1. Write dissociation equations for the following when they are dissolved in water.

b. SrBr₂

d. NH₄Cl

2. Classify the following as strong, weak or nonelectrolyte.

b. C₁₂H₂₂O₁₁ (sugar)

c. HCl

3. Calculate the molarity of the following solutions.

a. 49.73 g H₂SO₄ in enough water to make 500 mL of solution.

b. 4.739 g RuCl₃ in enough water to make 1.00 L of solution.

c. 5.035 g FeCl₃ in enough water to make 250 mL of solution.

4. Calculate the concentrations of each of the ions in the following solutions.

b. 0.15 M Al₂(SO₄)₃

c. 0.87 M Na₂CO₃

5. Describe how you would prepare the following solutions.

b. 250 mL of 1.0 M Na₂SO₄

c.1.5 L of 0.5 M K₂Cr₂O₇.

6. Describe how you would prepare the following solutions:

a. 500 mL of 1.0 M H₂SO₄ from 17.8 M H₂SO₄.

b. 1.5 L of 0.25 M KMnO₄ from 1.0 M stock solution.

c. 1.0 L of 0.15 M KBrO₃ from solid KBrO₃.

7. A standard solution of KHP(C₈H₅O₄K) was made by dissolving 3.697 g of KHP in enough water to make 100.0 mL of solution. Calculate the concentration.

8. How many moles of KHP are contained in 30.00 mL of the solution in problem 7?

9. How many milliliters of 0.136 M NaOH are required to react with the H₂SO₄ in 10 mL of a 0.202 M solution? The reaction of the two is

2NaOH + H₂SO₄ ® Na₂SO₄ + 2H₂O

10. Complete and balance the following reactions:

b. Ca(OH)₂(aq) + Na₂CO₃(aq) ®

c. Na₂S(aq) + FeCl₃(aq) ®

11. How would you separate the following by selective precipitation?

Ba²⁺, Pb²⁺, Fe²⁺

12. Write molecular, complete ionic and net ionic equations for the following reactions.

a. aqueous sodium sulfide reacts with aqueous copper(II) nitrate.

b. aqueous hydrogen fluoride reacts with aqueous potassium hydroxide.

13. Calculate the mass of CaSO₄ produced when 10 mL of 6.0 M H₂SO₄ is added to 100 mL of 0.52 M Ca(NO₃)₂.

14. Calculate the mass of Al₂S₃ produced when 100 mL of 0.50 M AlCl₃ is added to 100 mL of 0.50 M Na₂S.

15. What is the percentage of iron in an ore sample if a 0.9973 g sample dissolved in acid produces 0.8314 g of Fe(OH)₃ precipitate when treated with excess KOH?

16. A sample containing only sodium chloride and potassium chloride is dissolved and treated with excess AgNO₃. A 0.9341 g sample of the salt mixture gave 2.0321 g of AgCl. Calculate the percentage of chloride in the sample.

17. How many mL of 1.50 M NaOH is required to neutralize 275 mL of 0.5 M H₂SO₄?

18. What is the molarity of a solution of HCl if it requires 29.31 mL of a 0.0923 M NaOH solution to reach a phenolphthalein endpoint for the titration of a 10.0 mL aliquot of the HCl solution?

19. Determine the oxidation number for Mn in each of the following:

b. LiMnO₂

c. MnO₂

20. A titration is done using 0.1302 M NaOH to determine the molecular weight of an acid. The acid contains one acidic hydrogen per molecule. If 1.863 g of the acid require 70.11 mL of the NaOH solution what is the molecular weight of the acid?

26. Determine the oxidation number for each atom in the following compounds or ions:

b. P₄O₁₀

c. S₈

d. H₂CO

27. Balance the following oxidation reduction reactions. Which species in each is the oxidizing agent? Which is the reducing agent?

b. Sn²⁺ + Cu²⁺ ® Sn⁴⁺ + Cu⁺

c. Cu + H⁺ + NO₃^- ® Cu2+ + NO₂ + H₂O

28. Balance the following in basic solution:

b. Cl₂ + OH- ® Cl + ClO₃^-

c. Zn + NO₃- ® Zn2+ + NH₃

29. Iron(II) can be determined by redox titration with a cerium (IV) solution. The oxidation reduction reaction is

Fe²⁺ + Ce⁴⁺ ® Fe³⁺ + Ce³⁺

What is the concentration of Fe²⁺ if it requires 21.35 mL of 0.3136 M Ce⁴⁺ to titrate a 10.00 mL aliquot to the endpoint?