State the ph of the solution at the equivalence point

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Reference no: EM13212087

The next three (3) problems deal with the titration of 461 mL of 0.501 M carbonic acid (H2CO3) (Ka1 = 4.3 x 10-7, Ka2 = 5.6 x 10-11) with 1.1 M NaOH.

What is the pH of the solution at the 2nd equivalence point?

What will the pH of the solution be when 0.2709 L of 1.1 M NaOH are added to the 461 mL of 0.501 M carbonic acid?

How many mL of the 1.1 M NaOH are needed to raise the pH of the carbonic acid solution to a pH of 5.935?

Reference no: EM13212087

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