4) What is the pH of a solution of 0.02M of Na2HPO4? The stepwise dissociation of H3PO4(aq) is described using these three acidity constants: pK₁₁= 2.1, pka2= 7.4, pka3= 12.4. (17 pts) a) Start by showing a speciation diagram. b) Write down the mass-balance, proton-balance, and charge-balance equations. c) What is the speciation of this solution at pH=4? d) What is the pH after you make up this solution to be 0.02M of Na2HPO4? e) Is this system open or closed with respect to phosphate? Why?
4) What is the pH of a solution of 0.02M of Na2HPO4? The stepwise dissociation of H3PO4(aq) is described using these three acidity constants: pK₁₁= 2.1, pka2= 7.4, pka3= 12.4. (17 pts) a) Start by showing a speciation diagram. b) Write down the mass-balance, proton-balance, and charge-balance equations. c) What is the speciation of this solution at pH=4? d) What is the pH after you make up this solution to be 0.02M of Na2HPO4? e) Is this system open or closed with respect to phosphate? Why?
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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Transcribed Image Text:4) What is the pH of a solution of 0.02M of Na2HPO4? The stepwise dissociation of
H3PO4(aq) is described using these three acidity constants: pK₁₁= 2.1, pka2= 7.4, pka3=
12.4. (17 pts)
a) Start by showing a speciation diagram.
b) Write down the mass-balance, proton-balance, and charge-balance equations.
c) What is the speciation of this solution at pH=4?
d) What is the pH after you make up this solution to be 0.02M of Na2HPO4?
e) Is this system open or closed with respect to phosphate? Why?
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