For the diprotic weak acid H2A,Ka1-3.4x10-6 and Ka2=6.1×10-9.What is the pH of a 0.0500 M solutionof H2A? What are the equilibriumconcentrations of H2A and A2- in thissolution?Express Ka1 in terms of x, and thenshow the simplified expression (when xis assumed to be negligible comparedto to the initial concentration).Kal-A/B =C/Dnumerator A in complete expression:denominator B in completeexpression:numerator C in simplified expression:denominator D in simplifiedexpression:Also, give the numerical value of xusing the appropriate approximation.What is the pH of the solution if youstopped here?X:pH:

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Answered: For the diprotic weak acid H2A,…

For the diprotic weak acid H2A, Ka1-3.4×10–6 and Ka2=6.1×10-9. What is the pH of a 0.0500 M solution of H2A? What are the equilibrium concentrations of H2A and A2- in this solution?

Chemistry

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ISBN:9781305957404

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Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Question

For the diprotic weak acid H2A,
Ka1-3.4x10-6 and Ka2=6.1×10-9.
What is the pH of a 0.0500 M solution
of H2A? What are the equilibrium
concentrations of H2A and A2- in this
solution?
Express Ka1 in terms of x, and then
show the simplified expression (when x
is assumed to be negligible compared
to to the initial concentration).
Kal-A/B =C/D
numerator A in complete expression:
denominator B in complete
expression:
numerator C in simplified expression:
denominator D in simplified
expression:
Also, give the numerical value of x
using the appropriate approximation.
What is the pH of the solution if you
stopped here?
X:
pH:

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