Asked 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:
a) 25 mL KOH added
b) 50 mL KOH added
c) 75 mL KOH added
d) 100 mL KOH added
e) 125 mL KOH added

Answers

Answered by DrBob222
see below.
Answered by qwerty
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