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8. A titration of 200.0 ml of 1.00 M H;A was done with 1.38 M NAOH. For the diprotic acid H2A, Ka1 = 2.5 x 10, Kaz = 3.1 x 10. Calculate the pH after 100.0 mL of 1.38 M NAOH have been added. A) 9.05 B) 8.86 C) 5.14 D) 9.90 E) 4.95

8. A titration of 200.0 ml of 1.00 M H;A was done with 1.38 M NAOH. For the diprotic acid H2A, Ka1 = 2.5 x 10, Kaz = 3.1 x 10. Calculate the pH after 100.0 mL of 1.38 M NAOH have been added. A) 9.05 B) 8.86 C) 5.14 D) 9.90 E) 4.95

Introduction to Chemical Engineering Thermodynamics
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
Chapter1: Introduction
Section: Chapter Questions
Problem 1.1P
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8. A titration of 200.0 mL of 1.00 M HzA was done with 1.38 M NaOH. For the diprotic acid H2A, Kai = 2.5 x 10, Ka2 = 3.1 x 109. Calculate the pH after 100.0 mL of 1.38 M NaOH have been added. %3D A) 9.05 B) 8.86 C) 5.14 D) 9.90 E) 4.95 To J 9. Consider the titration of 300.0 ml of 0.577 M NH; (K, = 1.8 x 10) with 0.500 M HNO. After 150.0 mL !! of 0.500 M HNO, have been added, the pH of the solution is: A) 4.63 B) 11.37 C) 6.37 D) 9.37 MASSOG E) none of these
Transcribed Image Text:8. A titration of 200.0 mL of 1.00 M HzA was done with 1.38 M NaOH. For the diprotic acid H2A, Kai = 2.5 x 10, Ka2 = 3.1 x 109. Calculate the pH after 100.0 mL of 1.38 M NaOH have been added. %3D A) 9.05 B) 8.86 C) 5.14 D) 9.90 E) 4.95 To J 9. Consider the titration of 300.0 ml of 0.577 M NH; (K, = 1.8 x 10) with 0.500 M HNO. After 150.0 mL !! of 0.500 M HNO, have been added, the pH of the solution is: A) 4.63 B) 11.37 C) 6.37 D) 9.37 MASSOG E) none of these
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