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1. Volume of 0.10 M acetic acid needed for 25.0 mL of 0.020 M. mL 2. Molar mass of sodium acetate. g 3. Mass of sodium acetate transferred to beaker “A". 0.0396 g 4. Moles of sodium acetate measured. mol 5. Volume of 0.020 M acetic acid needed. mL 6. pH of beaker “A" mixture. pH = 4.75 7. Mass of sodium acetate transferred to beaker "B". 0.1920g 8. Moles of sodium acetate measured. mol 9. Volume of 0.10 M acetic acid needed. mL 10. pH of beaker “B" mixture. pH = 4.74 11. Accepted pK, of acetic acid. pKa = 4.74 12. Calculated K, from pH of beaker “A". K. = %3D 13. Calculated Ka from pH of beaker “B". Ka = %3D 14. Accepted K, of acetic acid. K. = 1.8 x 10-5

1. Volume of 0.10 M acetic acid needed for 25.0 mL of 0.020 M. mL 2. Molar mass of sodium acetate. g 3. Mass of sodium acetate transferred to beaker “A". 0.0396 g 4. Moles of sodium acetate measured. mol 5. Volume of 0.020 M acetic acid needed. mL 6. pH of beaker “A" mixture. pH = 4.75 7. Mass of sodium acetate transferred to beaker "B". 0.1920g 8. Moles of sodium acetate measured. mol 9. Volume of 0.10 M acetic acid needed. mL 10. pH of beaker “B" mixture. pH = 4.74 11. Accepted pK, of acetic acid. pKa = 4.74 12. Calculated K, from pH of beaker “A". K. = %3D 13. Calculated Ka from pH of beaker “B". Ka = %3D 14. Accepted K, of acetic acid. K. = 1.8 x 10-5

Chemistry
Chemistry
10th Edition
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 to calculate this data please

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Data Sheet with Sample Results 1. Volume of 0.10 M acetic acid needed for 25.0 mL of 0.020 M. mL 2. Molar mass of sodium acetate. g 3. Mass of sodium acetate transferred to beaker “A". 0.0396 g 4. Moles of sodium acetate measured. mol 5. Volume of 0.020 M acetic acid needed. mL 6. pH of beaker “A" mixture. pH = 4.75 7. Mass of sodium acetate transferred to beaker "B". 0.1920g 8. Moles of sodium acetate measured. mol 9. Volume of 0.10 M acetic acid needed. mL 10. pH of beaker "B" mixture. pH = 4.74 11. Accepted pKa of acetic acid. pKa = 4.74 12. Calculated Ka from pH of beaker “A". Ka 13. Calculated Ka from pH of beaker “B". Ka = 14. Accepted K, of acetic acid. Ka = 1.8 x 10-5
Transcribed Image Text:Data Sheet with Sample Results 1. Volume of 0.10 M acetic acid needed for 25.0 mL of 0.020 M. mL 2. Molar mass of sodium acetate. g 3. Mass of sodium acetate transferred to beaker “A". 0.0396 g 4. Moles of sodium acetate measured. mol 5. Volume of 0.020 M acetic acid needed. mL 6. pH of beaker “A" mixture. pH = 4.75 7. Mass of sodium acetate transferred to beaker "B". 0.1920g 8. Moles of sodium acetate measured. mol 9. Volume of 0.10 M acetic acid needed. mL 10. pH of beaker "B" mixture. pH = 4.74 11. Accepted pKa of acetic acid. pKa = 4.74 12. Calculated Ka from pH of beaker “A". Ka 13. Calculated Ka from pH of beaker “B". Ka = 14. Accepted K, of acetic acid. Ka = 1.8 x 10-5
Experimental Materials Sodium acetate Magnetic stirring bar (x 2) Acetic acid (0.10 M and 0.02 M) Beaker 50 mL (x 2) Hot plate (x 2) pH meter Graduated cylinder 25 mL (x 2) Dropper (x 2) Experimental Procedure 1. Label two 50 mL beakers “A" and "B" 2. Determine the volume in mL of 0.10 M acetic acid needed to make 25.0 mL of 0.020 M concentration, transfer that volume to a 25 mL graduated cylinder, then fill the graduated cylinder up to the 25 mL mark with distilled water. 3. Determine the molar mass of sodium acetate (CH3CO,Na). 4. Using a scale measure up to but no more than 0.040 g of sodium acetate, record the mass down to the milligram level, and transfer to the 50 mL beaker labelled “A". 5. Determine the number of moles of sodium acetate contained in the sample and record that number. 6. Determine the volume of 0.020 M acetic acid that contains the same number of moles of acetic acid as the sample of sodium acetate, use a graduated cylinder to transfer that volume to the 50 mL beaker labelled “A", add a magnetic stirring bar to the mixture, then place the 50 mL beaker labelled “A" on a hot plate to stir. 7. Once all the sodium acetate has been dissolved measure the pH of the solution with the pH meter. Note: be sure to rinse the pH meter probe with distilled water and wipe it dry with a "Kim Wipe" before and after each use. 8. Repeat steps 5 - 10 with the following changes: a. Use up to but no more than 0.200 g of sodium acetate b. Use 0.10 M acetic acid c. Use the beaker labeled "B" 9. Convert the pH value to the experimental Ka of the weak acid.
Transcribed Image Text:Experimental Materials Sodium acetate Magnetic stirring bar (x 2) Acetic acid (0.10 M and 0.02 M) Beaker 50 mL (x 2) Hot plate (x 2) pH meter Graduated cylinder 25 mL (x 2) Dropper (x 2) Experimental Procedure 1. Label two 50 mL beakers “A" and "B" 2. Determine the volume in mL of 0.10 M acetic acid needed to make 25.0 mL of 0.020 M concentration, transfer that volume to a 25 mL graduated cylinder, then fill the graduated cylinder up to the 25 mL mark with distilled water. 3. Determine the molar mass of sodium acetate (CH3CO,Na). 4. Using a scale measure up to but no more than 0.040 g of sodium acetate, record the mass down to the milligram level, and transfer to the 50 mL beaker labelled “A". 5. Determine the number of moles of sodium acetate contained in the sample and record that number. 6. Determine the volume of 0.020 M acetic acid that contains the same number of moles of acetic acid as the sample of sodium acetate, use a graduated cylinder to transfer that volume to the 50 mL beaker labelled “A", add a magnetic stirring bar to the mixture, then place the 50 mL beaker labelled “A" on a hot plate to stir. 7. Once all the sodium acetate has been dissolved measure the pH of the solution with the pH meter. Note: be sure to rinse the pH meter probe with distilled water and wipe it dry with a "Kim Wipe" before and after each use. 8. Repeat steps 5 - 10 with the following changes: a. Use up to but no more than 0.200 g of sodium acetate b. Use 0.10 M acetic acid c. Use the beaker labeled "B" 9. Convert the pH value to the experimental Ka of the weak acid.
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