AP CHEMISTRY CHAPTER 4 REVIEW



AP CHEMISTRY CHAPTER 4 REVIEW

(100 points)

(6 points) 1. Determine whether the following compounds are soluble or insoluble in water:

a. Hg2Cl2

b. KI

c. Pb(NO3)2

d. NaBr

e. Ba(OH)2

f. CrCO3

(4 points) 2. Determine the precipitate that will form, if any, when the following solutions are mixed:

a. BaCl2 (aq) + Na2SO4 (aq)

b. Pb(NO3)2 (aq) + 2 KCl (aq)

c. 3 AgNO3 (aq) + Na3PO4 (aq)

d. 3 NaOH (aq) + Fe(NO3)3 (aq)

(12 points) 3. Write net ionic equations for the reaction, if any, that occurs when aqueous solutions of the following are mixed:

a. copper (II) nitrate and ammonium sulfate

b. silver nitrate and iron (III) chloride

c. ammonium phosphate and potassium carbonate

d. sodium hydroxide and manganese (II) nitrate

(3 points) 4. Determine the volume of 0.100M Na3PO4 required to precipitate all the lead (II) ions from 150.0 mL of 0.250M Pb(NO3)2.

(4 points) 5. Determine the mass of barium sulfate that is produced when 100.0 mL of 0.100 M BaCl2 is mixed with 100.0 mL of 0.100 M Fe2(SO4)3.

(3 points) 6. Determine the molarity of a solution prepared by dissolving 11.85 g of KMnO4 in enough water to make 750.0 mL of solution.

(5 points) 7. A 0.1025gsample of copper metal is dissolved in 35.0 mL of concentrated nitric acid forming Cu2+ ions in solution. The solution is then diluted to a total volume of 200.0 mL. Determine the molarity of the Cu2+.

(4 points) 8. Determine the volume of 0.850M Al(NO3)3 that contains 50.00g of Al(NO3)3.

(3 points) 9. Determine the volume of 18.0M H2SO4 solution needed to prepare 250.0 mL of

1.75M H2SO4.

(3 points) 10. Determine the concentration of a solution of NaOH after diluting 10.0 mL of 10.0 M stock solution to 250.0 mL.

(3 points) 11. Heme, obtained from red blood cells, binds oxygen, O2. Calculate the number of moles of heme in 150.0 mL of 0.0019M heme solution.

(3 points) 12. Determine the volume of 0.100 M NaOH required toreact completely with 25.0 mL

of 0.200 M H2SO4.

(4 points) 13. Determine the molarity of Fe3+ and SO42- ions in a solution prepared by dissolving 48.05g of Fe2(SO4)3 in enough water to make a 800.0 mL solution.

(5 points) 14. The distinctive odor of vinegar is due to acetic acid, HC2H3O2, which reacts with sodium hydroxide in the following fashion:

HC2H3O2 (aq) + NaOH (aq) → H2O (l) + NaC2H3O2 (aq)

3.45 mL of vinegar requires 42.5 mL of 0.115 M NaOH to reach the equivalence point in a titration. Determine the mass, in grams, of vinegar titrated by the NaOH solution.

15. A solution of 100.0 mL of 0.200 M KOH is mixed with a solution of 200.0 mL

of 0.150 M NiSO4 according to the following reaction:

2 KOH (aq) + NiSO4 (aq) → K2SO4 (aq) + Ni(OH)2 (s)

(4 points) (a) Determine the mass, in grams, of Ni(OH)2 that will precipitate.

(1 point) (b) What is the identity of the limiting reactant?

(1 point) (c) What is the identity of the excess reactant?

(7 points) (d) Determine the concentration of each ion remaining in solution after the precipitation is complete.

(7 points) 16. Assign oxidation states to each of the atoms in the following compounds.

a. GaO3

b. KBrO4

c. NbO2

d. CrO3

e. Na3PO4

f. NH2-

g. IO3-

(8 points) 17. Balance the following oxidation-reduction reactions that occur in acidic solution.

a. Zn (s) + NO3- (aq) → Zn2+ (aq) + NH4+ (aq)

b. Br - (aq) + MnO4 - (aq) → Br2 (l) + Mn2+ (aq)

(10 points) 18. Balance the following oxidation-reduction reactions in basic solution.

a. MnO4- (aq) + SO32- (aq) → MnO2 (s) + SO42- (aq)

b. Co2+ (aq) + H2O2 (l) → Co(OH)3 (s) + H2O (l)

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