Calculate the pH of a solution prepared by mixing 0.0720 mol of chloroacetic acid plus 0.0280 mol of sodium chloroacetate in 1.00 L of water. First do the calculation by assuming that the concentrations of HA and A equal their formal concentrations. The pK₂ of chloroacetic acid is 2.865. pH = Then do the calculation with [HA] and [A] from Equations 9-21 and 9-22. [HA] = FHA - [H+] + [OH-] [A] = FA- + [H+] - [OH-] pH = (9-21) pH = (9-22) Using first your head, and then the Henderson-Hasselbalch equation, find the pH of a solution prepared by dissolving all the following compounds in one beaker containing a total volume of 1.00 L: 0.170 mol CICH₂CO₂H, 0.030 mol CICH₂CO₂ Na, 0.070 mol HNO3, and 0.070 mol Ca(OH)₂. Ca(OH)₂ provides 2 OH-.

Calculate the pH of a solution prepared by mixing 0.0720 mol of chloroacetic acid plus 0.0280 mol of sodium chloroacetate in 1.00 L of water. First do the calculation by assuming that the concentrations of HA and A equal their formal concentrations. The pK₂ of chloroacetic acid is 2.865. pH = Then do the calculation with [HA] and [A] from Equations 9-21 and 9-22. [HA] = FHA - [H+] + [OH-] [A] = FA- + [H+] - [OH-] pH = (9-21) pH = (9-22) Using first your head, and then the Henderson-Hasselbalch equation, find the pH of a solution prepared by dissolving all the following compounds in one beaker containing a total volume of 1.00 L: 0.170 mol CICH₂CO₂H, 0.030 mol CICH₂CO₂ Na, 0.070 mol HNO3, and 0.070 mol Ca(OH)₂. Ca(OH)₂ provides 2 OH-.

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter16: Reactions Between Acids And Bases

Section: Chapter Questions

Problem 16.46QE

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