecular substance that ionizes only slightly in water to produce an alkaline solution
    3. Are a substance that conducts electricity well in dilute aqueous solution
    4. Are a substance that conducts electricity poorly in dilute aqueous solution
    5. Are a substance that does not conduct electricity at low temperatures but does so at higher temperatures

 

Mark the following as (a) soluble, (b) moderately soluble or (c) insoluble in water.

 

12. (NH4)2CO2                        13. H2S            14. PbBr2         15. Ca3(PO4)2              16. H2O

 

17. AgNO2                  18. BaSO4       19. FeI             20. CaO                       21. KOH

 

For each of the following write balanced formula unit, total ionic and net ionic equations that occur when aqueous solutions of the compounds are mixed.

 

22. Cu(NO3)2 + Na2S à

 

 

 

23. Al2(SO4)3 + NaOH à

 

 

 

24. acetic acid + sodium hydroxide à

 

 

 

25. lead (II) hydroxide + phosphoric acid à

 

 

 

26. Ba(NO3)2 + AgBr à

 

 

 

Determine which of the following are oxidation reduction reactions. For those that are, identify the oxidizing and reducing agents.

 

27. HNO3 + 3HCl à NOCl + Cl2 + 2 H2O

 

 

 

28. 2KI + HgCl2 à 2KCl + HgI2

 

 

 

 

29. 2CoCl3 + 3Ca à 3CaCl2 + 2Co

 

 

 

30. What is the order of increasing activity of halogens?

 

 

Which of the following reactions occur?

31. 2I- + Cl2 à 2Cl- + I2

32. Cu + Mg+2 à Mg + Cu+2

33. Al2O3 + 3H2 à 2Al + 3H2O

34. Mg + H2O à MgO + H2

35. 2Br - + F2 à 2F- + Br2

 

 

ANSWERS

 

  1. b
  2. i
  3. g
  4. a
  5. d
  6. c
  7. h
  8. strong acids, strong soluble base, soluble salts
  9. HClO4 à H+ + ClO4-  (100% ionization because it is a strong acid)
  10. c
  11. a
  12. a
  13. c
  14. c
  15. c
  16. c
  17. b
  18. c
  19. c
  20. b
  21. a
  22. Cu(NO3)2 + Na2S à CuS¯ + 2NaNO3 formula unit

Cu+2 + 2NO3 -1 + 2Na+1 + S-2 àCuS¯ + 2 Na+1 + 2NO3-1 total ionic

Cu+2  + S-2 àCuS¯  net ionic

 

23. Al2(SO4)3 + 6NaOH à 2Al(OH)3¯  + 3Na2SO4 formula unit

            2Al+3 + 3SO4-2 + 6Na+1 + 6OH-1 à 2Al(OH)3¯ + 6Na+1 + 3SO4 –2 total ionic

            2Al+3 + 6OH-1 à 2Al(OH)3¯ net ionic

 

 

 

24. acetic acid + sodium hydroxide à

            HC2H3O2 + NaOH à NaC2H3O2 + H2O formula unit

            H+1 + C2H3O2-1 + Na+1 + OH-1 à Na+1 + C2H3O2-1 + H2O total ionic

            H+1 + OH-1 à H2O net ionic

 

25. lead (II) hydroxide + phosphoric acid à

            3Pb(OH)2 + 2H3PO4 à Pb3 (PO4)2 ¯  + 6H2O formula unit

            3Pb+2 + 6OH-1 + 6H+ + 2PO4 à Pb3(PO4)2 ¯ + 6H2O total ionic

            3Pb+2 + 6OH-1 + 6H+ + 2PO4 à Pb3(PO4)2 ¯ + 6H2O net ionic

 

26. Ba(NO3)2 + 2AgBr¯  à BaBr2 + 2AgNO3 formula unit

      Ba+2 + 2NO3-1 + 2AgBr¯ à Ba+2 + 2Br –1 + 2Ag+1­­ + 2NO3-1 total ionic

      2AgBr¯ à 2Br -1 + 2 Ag+1 net ionic

 

  1.  H+1 N+5 O3-2 + 3 H+1 Cl-1 à N+3O-2Cl-1 +Cl20 + 2H2O

 

N is reduced (gaining electrons); oxidizing agent

Cl is oxidized (losing electrons); reducing agent

 

  1. 2K+1 I-1 + Hg+2 Cl2 -1 à 2K+1 Cl-1 + Hg+2 I2 -1

Not a red-ox

 

  1. 2 Co+3 Cl3 -1 + 3Ca0 à 3 Ca+2 Cl2 -1 + 2Co0

 

Co is reduced (gaining electrons); oxidizing agent

Ca is oxidized (losing electrons); reducing agent

  1. I2< Br2 < Cl2 < F2
  2. Yes
  3. No
  4. No
  5. Yes
  6. Yes