A titration flask contains 0.00405 moles of an acetic acid sample a. Determine the moles of the base (NaOH) required to completely neutralize the acid. b. If the molarity of the based added from the buret was 0.200 M, determine the volume of the base (in mL) required to reach the end point of this titration.
A titration flask contains 0.00405 moles of an acetic acid sample a. Determine the moles of the base (NaOH) required to completely neutralize the acid. b. If the molarity of the based added from the buret was 0.200 M, determine the volume of the base (in mL) required to reach the end point of this titration.
Chemistry by OpenStax (2015-05-04)
1st Edition
ISBN:9781938168390
Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Chapter4: Stoichiometry Of Chemical Reactions
Section: Chapter Questions
Problem 79E: Titration of a 20.0-mL sample of acid rain required 1.7 mL of 0.08 11 M NaOH to reach the end point....
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A titration flask contains 0.00405 moles of an acetic acid sample | |
a. Determine the moles of the base (NaOH) required to completely neutralize the acid. |
|
b. If the molarity of the based added from the buret was 0.200 M, determine the volume of the base (in mL) required to reach the end point of this titration. |
|
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