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of a 0.7900M solution of aniline C6H5NH2 with a 0.2500M solution of HNO3 . The pKb of aniline is 9.37 . Calculate the pH of the base solution after the chemist has added 39.3mL of the HNO3

of a 0.7900M solution of aniline C6H5NH2 with a 0.2500M solution of HNO3 . The pKb of aniline is 9.37 . Calculate the pH of the base solution after the chemist has added 39.3mL of the HNO3

Chemistry
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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Question

An analytical chemist is titrating

99.1mL

of a

0.7900M

solution of aniline

C6H5NH2

with a

0.2500M

solution of

HNO3

. The

pKb

of aniline is

9.37

. Calculate the pH of the base solution after the chemist has added

39.3mL

of the

HNO3

solution to it.

 

Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of

HNO3

solution added.

 

Round your answer to

2

decimal places.

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