A student needs to prepare a buffer solution with a pH of 5.86. Assuming a pką of 4.30, how many mL of 0.1 M NaOH would need to be added to 24.0 mL of 0.1 M HB to prepare this buffer? Please include a proper (abbreviated) unit. HINT : Use pH = pka + log ([B minus]/[HB]) or, if concentrations are the same, %3D pH = pkg + log (Volume of OH minus/ (Volume of HB minus Volume of OH minus) %3D

A student needs to prepare a buffer solution with a pH of 5.86. Assuming a pką of 4.30, how many mL of 0.1 M NaOH would need to be added to 24.0 mL of 0.1 M HB to prepare this buffer? Please include a proper (abbreviated) unit. HINT : Use pH = pka + log ([B minus]/[HB]) or, if concentrations are the same, %3D pH = pkg + log (Volume of OH minus/ (Volume of HB minus Volume of OH minus) %3D

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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Concept explainers

Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.

Question

**Buffer Preparation Problem**

A student needs to prepare a buffer solution with a pH of 5.86. Assuming a pKₐ of 4.30, how many mL of 0.1 M NaOH would need to be added to 24.0 mL of 0.1 M HB to prepare this buffer?

Please include a proper (abbreviated) unit.

**HINT:** Use pH = pKₐ + log ([B⁻]/[HB]) or, if concentrations are the same,

pH = pKₐ + log (Volume of OH⁻ / (Volume of HB minus Volume of OH⁻))

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