Calculations: a) Average the two closest burette readings. Average all three readings if they agree within + 0.25 ml. b) Write the chemical equation for the reaction of acetic acid with sodium hydroxide. c) Calculate the amount (in moles) of sodium hydroxide that you needed to reach the equivalence point. Then calculate the concentration of acetic acid in the vinegar. d) Find the molar mass of acetic acid. Then calculate the mass of acetic acid in the volume of vinegar you used. e) The density of vinegar is 1.01 g/ml. Calculate the mass of the vinegar you used. Then find the percent (m/v) of acetic acid in the vinegar. Discussion: a) Compare your results with other students. What can you conclude about the concentration of vinegar you and the rest of the class used? b) Discuss how accurate you believe your results to do and any possible sources of error. c) Phenolphthalein was used as an indicator. Why should we place the vinegar, rather than sodium hydroxide, in the Erlenmeyer flask? d) Water was added to the Erlenmeyer flask at the beginning of the lab. Near the end of the titration, a partial drop on the tip of the burette can be washed into the Erlenmeyer flask using distilled water. Why will this distilled water not affect the end point of the titration? Name: Partners:

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
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Calculations:
a) Average the two closest burette readings. Average all three readings if they agree within +
0.25 ml.
b) Write the chemical equation for the reaction of acetic acid with sodium hydroxide.
c) Calculate the amount (in moles) of sodium hydroxide that you needed to reach the
equivalence point. Then calculate the concentration of acetic acid in the vinegar.
d) Find the molar mass of acetic acid. Then calculate the mass of acetic acid in the volume of
vinegar you used.
e) The density of vinegar is 1.01 g/ml. Calculate the mass of the vinegar you used. Then find the
percent (m/v) of acetic acid in the vinegar.
Discussion:
a) Compare your results with other students. What can you conclude about the concentration of
vinegar you and the rest of the class used?
b) Discuss how accurate you believe your results to do and any possible sources of error.
c) Phenolphthalein was used as an indicator. Why should we place the vinegar, rather than
sodium hydroxide, in the Erlenmeyer flask?
d) Water was added to the Erlenmeyer flask at the beginning of the lab. Near the end of the
titration, a partial drop on the tip of the burette can be washed into the Erlenmeyer flask using
distilled water. Why will this distilled water not affect the end point of the titration?
Name:
Partners:
Transcribed Image Text:Calculations: a) Average the two closest burette readings. Average all three readings if they agree within + 0.25 ml. b) Write the chemical equation for the reaction of acetic acid with sodium hydroxide. c) Calculate the amount (in moles) of sodium hydroxide that you needed to reach the equivalence point. Then calculate the concentration of acetic acid in the vinegar. d) Find the molar mass of acetic acid. Then calculate the mass of acetic acid in the volume of vinegar you used. e) The density of vinegar is 1.01 g/ml. Calculate the mass of the vinegar you used. Then find the percent (m/v) of acetic acid in the vinegar. Discussion: a) Compare your results with other students. What can you conclude about the concentration of vinegar you and the rest of the class used? b) Discuss how accurate you believe your results to do and any possible sources of error. c) Phenolphthalein was used as an indicator. Why should we place the vinegar, rather than sodium hydroxide, in the Erlenmeyer flask? d) Water was added to the Erlenmeyer flask at the beginning of the lab. Near the end of the titration, a partial drop on the tip of the burette can be washed into the Erlenmeyer flask using distilled water. Why will this distilled water not affect the end point of the titration? Name: Partners:
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