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12 Dec 2019

Buffer Solution from Strong Base and Weak Acid

Solution=
30.0 mL of 1.0 M CH3COOH
5.0 mL of 1.0 M NaOH

1. Calculate the total volume. 35 mL

2. What is the concentration of acetic acid in this solution after mixing? (include units)

3. What is the concentration of sodium hydroxide in this solution after mixing (include units)

4. Calculate the expected pH of this buffer solution.

5. Measured pH of this buffer solution. 3.89

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Keith LeannonLv2

13 Dec 2019

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Related questions

IV. Comparing Buffering Capacity

A. pH of Pure Water

i. Measure out 30.0 mL DI H2O into a beaker.

1. Calculate the expected pH of pure water. pH ________

2. Measured pH of pure water. pH ___3.88______

3. What is the percent error between the calculated and measured value? What are some of the possible sources of this error?

% error __________

B. pH of Water and Strong Acid

i. Measure out 30.0 mL DI H2O and 2.0 mL of 1.0 M HCl into a beaker.

1. Calculate the expected pH of this solution. pH _________

2. Measured pH of this solution. pH ___1.64______

3. What is the percent error between the calculated and measured value? What are some of the possible sources of this error?

% error ____

C. pH of Water and Strong Base

i. Measure out 30.0 mL DI H2O and 2.0 mL of 1.0 M NaOH into a beaker.

1. Calculate the expected pH of this solution. pH _________

2. Measured pH of this solution. pH __12.03_______

3. What is the percent error between the calculated and measured value? What are some of the possible sources of this error?

% error ____

D. pH of Buffer solution

i. Measure out 50.0 mL 1.0 M CH3COOH and 50.0 mL of 1.0 M NaCH3COO into a beaker.

1. Calculate the total volume. (include units) Vol __________

2. What is the concentration of acetic acid in this solution after mixing. (include units)

[CH3COOH] _________

3. What is the concentration of acetate ion in this solution after mixing. (include units)

[CH3COO-] ___________

4. Calculate the expected pH of this buffer solution. pH __________

5. Measured pH of this buffer solution. pH __4.56________

6. What is the percent error between the calculated and measured value? What are some of the possible sources of this error?

% error __________

E. pH of Buffer after the addition of the Strong Acid

Measure out 50.0 mL the buffer in part D and add 2.0 mL of 1.0 M HCl into a clean beaker.

1. Calculate the expected pH of this solution. pH _________

2. Measured pH of this solution. pH ____5.30_____

3. What is the percent error between the calculated and measured value? What are some of the possible sources of this error?

% error ____

F. pH of Buffer after the addition of the Strong Base

Measure out 50.0 mL the buffer in part D and 2.0 mL of 1.0 M NaOH into a clean beaker.

1. Calculate the expected pH of this solution. pH _________

2. Measured pH of this solution. pH _4.57________

3. What is the percent error between the calculated and measured value? What are some of the possible sources of this error?

% error ____

1 A buffer is prepared by mixing 50.0 mL of 0.100 M acetic acid with 30.0 mL of 0.100 M sodium hydroxide and 20.0 mL of distilled water. Estimate the concentration of acetic acid in the resulting buffer. Report your answer in moles/liter, but do not include units with your answer. 2 Determine the concentration of acetate ions in the buffer solution. Report your answer in moles per liter, but do not include units in your answer. 3 Estimate the pH of the buffer solution using the Henderson-Hasselbalch equation. 4 Using the Henderson-Hasselbalch equation, estimate the pH of the buffer if an additional 10.0 mL of 0.100 M sodium hydroxide is added. 5 Estimate the pH of the original buffer if 10.0 mL of 0.100 M hydrochloric acid is added.