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An aqueous solution containing 1.00 g of oxobutanedioc acid (FM 132.07) per 100 mL was titrated...

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Chemistry

An aqueous solution containing 1.00 g of oxobutanedioc acid (FM132.07) per 100 mL was titrated with 0.09432 M NaOH.

  1. Calculate the pH at th following volumes of added base:0.5Ve1, Ve1, 1.5Ve2,Ve2, 1.05Ve2
  2. Sketch the titration curve, using the values calculatedabove.
  3. Which equivalence point would be best to use in this titration(which one is not blurred)?

Ka1 = 2.56

Ka2 = 4.37

Ve1 = equivalence point 1

Ve2 = equivalence point 2

Answer & Explanation Solved by verified expert
4.5 Ratings (872 Votes)
Lets say oxobutanedoic acid H2A a weak diprotic acidH2A NaOHNaHA H2ONaHA NaOH Na2A H2O1 as we know at first half equivalence point a    See Answer
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