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An analytical chemist is titrating 178.7 mL of a 0.8900 M solution of trimethylamine ((CH3),N) with a 0.6500 M solution of HNO3. The p K, of trimethylamine is 4.19. Calculate the pH of the base solution after the chemist has added 136.7 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.

An analytical chemist is titrating 178.7 mL of a 0.8900 M solution of trimethylamine ((CH3),N) with a 0.6500 M solution of HNO3. The p K, of trimethylamine is 4.19. Calculate the pH of the base solution after the chemist has added 136.7 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.

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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Please round to 2 decimal places - my original answer was 4.29 which was marked incorrect.

 

 

An analytical chemist is titrating 178.7 mL of a 0.8900 M solution of trimethylamine \(((CH_3)_3 N)\) with a 0.6500 M solution of HNO₃. The \(pK_b\) of trimethylamine is 4.19. Calculate the pH of the base solution after the chemist has added 136.7 mL 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. ``` pH = [ ] [ x ] [ ↻ ] [ ? ] ```
Transcribed Image Text:An analytical chemist is titrating 178.7 mL of a 0.8900 M solution of trimethylamine \(((CH_3)_3 N)\) with a 0.6500 M solution of HNO₃. The \(pK_b\) of trimethylamine is 4.19. Calculate the pH of the base solution after the chemist has added 136.7 mL 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. ``` pH = [ ] [ x ] [ ↻ ] [ ? ] ```
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