acid. 2. Hypochlorous acid, HC10, is a weak acid with Ka = 3.0 x 10-8 a. Compute the pH of the mixture after 0.094 moles of Naot is added to 1 L of a 0.155 M HC10 solution. b. Consider a mixture of 0.155 moles of HC10 and 0.184 moles of KC10 in 1 L of solution. Use the Henderson-Hasselbach equation to compute the pH of this buffer. c. Compute the pH of the mixture after 0.094 moles of NaOH is added to i L of the buffer solution described in part b. d. Compute the pH of the mixture after 0.194 moles of NAOH is added to 1 Lof the buffer solution described in part b.

acid. 2. Hypochlorous acid, HC10, is a weak acid with Ka = 3.0 x 10-8 a. Compute the pH of the mixture after 0.094 moles of Naot is added to 1 L of a 0.155 M HC10 solution. b. Consider a mixture of 0.155 moles of HC10 and 0.184 moles of KC10 in 1 L of solution. Use the Henderson-Hasselbach equation to compute the pH of this buffer. c. Compute the pH of the mixture after 0.094 moles of NaOH is added to i L of the buffer solution described in part b. d. Compute the pH of the mixture after 0.194 moles of NAOH is added to 1 Lof the buffer solution described in part b.

Chemistry & Chemical Reactivity

10th Edition

ISBN:9781337399074

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter16: Principles Of Chemical Reactivity: The Chemistry Of Acids And Bases

Section16.7: Calculations With Equilibrium Constants

Problem 16.8CYU: Calculate the pH after mixing 15 mL of 0.12 M acetic acid with 15 ml of 0.12 M NaOH. What are the...

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