3) What is the pH of a 0.02 M solution of sodium propionate? (12 pts) Reaction of sodium propionate in water: Pr (aq) + H₂O (1) ⇒ HPr (aq) + OH-(aq) Ka= 10-4.⁹ *Hint* This is a Kb problem therefore you must convert Ka to Kb. You can assume that the sodium propionate dissociates completely from the propionate and is not involved in any other important reactions. a) Is this the conjugate base or an acid that you are adding to solution? b) Write down the Mass-Balance Relations, the Proton Balance Relation and the c) Equilibrium Relation. Calculate the pH using both an analytic method, and by drawing the predominance diagram. *Hint* [OH-]=[HPr].
3) What is the pH of a 0.02 M solution of sodium propionate? (12 pts) Reaction of sodium propionate in water: Pr (aq) + H₂O (1) ⇒ HPr (aq) + OH-(aq) Ka= 10-4.⁹ *Hint* This is a Kb problem therefore you must convert Ka to Kb. You can assume that the sodium propionate dissociates completely from the propionate and is not involved in any other important reactions. a) Is this the conjugate base or an acid that you are adding to solution? b) Write down the Mass-Balance Relations, the Proton Balance Relation and the c) Equilibrium Relation. Calculate the pH using both an analytic method, and by drawing the predominance diagram. *Hint* [OH-]=[HPr].
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
Related questions
Question
![3) What is the pH of a 0.02 M solution of sodium propionate? (12 pts)
Reaction of sodium propionate in water:
Pr (aq) + H₂O (1) ⇒ HPr (aq) + OH-(aq)
Ka= 10-4.⁹ *Hint* This is a Kb problem therefore you must convert Ka to Kb.
You can assume that the sodium propionate dissociates completely from the propionate
and is not involved in any other important reactions.
a) Is this the conjugate base or an acid that you are adding to solution?
b) Write down the Mass-Balance Relations, the Proton Balance Relation and the
c)
Equilibrium Relation.
Calculate the pH using both an analytic method, and by drawing the predominance
diagram. *Hint* [OH-]=[HPr].](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fdcef96bb-8ba9-493e-80de-a4b6e78a1db2%2Fce4dcf8d-ef53-403a-9211-7f1833b08dc9%2Fgw57hlr_processed.png&w=3840&q=75)
Transcribed Image Text:3) What is the pH of a 0.02 M solution of sodium propionate? (12 pts)
Reaction of sodium propionate in water:
Pr (aq) + H₂O (1) ⇒ HPr (aq) + OH-(aq)
Ka= 10-4.⁹ *Hint* This is a Kb problem therefore you must convert Ka to Kb.
You can assume that the sodium propionate dissociates completely from the propionate
and is not involved in any other important reactions.
a) Is this the conjugate base or an acid that you are adding to solution?
b) Write down the Mass-Balance Relations, the Proton Balance Relation and the
c)
Equilibrium Relation.
Calculate the pH using both an analytic method, and by drawing the predominance
diagram. *Hint* [OH-]=[HPr].
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