Calculating the pH at equivalence of a titrationA chemist titrates 50.0 mL of a 0.5851 M ethylamine (C2H5NH2) solution with 0.8192M HBr solution at 25 °C. Calculate the pH atequivalence. The pK of ethylamine is 3.19.bRound your answer to 2 decimal places.Note for advanced students: you may assume the total volume of the solution equals the initial volume plus the volume of HBr solutionadded.pH = ]☑

Step 1:Firstly, volume of strong acid to reach the equivalence, is calculated. Step 2: Then…

Answered: Calculating the pH at equivalence of a…

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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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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A chemist titrates 240.0 mL of a 0.3902 M lidocaine (C14H₂, NONH) solution with 0.7622 M HBr solution at 25 °C. Calculate the pH at equivalence. The pK of lidocaine is 7.94. Round your answer to 2 decimal places. Note for advanced students: you may assume the total volume of the solution equals the initial volume plus the volume of HBr solution added. pH = 0 X
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A chemist titrates 80.0 mL of a 0.3825 M ethylamine (C2H5NH2) solution with 0.8602 M HBr solution at 25 °C. Calculate the pH at equivalence. The pK, of ethylamine is 3.19. Round your answer to 2 decimal places. Note for advanced students: you may assume the total volume of the solution equals the initial volume plus the volume of HBr solution added. pH = ☐ ×

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