1. 25.6ml of 0.15M KOH is added to 43.5ml of 0.25 M HCl. What is the pH of the solution?

2. What is the pH of a solution made by combining 0.50 moles of hypobromous acid with 0.30 moles of calcium hypobromite in a 1 liter container? Ka HBrO = 2 x 10^-9

3. Calculate the pH of a solution that has 42.3mL of 0.10M HCl added to 100.0mL of a buffer containing 0.50M NH₃ and 0.5M NH₄Cl Kb = 1.8 x 10^-5

4. Calculate the pH of a solution that has 20.0 ml. of 0.2 M NaOH added to 30.0 ml. of 0.15 M acetic acid Ka = 1.8 x 10^-5 .

5. Calculate the pH of a solution that has 30.0 ml. of 0.2 M NaOH added to 30.0 ml. of 0.2M acetic acid.

6. Calculate the pH of a solution that has 15.0 ml. of 0.2 M NaOH added to 30.0 ml. of .15 M acetic acid.

7. How many grams of NaOH must be added to 100.0mL of 0.1M HC₂H₃O₂ to produce a buffer with a pH of 5.2 ?

8. 25.0mL of H₂SO₄ is titrated to the equivalence point with 32.6 mL of 0.15M Al(OH)₃. what is the concentration of the acid?

9. Give the approximate pH of the equivalence pint for the following neutralization reactions

Strong acid/strong base

weak acid/strong base

weak base strong acid

weak acid Ka = 10^-5 / weak base Kb = 10^-7

10. Give the definition of a buffer.

Answers:

1. pH = 0.993 2. pH =8.78 3. pH = 9.18 4. pH = 5.65 5. pH = 8.87

6. pH = 5.05 7. 0.297 g 8. 0.293M