Chapter9: Acids, Bases, And Salts
Section: Chapter Questions
Problem 9.20E
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Question
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+):
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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