6. 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+): Only answer 6B
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Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.
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Bronsted Lowry Base In Inorganic Chemistry
Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.
6. 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+):
Only answer 6B
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