An analytical chemist is titrating 139.8 mL of a 0.1600M solution of aniline (C,H,NH,) with a 0.6500M solution of HNO3. The p K, of aniline is 9.37. Calculate the pH of the base solution after the chemist has added 9.9 mL of the HNO, solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO, solution added. Round your answer to 2 decimal places. pH = ||

Given that, 139.8 mL of 0.1600 M of aniline was titrated with 0.6500 M solution of HNO3. The pKb of…

Answered: An analytical chemist is titrating 139.8 mL of a 0.1600M solution of aniline (C,H,NH,) with a 0.6500M solution of HNO3. The p K, of aniline is 9.37. Calculate…

Chemistry

10th Edition

ISBN: 9781305957404

Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher: Cengage Learning

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Question

An analytical chemist is titrating 139.8 mL of a 0.1600M solution of aniline (C,H,NH,) with a 0.6500M solution of HNO,. The p K, of aniline is 9.37.
Calculate the pH of the base solution after the chemist has added 9.9 mL of the HNO, solution to it.
Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO, solution added.
Round your answer to 2 decimal places.
pH
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Explanation
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