### Preparing a pH 4.00 Buffer SolutionYou are tasked with preparing 100.0 mL of a buffer solution with a pH of 4.00. This requires the use of 0.100 M benzoic acid, which has a \( pK_a \) of 4.20, and 0.200 M sodium benzoate. The question at hand is: **How many milliliters of each solution should be mixed to prepare this buffer?****Input Values:**- **Benzoic acid:** 25.96 mL (marked as incorrect)- **Sodium benzoate:** 74.04 mL (marked as incorrect)### ExplanationIn this setup, you are trying to use the Henderson-Hasselbalch equation to determine the correct volumes of benzoic acid and sodium benzoate to mix in order to achieve the desired buffer pH:\[ \text{pH} = pK_a + \log \left( \frac{[\text{A}^-]}{[\text{HA}]} \right) \]- Where \( [\text{A}^-] \) is the concentration of the conjugate base (sodium benzoate).- \( [\text{HA}] \) is the concentration of the weak acid (benzoic acid).Your calculations should align with maintaining the correct ratio between these two components to achieve the desired pH.

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You need to prepare 100.0 mL of a pH 4.00 buffer solution using 0.100 M benzoic acid (pK, = 4.20) and 0.200 M sodium benzoate. How many milliliters of each solution should be mixed to prepare this buffer? benzoic acid: 25.96 Incorrect sodium benzoate: 74.04 Incorrect mL mL

You need to prepare 100.0 mL of a pH 4.00 buffer solution using 0.100 M benzoic acid (pK, = 4.20) and 0.200 M sodium benzoate. How many milliliters of each solution should be mixed to prepare this buffer? benzoic acid: 25.96 Incorrect sodium benzoate: 74.04 Incorrect mL mL

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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