**Question:**Propionic acid, CH₃CH₂COOH, has a \( K_a = 1.34 \times 10^{-5} \). If 10.00 mL of 0.080 M propionic acid is mixed with 10.00 mL of 0.060 M KOH, what is the pH of the resulting solution?**Options:**- 4.40- 3.29- 3.44- 5.35- 4.87**Explanation:**The problem requires calculating the pH of a solution formed by mixing propionic acid with potassium hydroxide (KOH), a strong base. You will need to use the given \( K_a \) value for propionic acid and apply the concepts of acid-base reactions and buffer solutions. The options suggest possible pH values for the solution.

Answered: Image /qna-images/answer/5d6d79e8-8fd6-4886-8763-d76c722835cf.jpg

Propionic acid, CH3CH2COOH, has a Ka = 1.34 x 105. If 10.00 mL of 0.080 M propionic acid is mixed with 10.00 mL of 0.060 M KOH, what is the pH of the resulting solution? O 4.40 O 3.29 O 3.44 O 5.35 O 4.87

Propionic acid, CH3CH2COOH, has a Ka = 1.34 x 105. If 10.00 mL of 0.080 M propionic acid is mixed with 10.00 mL of 0.060 M KOH, what is the pH of the resulting solution? O 4.40 O 3.29 O 3.44 O 5.35 O 4.87

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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