Calculate the pH of a solution prepared by mixing 0.0730 mol of chloroacetic acid plus 0.0140 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 pKa of chloroacetic acid is 2.865. pH = 2.15 Then do the calculation with [HA] and [A¯] from Equations 9-21 and 9-22. [HA] = FHA [H*]+ [OH¯] (9-21) [A¯] = FA- + [H*] - [OH¯] (9-22) pH = 2.865 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 CICH, CO,H, 0.050 mol CICH,CO,Na, 0.060 mol HNO,, and 0.060 mol Ca(OH), . Ca(OH), provides 2 OH¯.

Calculate the pH of a solution prepared by mixing 0.0730 mol of chloroacetic acid plus 0.0140 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 pKa of chloroacetic acid is 2.865. pH = 2.15 Then do the calculation with [HA] and [A¯] from Equations 9-21 and 9-22. [HA] = FHA [H]+ [OH¯] (9-21) [A¯] = FA- + [H] - [OH¯] (9-22) pH = 2.865 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 CICH, CO,H, 0.050 mol CICH,CO,Na, 0.060 mol HNO,, and 0.060 mol Ca(OH), . Ca(OH), provides 2 OH¯.

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter15: Acid–base Equilibria

Section: Chapter Questions

Problem 30P

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