1. Read the Chapter and Review Your Notes

CHAPTER 4 HOMEWORK

1. Read the chapter and review your notes.

2. Answer the following questions; solve the following problems – remember answers without supporting work will not receive credit.

1. Show how each of the following strong electrolytes dissociates upon dissolving in water:

(a) NaBr

(b) MgCl2

(d) HNO3

(e) Al(NO3)3

2. Calculate the molarity of each of the following solutions.

(a) A 5.623g sample of NaHCO3 is dissolved in enough water to make a 250.0 mL solution.

(b) A 184.6 mg sample of K2Cr2O7 is dissolved in enough water to make a 500.0 mL solution.

(c) A 0.1025g sample of copper metal is dissolved in 35.0 mL of concentrated Cu2+ ions and then water is added to make a total volume of 200.0 mL. Calculate the molarity of the Cu2+ ions.

3. Calculate the concentration of all ions present in each of the following solutions of strong electrolytes.

(a) 0.15 M CaCl2

(b) 0.26 M Al(NO3)3

(d) 2.0 x 10-3 M Al2(SO4)3

4. Calculate the volume of a 0.100 M solution of NaHCO3 that contains 0.350 g of NaHCO3.

5. Describe how you would prepare 2.00 L of 0.250 M NaOH from solid NaOH.

6. Describe how you would prepare 1.00 L of 0.500 M HCl from a concentrated (12 M) stock solution.

7. A solution is prepared by dissolving 10.8 g of ammonium sulfate in enough water to make a 100.0 mL stock solution. A 10.00 mL sample of this stock solution is added to 50.00 mL of water. Calculate the concentrations of ammonium ions and sulfate ions in the final solution.

8. When the following solutions are mixed together, what precipitate (if any) will form?

(a) BaCl2 (aq) and Na2SO4 (aq)

(b) Pb(NO3)2 (aq) and KCl (aq)

9. Write complete, balanced molecular equations and net ionic equations for the reaction, if any, which occurs when aqueous solutions of the following are mixed:

(a) silver nitrate and barium chloride

(b) iron (II) sulfate and potassium sulfide

(d) dimercury (I) nitrate and calcium chloride

10. What mass of solid aluminum hydroxide is produced when 50.0 mL of a 0.200 M solution of Al(NO3)3 is added to 200.0 mL of 0.100 M KOH?

11. Determine the mass, in grams, of sodium carbonate (Na2CO3) required to completely react with 25.0 mL of 0.155 M nitric acid (HNO3).

Na2CO3 (aq) + 2 HNO3 (aq) → 2 NaNO3 (aq) + CO2 (g) + H2O (l)

12. Calculate the mass of carbon dioxide produced when 75.0 mL of 0.350 M HCl reacts with excess Na2CO3.

Na2CO3 (s) + 2 HCl (aq) → 2 NaCl (aq) + H2O (l) + CO2 (g)

13. You can dissolve an aluminum soft drink can in an aqueous base such as potassium hydroxide:

2 Al (s) + 2 KOH (aq) + 6 H2O (l) → 2 KAl(OH)4 (aq) + 3 H2 (g)

If you place 2.05g of aluminum in a beaker with 185 mL of 1.35 M KOH, will any aluminum remain? What mass, in grams, of KAl(OH)4 is produced?

14. How many grams of silver chloride can be prepared by the reaction of 100.0 mL of 0.200 M silver nitrate with 100.0 mL of 0.150 M calcium chloride? Calculate the concentration of each ion remaining in solution after the precipitation reaction is complete.

15. Determine the volume of 0.150 M HNO3 required to neutralize 50.00 mL of 0.200 M NaOH.

16. Determine the volume of 0.0200 M calcium hydroxide is required to neutralize 35.00 mL of 0.0500 M nitric acid?

17. Assign oxidation states to each of the atoms in the following ions/compounds:

(a) Cr(OH)4-

(b) K2SO4

(d) H2PO4-

18. Balance the following oxidation-reduction reactions in an acidic solution:

(a) VO2+ (aq) + Zn (s) → VO2+ (aq) + Zn2+ (aq)

(b) Cr2O72- (aq) + Fe2+ (aq) → Cr3+ (aq) + Fe3+ (aq)

19. Balance the following oxidation-reduction reactions in a basic solution:

(a) CrO42- (aq) + SO32- (aq) → Cr(OH)3 (s) + SO42- (aq)

(b) NiO2 (s) + Zn (s) → Ni(OH)2 (s) + Zn(OH)2 (s)

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