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
Answered by DrBob222
see below.
Answered by qwerty
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