In this exercise, using the Henderson-Hasselbach equation, you will be asked to make the necessary computations to prepare a buffer on your own. Choosing from various solutions with corresponding pK, values given on the table below, choose a pair that would be ideal for the preparation of a 100mL buffer solution with a pH of 9.02 a. Selection of the conjugate base pair solutions Using the table of pKa values, pick a pair of solutions appropriate for the preparation of the buffer with the desired pH. Reagent (0.1 M solutions) pka Ammonia 9.25 Acetic acid 4.75 Ammonium Chloride 9.24 Sodium acetate 4.75 Using the equation below, calculate the ratio of [base] to [acid] to get the buffer of desired pH. pH = pK, + log [base]/[acid] b. Chosen conjugate acid base pair: volume of 0.1 M acid needed: volume of 0.1 M base needed:
In this exercise, using the Henderson-Hasselbach equation, you will be asked to make the necessary computations to prepare a buffer on your own. Choosing from various solutions with corresponding pK, values given on the table below, choose a pair that would be ideal for the preparation of a 100mL buffer solution with a pH of 9.02 a. Selection of the conjugate base pair solutions Using the table of pKa values, pick a pair of solutions appropriate for the preparation of the buffer with the desired pH. Reagent (0.1 M solutions) pka Ammonia 9.25 Acetic acid 4.75 Ammonium Chloride 9.24 Sodium acetate 4.75 Using the equation below, calculate the ratio of [base] to [acid] to get the buffer of desired pH. pH = pK, + log [base]/[acid] b. Chosen conjugate acid base pair: volume of 0.1 M acid needed: volume of 0.1 M base needed:
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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![In this exercise, using the Henderson-Hasselbach equation, you will be asked to make the
necessary computations to prepare a buffer on your own. Choosing from various solutions with
corresponding pK, values given on the table below, choose a pair that would be ideal for the
preparation of a 100mL buffer solution with a pH of 9.02
a. Selection of the conjugate base pair solutions
Using the table of pKa values, pick a pair of solutions appropriate for the preparation of the buffer
with the desired pH.
Reagent (0.1 M solutions)
pka
Ammonia
9.25
Acetic acid
4.75
Ammonium Chloride
9.24
Sodium acetate
4.75
Using the equation below, calculate the ratio of [base] to [acid] to get the buffer of desired pH.
pH = pk + log [base]/[acid]
b. Chosen conjugate acid base pair:
volume of 0.1 M acid needed:
volume of 0.1 M base needed:](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F60242f42-493f-4bd0-82bb-acea33cb80f8%2F2e4000de-c8b7-4123-9d75-dd59f65fa751%2Ffp30sx_processed.jpeg&w=3840&q=75)
Transcribed Image Text:In this exercise, using the Henderson-Hasselbach equation, you will be asked to make the
necessary computations to prepare a buffer on your own. Choosing from various solutions with
corresponding pK, values given on the table below, choose a pair that would be ideal for the
preparation of a 100mL buffer solution with a pH of 9.02
a. Selection of the conjugate base pair solutions
Using the table of pKa values, pick a pair of solutions appropriate for the preparation of the buffer
with the desired pH.
Reagent (0.1 M solutions)
pka
Ammonia
9.25
Acetic acid
4.75
Ammonium Chloride
9.24
Sodium acetate
4.75
Using the equation below, calculate the ratio of [base] to [acid] to get the buffer of desired pH.
pH = pk + log [base]/[acid]
b. Chosen conjugate acid base pair:
volume of 0.1 M acid needed:
volume of 0.1 M base needed:
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