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With the titration of 281 mL of 0.501 M carbonic acid (H2CO3) (Ka1 = 4.3 x...

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Chemistry

With the titration of 281 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. How many mLof the 1.1 M NaOH are needed to raise the pH of the carbonic acidsolution to a pH of 6.019?

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4.2 Ratings (534 Votes)
H2CO3 NaOH NaHCO3 H2O pKa 637 NaHCO3 NaOH Na2CO3 H2O pKa 1025 Let y mL NaOH is needed to raise the pH of the carbonic acid solution to a pH of 6019 At this pH the reaction is governed by the first equation Concentration of H2CO3 after adding y mL NaOH 2810501 y11 281y 1408 11y281y Concentration of NaHCO3 after adding y mL NaOH 11 y 281y Mixture of    See Answer
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