A solution of 0.0490 M HCIis used to titrate 29.0 ml of an ammonia solution of unknown concentration. The equivalence point is reached when 16.0 mL HCl solution have been added. (Assume KW = 1.01 e-14.) What was the original pH of the ammonia solution? Type your numeric answer and submit

A solution of 0.0490 M HCIis used to titrate 29.0 ml of an ammonia solution of unknown concentration. The equivalence point is reached when 16.0 mL HCl solution have been added. (Assume KW = 1.01 e-14.) What was the original pH of the ammonia solution? Type your numeric answer and submit

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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pKa
12.5 mL 25 mL
Volume added
[4] Equilibrium Point Calculations
Prelab 3
Homework Unanswered
A solution of 0.0490 M HCI is used to titrate 29.0 mL of an ammonia solution of unknown concentration. The equivalence
point is reached when 16.0 mL HCl solution have been added. (Assume KW = 1.01e-14.)
What was the original pH of the ammonia solution?
Type your numeric answer and submit
Unanswered 2 attempts left
Submi
E Fulls
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7:11 PM
3/22/202

A solution of 0.0490 M HCl is used to titrate 29.0 ml of an ammonia solution of unknown concentration. The equivalence
point is reached when 16.0 mL HCl solution have been added. (Assume KW = 1.01 e-14.)
What was the pH at the equivalence point?
Type your numeric answer and submit

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