Explain the titration of carbonic acid

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Reference no: EM13211585

The next three (3) problems deal with the titration of 331 mL of 0.501 M carbonic acid (H2CO3) (Ka1 = 4.3 x 10-7, Ka2 = 5.6 x 10-11) with 1.5 M KOH.

a) What is the pH of the solution at the 2nd equivalence point?
b) What will the pH of the solution be when 0.1913 L of 1.5 M KOH are added to the 331 mL of 0.501 M carbonic acid?
c) How many mL of the 1.5 M KOH are needed to raise the pH of the carbonic acid solution to a pH of 6.598?

The next three (3) problems deal with the titration of 521 mL of 0.501 M carbonic acid (H2CO3) (Ka1 = 4.3 x 10-7, Ka2 = 5.6 x 10-11) with 1.9 M KOH.

a) What is the pH of the solution at the 2nd equivalence point?
b) What will the pH of the solution be when 0.2432 L of 1.9 M KOH are added to the 521 mL of 0.501 M carbonic acid?
c) How many mL of the 1.9 M KOH are needed to raise the pH of the carbonic acid solution to a pH of 6.714?

Reference no: EM13211585

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