Answer to Question #47454 in Inorganic Chemistry for Eliza Maldonado
The next three (3) problems deal with the titration of 421 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.
1. What is the pH of the solution at the 2nd equivalence point?
2. What will the pH of the solution be when 0.1316 L of 2.1 M NaOH are added to the 421 mL of 0.501 M carbonic acid?
3. How many mL of the 2.1 M NaOH are needed to raise the pH of the carbonic acid solution to a pH of 6.019?
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