Question

2. Consider a buffer prepared by mixing 15.0 mL of a 0.300 M lactic acid (Ka = 1.4 x 10^-4) and 15.0 mL of 0.300 M potassium lactate. Calculate the pH. 3. Calculate the pH of a buffer when 15.0 mL of a 0.150 M sodium hydroxide is mixed with 15.0 mL of a 0.300 M lactic acid. 4. Buffers can also be basic. Would a solution that is 0.20 M in ammonia and 0.20 M in ammonium chloride be a buffer? Explain. Make a drawing as was done in Pre-lab Question 2 showing the composition of this solution. Write the Henderson- Hasselbalch equation for a basic buffer and calculate the pH. 5. Explain what happens when a small amount of acid is added to the ammonia/ammonium chloride solution. Use the illustration in Question 4 to help in the reasoning process. You may want to include another illustration. Predict and then calculate the pH after the addition of 10.0 mL of 0.10 M HCl to 65.0 mL of the ammonia/ammonium chloride solution.

          2. Consider a buffer prepared by mixing 15.0 mL of a 0.300 M lactic acid (Ka =
1.4 x 10^-4) and 15.0 mL of 0.300 M potassium lactate. Calculate the pH.

3. Calculate the pH of a buffer when 15.0 mL of a 0.150 M sodium hydroxide is
mixed with 15.0 mL of a 0.300 M lactic acid.

4. Buffers can also be basic. Would a solution that is 0.20 M in ammonia and 0.20
M in ammonium chloride be a buffer? Explain. Make a drawing as was done in Pre-lab
Question 2 showing the composition of this solution. Write the Henderson-
Hasselbalch equation for a basic buffer and calculate the pH.

5. Explain what happens when a small amount of acid is added to the ammonia/ammonium
chloride solution. Use the illustration in Question 4 to help in the reasoning process.
You may want to include another illustration. Predict and then calculate the pH after
the addition of 10.0 mL of 0.10 M HCl to 65.0 mL of the ammonia/ammonium chloride
solution.

2. Consider a buffer prepared by mixing 15.0 mL of a 0.300 M lactic acid (Ka =
1.4 x 10^-4) and 15.0 mL of 0.300 M potassium lactate. Calculate the pH.

3. Calculate the pH of a buffer when 15.0 mL of a 0.150 M sodium hydroxide is
mixed with 15.0 mL of a 0.300 M lactic acid.

4. Buffers can also be basic. Would a solution that is 0.20 M in ammonia and 0.20
M in ammonium chloride be a buffer? Explain. Make a drawing as was done in Pre-lab
Question 2 showing the composition of this solution. Write the Henderson-
Hasselbalch equation for a basic buffer and calculate the pH.

5. Explain what happens when a small amount of acid is added to the ammonia/ammonium
chloride solution. Use the illustration in Question 4 to help in the reasoning process.
You may want to include another illustration. Predict and then calculate the pH after
the addition of 10.0 mL of 0.10 M HCl to 65.0 mL of the ammonia/ammonium chloride
solution.

Added by Kyle M.

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