Part A MISSED THIS? Read Section 18.2 (Pages 788 - 799) ; Watch KCV 18.2B, IWE 18.2. a solution that is 0.16 M in HCHO2 and 0.13 M in NaCHO2 (Ka(HCHO2) = 1.8 × 10-4) Use the Henderson-Hasselbalch equation to calculate the pH of each solution: Express your answer to two decimal places. pH = 3.52 Submit Previous Answers Request Answer X Incorrect; Try Again; 5 attempts remaining

Part A MISSED THIS? Read Section 18.2 (Pages 788 - 799) ; Watch KCV 18.2B, IWE 18.2. a solution that is 0.16 M in HCHO2 and 0.13 M in NaCHO2 (Ka(HCHO2) = 1.8 × 10-4) Use the Henderson-Hasselbalch equation to calculate the pH of each solution: Express your answer to two decimal places. pH = 3.52 Submit Previous Answers Request Answer X Incorrect; Try Again; 5 attempts remaining

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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Answer part a, b, c
I need help solving these
We add 10mL of 0.1M NaOH to 100mL of 0.1M CH3COOH/ 0.1M CH3COO^-. (Ka = 1.8 x10 ^-5). Using the Henderson-Hasselbach equation, pH=pKa + log [A-]/[HA] a) before the addition of NaOH b) after the addition of NaOH
Please answer both parts.