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the titration of 301 mL of 0.501 M carbonic acid (H2CO3) (Ka1 = 4.3 x 10-7,...

the titration of 301 mL of 0.501 M carbonic acid (H2CO3) (Ka1 = 4.3 x 10-7, Ka2 = 5.6 x 10-11) with 2.1 M NaOH. What is the pH of the solution at the 2nd equivalence point? What will the pH of the solution be when 0.09694 L of 2.1 M NaOH are added to the 301 mL of 0.501 M carbonic acid?How many mL of the 2.1 M NaOH are needed to raise the pH of the carbonic acid solution to a pH of 5.978?

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queen_honey_blossom answered 2 years ago
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