college chemistry

posted by Aubree

Consider the titration of a 50.0 mL sample of a 0.100 M solution of the triprotic weak acid citric acid (H3C6H5O7) with 0.100 M KOH. For citric acid, the three (3) acid dissociation constant values are ka1 = 7.40x10-3, ka2 = 1.70x10-5, and ka3 = 4.00x10-7, respectively. Given this information, calculate the pH upon addition of each of the following volume of KOH to the citric acid solution during this titration:

1. DrBob222

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2. qwerty

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