Answered: 6D. Determine the pH of a 250.00 mL…

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

Chapter4: Stoichiometry: Quantitative Information About Chemical Reactions

Section: Chapter Questions

Problem 109GQ: (a) What is the pH of a 0.105 M HCl solution? (b) What is the hydronium ion concentration in a...

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Diprotic oxalic acid (HO2C−CO2H) ionizes in water as follows.
HO2C−CO2H + H2O  HO2C−CO2- + H3O+ Ka1= 5.62×10−2
HO2C−CO2- + H2O  -O2C−CO2- + H3O+ Ka2 = 5.42× 10−5
You may use the abbreviations H2A, HA- and A2- for HO2C−CO2H, HO2C−CO2- and -O2C−CO2-
respectively.
6A. Determine the pH, and the concentrations of [HO2C−CO2H], [HO2C−CO2-] and [-O2C−CO2-] in a
solution of 0.100 M aqueous oxalic acid (HO2C−CO2H) solution. Note that Ka1 is not too small compared to
the initial concentration (F) of oxalic acid.
6B. Estimate the pH of 0.10 M solution of potassium oxalate (HO2C−CO2- K+):

6C. Complete the following ladder diagram by marking the values of pKa1 and pKa2 and the dominant
species resulting from the ionization of oxalic acid (HO2CCO2H) in each pH region to determine the
dominant form at pH = 3.80.

6D. Determine the pH of a 250.00 mL buffer that is 0.100M oxalic acid (HO2CCO2H) and 0.150M
sodium oxalate (HO2CCO2Na).
Answer 6D

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