In an experiment 0.1 M H3PO4 solution is titrated with the standardized 0.1 M NAOH by a chemist and obtained the graph above. The chemist observed the first end point at pH = 4.35 while observing the second end point at pH = 10.2 According to the given information, calculate Kal and Ka2 for phosphoric acid. 14.0 12.0 10.0 - 8.0 6.0 - 4.0 2.0 0.0 2.5 5.0 7.5 10.0 12.5 15.0 17.5 20.0 22.5 25.0 27.5 30.0 32.5 35.0 Hd

Introduction to Chemical Engineering Thermodynamics
8th Edition
ISBN:9781259696527
Author:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Publisher:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
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In an experiment 0.1 M H3PO4 solution is titrated with the standardized 0.1 M NaOH by a chemist and obtained the graph above. The chemist observed the first end point at pH = 4.35 while observing the second end point at pH = 10.2. According to the given information, calculate Ka1 and Ka2 for phosphoric acid.

In an experiment 0.1 M H3PO4 solution is titrated with the standardized 0.1 M N2OH by a chemist and
obtained the graph above. The chemist observed the first end point at pH = 4.35 while observing the
second end point at pH = 10.2. According to the given information, calculate Kal and Ka2 for phosphoric
acid.
14.0
12.0
10.0
8.0
6.0
4.0
2.0
0.0
2.5 5.0 7.5 10.0 12.5 15.0 17.5 20.0 22.5 25.0 27.5 30.0 32.5 35.0
Volume of 0100M NaOH ml
Hd
Transcribed Image Text:In an experiment 0.1 M H3PO4 solution is titrated with the standardized 0.1 M N2OH by a chemist and obtained the graph above. The chemist observed the first end point at pH = 4.35 while observing the second end point at pH = 10.2. According to the given information, calculate Kal and Ka2 for phosphoric acid. 14.0 12.0 10.0 8.0 6.0 4.0 2.0 0.0 2.5 5.0 7.5 10.0 12.5 15.0 17.5 20.0 22.5 25.0 27.5 30.0 32.5 35.0 Volume of 0100M NaOH ml Hd
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