please do 2nd part for Na2C2O4 Oxalic acid, H2C204 , has acid dissociationconstants of Ka1=5.90×10-2 andKa2=6.40x10-5.Calculate the pH andmolar concentrations of H2C204 , HC20-4and C202-4 at equilibrium for each of thesolutions.A 0.205 M solution of H2C204.pH=[H2C204]= M[HC204^-]= M[C204^-2]= MA 0.205 M solution of Na2C204.pH=[H2C2O4]= M[HC204^-]= M[C204^-2]= M

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A 0.205 M solution of Na2C204 . pH= [H2C204]= M [НC204^-]%3D М [C204^-2]= M

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter15: Acid–base Equilibria

Section: Chapter Questions

Problem 107AP

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Ionic Equilibrium

Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.

Arrhenius Acid

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Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.

Question

please do 2nd part for Na2C2O4

Oxalic acid, H2C204 , has acid dissociation
constants of Ka1=5.90×10-2 and
Ka2=6.40x10-5.Calculate the pH and
molar concentrations of H2C204 , HC20-4
and C202-4 at equilibrium for each of the
solutions.
A 0.205 M solution of H2C204.
pH=
[H2C204]= M
[HC204^-]= M
[C204^-2]= M
A 0.205 M solution of Na2C204.
pH=
[H2C2O4]= M
[HC204^-]= M
[C204^-2]= M

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