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Reactions and Periodicity: Review Questions for AP Chemistry

By — McGraw-Hill Professional
Updated on Feb 1, 2011

Review the following concepts if necessary:

Problems

  1. _____ Fe(OH)2(s) + _____ H3PO4(aq) → _____ Fe3(PO4)2(s) + _____ H2O(l)
  2. After the above chemical equation is balanced the lowest whole-number coefficient for water is:

    1. 3
    2. 1
    3. 9
    4. 6
    5. 12

    Choose one of the following for questions 2–4.

    1. Cu2+
    2. CO32–
    3. Fe3+
    4. Al3+
    5. Pb2+
  3. This ion will generate gas bubbles when hydrochloric acid is added.
  4. This ion initially gives a white precipitate when dilute sodium hydroxide is added to a solution containing this ion. The precipitate will dissolve in excess sodium hydroxide.
  5. Aqueous solutions of this ion are blue.
  6. Which of the following best represents the balanced net ionic equation for the reaction of lead(II) carbonate with concentrated hydrochloric acid?
    1. Pb2CO3 + 2 H+ + Cl → Pb2Cl +CO2 +H2O
    2. PbCO3 + 2 H+ + 2 Cl → PbCl2 + CO2 + H2O
    3. PbCO3 + 2 H+ → Pb2+ + CO2 + H2O
    4. PbCO3 + 2 Cl → PbCl2 + CO32–
    5. PbCO3 + 2 HCl → PbCl2 + CO2 + H2O
  7. A sample of copper metal is reacted with concentrated nitric acid in the absence of air. After the reaction, which of these final products are present?
    1. CuNO3 and H2O
    2. Cu(NO3)3, NO, and H2O
    3. Cu(NO3)2, NO, and H2O
    4. CuNO3, H2O, and H2
    5. Cu(NO3)2, NO, and H2
  8. Which of the following is the correct net ionic equation for the reaction of acetic acid with potassium hydroxide?
    1. HC2H3O2 + OH → C2H3O2 + H2O
    2. HC2H3O2 + K+ → KC2H3O2 + H+
    3. HC2H3O2 + KOH → KC2H3O2 + H2O
    4. H+ + OH → H2O
    5. C2H3O2 + KOH → KC2H3O2 + OH
  9. Which of the following is the correct net ionic equation for the addition of aqueous ammonia to a precipitate of silver chloride?
    1. AgCl + 4 NH3 → [Ag(NH3)4]+ + Cl
    2. AgCl + 2 NH4+ → [Ag(NH4)2]3+ + Cl
    3. AgCl + NH4+ → Ag+ + NH4Cl
    4. AgCl + NH3 → Ag+ + NH3Cl
    5. AgCl + 2 NH3 → [Ag(NH3)2]+ + Cl
  10. Potassium metal will react with water to release a gas and a potassium compound. Which of the following is a false statement?
    1. he solution is acidic.
    2. The gas is hydrogen.
    3. The potassium compound is water-soluble.
    4. The potassium compound will react with hydrochloric acid.
    5. A solution of the potassium compound will form a precipitate when added to an FeCl2 solution.
  11. A sample is tested for the presence of the 22+ion. This ion, along with others, may be precipitated with chloride ion. If Hg22+ is present in the chloride precipitate, a black color will form upon treatment with aqueous ammonia. The balanced net ionic equation for the formation of this black color is:
    1. Hg2Cl2 + 2 NH3 + 2 H2O → 2 Hg + 2 NH4+ + 2 Cl + 2 OH
    2. Hg2Cl2 + 2 NH3 → 2 Hg + 2 NH3Cl
    3. Hg2Cl2 + 2 NH4+ → 2 Hg + 2 NH4Cl
    4. Hg2Cl2 + NH4]+ → 2 Hg + NH4Cl + Cl
    5. Hg2Cl2 + 2 NH3 → Hg + HgNH2Cl + NH4+ + Cl
  12. Which of the following solids is not soluble in water, but is soluble in dilute nitric acid (HNO3)?
    1. NaOH
    2. BaCO3
    3. AgCl
    4. (NH4)3PO4
    5. FeCl2
  13. What is the minimum number of moles of Pb(NO3)2 must be added to 0.10 L of a solution that is 1.0 M in MgCl2 and 1.0 M in KCl? The compound PbCl2 precipitates.
    1. 1.0 moles
    2. 0.20 moles
    3. 0.50 moles
    4. 0.15 moles
    5. 0.30 moles
  14. When 50.0 mL of 1.0 M AgNO3 is added to 50.0 mL of 0.50 M HCl a precipitate of AgCl forms. After the reaction is complete, what is the concentration of silver ions in the solution?
    1. 0.50 M
    2. 0.0 M
    3. 1.0 M
    4. 0.25 M
    5. 0.75 M
  15. A student mixes 50.0 mL of 0.10 M Pb(NO3)2 solution with 50.0 mL of 0.10 M KCl. A white precipitate forms, and the concentration of the chloride ion becomes very small. Which of the following correctly places the concentrations of the remaining ions in order of decreasing concentration?
    1. [NO3] > [Pb2+] > [K+]
    2. [NO3] > [K+ ] > [Pb2+ ]
    3. [K+ ] > [NO3] > [Pb2+]
    4. [Pb2+] > [NO3] > [K+ ]
    5. [Pb2+] > [K+] > [NO3]
  16. A solution is prepared for qualitative analysis. The solution contains the following ions: Co2+, Pb2+, and Al3+. Which of the following will cause no observable reaction?
    1. Dilute NH3(aq) is added.
    2. Dilute K2CrO4(aq) is added.
    3. Dilute HNO3(aq) is added.
    4. Dilute K2S(aq) is added.
    5. Dilute HCl(aq) is added.
  17. Chlorine gas is bubbled through a colorless solution and the solution turns reddish. Adding a little methylene chloride to the solution extracts the color into the methylene chloride layer. Which of the following ions may be present in the original solution?
    1. Cl
    2. I
    3. SO42–
    4. Na+
    5. Br
  18. The addition of concentrated NaOH(aq) to a 1.0 M (NH4)2SO4 solution will result in which of the following observations?
    1. The solution becomes neutral.
    2. The formation of a brown precipitate takes place.
    3. Nothing happens because the two solutions are immiscible.
    4. The odor of ammonia will be detected.
    5. An odorless gas forms and bubbles out of the mixture.
  19. Which of the following solutions will give a yellow precipitate when a 0.1 M Na2CrO4 solution is added to a 0.1 M solution of the ion listed?
    1. K+(aq)
    2. Pb2+(aq)
    3. NO3(aq)
    4. OH(aq)
    5. NH4+(aq)
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