An analytical chemist Is titrating 150.5 mL of a 0.1400M solution of aniline (CH,NH,) with a 0.4000M solutlon of HNO.. The p K, of anline is 9.37. Calculate the pH of the base solution after the chemist has added 17.1 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 = [||

An analytical chemist Is titrating 150.5 mL of a 0.1400M solution of aniline (CH,NH,) with a 0.4000M solutlon of HNO.. The p K, of anline is 9.37. Calculate the pH of the base solution after the chemist has added 17.1 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 = [||

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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An analytical chemist is titrating 83.7 mL of a 0.3300M solution of isopropylamine ((CH,) CHNH, with a 0.5300M 2 solution of HNO3. The p K, of isopropylamine is 3.33. Calculate the pH of the base solution after the chemist has added 42.4 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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Calculate pH for a weak acid/strong base titration. Determine the pH during the titration of 64.2 mL of 0.368 M hypochlorous acid 3.5x10-8) by 0.368 M NaOH at the following points. (Ka (a) Before the addition of any NaOH (b) After the addition of 15.0 mL of NaOH (c) At the half-equivalence point (the titration midpoint) (d) At the equivalence point (e) After the addition of 96.3 mL of NaOH
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please help on my buffers worksheet for chem
When titrating 125 mL of nitric acid HNO3 0.165 mol/L, with KOH 0.219 mol/L.a) What is the pH of the solution before starting the titration, and what volume of KOH (in mL) is required to reach the equivalence point?b) What is the pH of the solution after the addition of 44.5 mL of KOH solution?c) What is the pH of the solution at the equivalence point, and the pH of the solution after the addition of 200 mL of KOH solution?
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