Part A Calculate the pH of a buffer solution that is 0.265 molal in CH3COOH (K₂ = 1.75 x 10-5) and 0.385 molal in CH3COONa using the Davies equation to calculate + at 298.15 K. Express your answer using two decimal places. pH = , Templates Symbols undo redo reset keyboard shortcuts 'help' help! AS 1 r Submit Request Answer Part B What pH value would you have calculated if you had assumed that 7+ = 1? Express your answer using two decimal places. pH = help r Templates Symbols undo redo reset keyboard shortcuts help ASA 1 Submit Request Answer

Part A Calculate the pH of a buffer solution that is 0.265 molal in CH3COOH (K₂ = 1.75 x 10-5) and 0.385 molal in CH3COONa using the Davies equation to calculate + at 298.15 K. Express your answer using two decimal places. pH = , Templates Symbols undo redo reset keyboard shortcuts 'help' help! AS 1 r Submit Request Answer Part B What pH value would you have calculated if you had assumed that 7+ = 1? Express your answer using two decimal places. pH = help r Templates Symbols undo redo reset keyboard shortcuts help ASA 1 Submit Request Answer

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

Chapter15: Acid-base Equilibria

Section: Chapter Questions

Problem 81E: Which of the indicators in Fig. 14-8 could be used for the titrations in Exercises 61 and 63?

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In the laboratory, a general chemistry student measured the pH of a 0.590 M aqueous solution of methylamine, CH3NH₂ to be 12.219. Use the Information she obtained to determine the K, for this base. Kb (experiment) = 5 R Submit Answer 800 F4 % 5 T G Retry Entire Group 9 more group attempts remaining FS Cengage Learning Cengage Technical Support A 6 Y H MacBook Air F6 & 7 ◄◄ U J F7 8 F8 K 1 9 eded for this question. F9 O F10 O P 1 4) F11 Previous Next> + 11 Save and Exit F12 1
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