An analytical chemist is titrating 59.5mL of a 0.8600M solution of aniline C6H5NH2 with a 0.07400M solution of HNO3. The pKb of aniline is 9.37. Calculate the pH of the base solution after the chemist has added 140.2mL 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.
An analytical chemist is titrating 59.5mL of a 0.8600M solution of aniline C6H5NH2 with a 0.07400M solution of HNO3. The pKb of aniline is 9.37. Calculate the pH of the base solution after the chemist has added 140.2mL 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.
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
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An analytical chemist is titrating 59.5mL of a 0.8600M solution of aniline C6H5NH2 with a 0.07400M solution of HNO3. The pKb of aniline is 9.37. Calculate the pH of the base solution after the chemist has added 140.2mL 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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