Please, solve step by step. Thanks The problem describes a buffer system consisting of equal volumes of AH (0.185 M) and A⁻ (0.186 M), with an acid dissociation constant \( K_a = 4.68 \times 10^{-5} \). It asks by what amount the pH will change when 17.1 mL of 0.199 M NaOH is added to the buffer, resulting in a total volume of 228.6 mL. A negative value indicates a decrease in pH, while a positive value indicates an increase.The multiple-choice options for the pH change are:- minus 0.06- 0.15 (marked as the correct answer)- 0.2This educational resource can aid students in understanding buffer systems and the calculation of pH changes due to the addition of strong base or acid.

Answered: A buffer is made up from equal volumes…

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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The problem describes a buffer system consisting of equal volumes of AH (0.185 M) and A⁻ (0.186 M), with an acid dissociation constant \( K_a = 4.68 \times 10^{-5} \). It asks by what amount the pH will change when 17.1 mL of 0.199 M NaOH is added to the buffer, resulting in a total volume of 228.6 mL. A negative value indicates a decrease in pH, while a positive value indicates an increase.

The multiple-choice options for the pH change are:
- minus 0.06
- 0.15 (marked as the correct answer)
- 0.2

This educational resource can aid students in understanding buffer systems and the calculation of pH changes due to the addition of strong base or acid.

Expert Solution

Step 1: Defining buffer solution

Answer:

Buffer solution is a type of solution that resists the change in its pH on adding small quantity of acid or base. Solution of weak acid (HA) and its conjugate base (A^-) can act like a buffer solution.

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