A student was required to prepare 250.0 mL of a cyanoacetic acid/sodium cyanoacetate buffer in which the concentration of the weak acid component was 0.067 M and the concentration of the conjugate base was 0.051 M. The student was supplied with 0.691 M cyanoacetic acid and 1.0M NaOH to perform this task. What volume (in mL) of the acid would the student need to prepare this buffer solution?
A student was required to prepare 250.0 mL of a cyanoacetic acid/sodium cyanoacetate buffer in which the concentration of the weak acid component was 0.067 M and the concentration of the conjugate base was 0.051 M. The student was supplied with 0.691 M cyanoacetic acid and 1.0M NaOH to perform this task. What volume (in mL) of the acid would the student need to prepare this buffer solution?
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
Chapter15: Acid-base Equilibria
Section: Chapter Questions
Problem 2RQ: Define a buffer solution. What makes up a buffer solution? How do buffers absorb added H+ or OH with...
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Transcribed Image Text:A student was required to prepare 250.0 mL of a cyanoacetic acid/sodium
cyanoacetate buffer in which the concentration of the weak acid
component was 0.067 M and the concentration of the conjugate base
was 0.051 M. The student was supplied with 0.691 M cyanoacetic acid
and 1.0M NaOH to perform this task. What volume (in mL) of the acid
would the student need to prepare this buffer solution?
Hint: assume that all of the conjugate base comes directly from the
reaction of NaOH with the weak acid (in other words, there is negligible
dissociation of the weak acid).
Please enter answers with 2 decimal places.
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