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In the case of your laboratory titration of citric acid, you are dealing with a triprotic acid in which the pKa values are close together. Therefore the first and second equivalence points are not easily discernible in the titration, but the third equivalence point is, and one can use that value to analyze the titration curve. Following is an example of a triprotic acid with pK values closer than 3 units, and pK3 less than 10. You have a 20.0 mL solution of the triprotic acid, H3A, with a concentration of 0.128 M, and are titrating it with a 0.250 M solution of NaOH.

a) How many millimoles of H3A are you titrating?

b) How many millimoles of NaOH are required to complete the titration?

c) What volume of NaOH will be needed to completely titrate the acid?

d) What volume of NaOH will be needed to reach the first equivalence point

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Category:- Chemistry
Reference No.:- M9875289

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