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1. Using a graduated cylinder to measure volumes, prepare a buffer solution from 20.0 mL of 0.10 M acetic acid and 30.0 mL of 0.10 sodium acetate. a Calculate the pH of the buffer. (Ka = 1.8 x 105) (b. Measure the actual pH of the solution using your pH meter. c. Compare the experimental result in (b) to the calculated value in (a). Determine the % error.

1. Using a graduated cylinder to measure volumes, prepare a buffer solution from 20.0 mL of 0.10 M acetic acid and 30.0 mL of 0.10 sodium acetate. a Calculate the pH of the buffer. (Ka = 1.8 x 105) (b. Measure the actual pH of the solution using your pH meter. c. Compare the experimental result in (b) to the calculated value in (a). Determine the % error.

Chemistry
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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I need help with 1a, 1c, 2c
Table I: Acetic acid/sodium acetate Buffer Buffer pH pH theoretical experimental pH pH pH theoretical pH Error theoretical after experimental Error after adding base experimental Error Initially Initially adding after adding after adding acid acid base HC2H3O2/ C2H3O2 H2O 4.95 4.516 5.14 8.62 Hand write ALL of your calculations under the table. 2. 30 1.960
Transcribed Image Text:Table I: Acetic acid/sodium acetate Buffer Buffer pH pH theoretical experimental pH pH pH theoretical pH Error theoretical after experimental Error after adding base experimental Error Initially Initially adding after adding after adding acid acid base HC2H3O2/ C2H3O2 H2O 4.95 4.516 5.14 8.62 Hand write ALL of your calculations under the table. 2. 30 1.960
Note: For each experiment requiring a calculation show the method and logic used in the calculation. Be sure to completely show all steps and units in each step. Use a pH meter to measure pHs. Prepare appropriate tables for each experiment to record your lab data. Remember to carefully record all procedures and observations. 1. Using a graduated cylinder to measure volumes, prepare a buffer solution from 20.0 mL of 0.10 M acetic acid and 30.0 mL of 0.10 sodium acetate. a Calculate the pH of the buffer. (Ka = 1.8 x 10-5) (b. Measure the actual pH of the solution using your pH meter. c. Compare the experimental result in (b) to the calculated value in (a). Determine the % error. 2. Divide your buffer solution in (1) into two equal 25.0 mL volumes. Calculate the expected pH of the following solutions and then measure the pH of each. a. To one of the 25.0 ml solutions add 5.0 mL of 0.10 M HCl and measure the pH. (b To the second add 5.0 mL of 0.10 M NAOH and record the pH. c. Compare the experimental results with the theoretical results. Why are there differences in their pHs? 3. Carry out the following measurements and also calculate the expected pH of the following solutions: Measure the pH of deionized water. (b. Add 5.0 mL of 0.10 M HCl to 25.0 mL of water and measure pH Add 5.0 mL of 0.10 M NAOH to a new sample of 25.0 mL of water and measure pH. Based on this data, is water a buffer?
Transcribed Image Text:Note: For each experiment requiring a calculation show the method and logic used in the calculation. Be sure to completely show all steps and units in each step. Use a pH meter to measure pHs. Prepare appropriate tables for each experiment to record your lab data. Remember to carefully record all procedures and observations. 1. Using a graduated cylinder to measure volumes, prepare a buffer solution from 20.0 mL of 0.10 M acetic acid and 30.0 mL of 0.10 sodium acetate. a Calculate the pH of the buffer. (Ka = 1.8 x 10-5) (b. Measure the actual pH of the solution using your pH meter. c. Compare the experimental result in (b) to the calculated value in (a). Determine the % error. 2. Divide your buffer solution in (1) into two equal 25.0 mL volumes. Calculate the expected pH of the following solutions and then measure the pH of each. a. To one of the 25.0 ml solutions add 5.0 mL of 0.10 M HCl and measure the pH. (b To the second add 5.0 mL of 0.10 M NAOH and record the pH. c. Compare the experimental results with the theoretical results. Why are there differences in their pHs? 3. Carry out the following measurements and also calculate the expected pH of the following solutions: Measure the pH of deionized water. (b. Add 5.0 mL of 0.10 M HCl to 25.0 mL of water and measure pH Add 5.0 mL of 0.10 M NAOH to a new sample of 25.0 mL of water and measure pH. Based on this data, is water a buffer?
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