Acids and Bases – Problem Set #2

Directions:  Do all work on a separate sheet of paper.  You do not need to recopy any of the questions.  Show ALL WORK to receive full credit – do not simply write down the answers.

1)    Find the pH for each of the following solutions:

1. 1.54 x 10^-2  M HI
2. 4.67 x 10^-5  M HNO₃
3. 8.76 x 10^-4  M KOH
4. 6.44 x 10^-3  M LiOH

2)    For each of the following pH values, calculate the [H₃O⁺] and the [OH^-].

1. 2
2. 12
3. 7
4. 4
5. 9

3)    For the following solutions, calculate the [H₃O⁺] and the [OH^-] using K_w.

5. 5.67 x 10^-3  M HCl
6. 6.32 x 10^-6  M HClO₄
7. 8.76 x 10^-5  M Ba(OH)₂
8. 1.56 x 10^-2  M NaOH

4)    21.0 mL of an unknown solution of H₂SO₄ was titrated to the end point with 37.0 mL of 0.426 M KOH.  What is the concentration of the sulfuric acid?

5)    In a titration, 23.5 mL of a .340 M solution of H₂CO₃ was used to neutralize 27.6 mL of LiOH.  What is the molarity of LiOH?

6)    In the titration of 42.0 mL of an NH₃ solution, the end point was reached when 35.4 mL of 0.143 M HCl was added.  What is the concentration of the ammonia solution?

7)    34.0 mL of HC₂H₃O₂ was neutralized by 11.2 mL of 0.0527 M Ca(OH)₂.  Calculate the concentration of the acetic acid.

8)    What volume of 0.320 M H₃PO₄ neutralizes 35.0 mL of 0.420 M Ba(OH)₂?