Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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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Given: A diprotic acid (H2A) has pKa1 = 2.8 and pKa2 = 8.4.
Question: What is the equilibrium constant for the conversion of
H2A to A2−?
![The image depicts a chemical equilibrium equation:
\[ \text{H}_2\text{A} \rightleftharpoons 2\text{H}^+ + \text{A}^{2-} \]
This equation represents the dissociation of a generic diprotic acid (H₂A) into two hydrogen ions (H⁺) and a divalent anion (A²⁻) in an aqueous solution. The double arrow indicates that the reaction is in equilibrium, meaning it can proceed in both forward and reverse directions under certain conditions.
Understanding this equation is essential in studying acid-base chemistry, particularly in analyzing how diprotic acids dissociate in solutions and affect pH levels.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F91195c14-8c67-42a0-b9d0-a3e8c2a59df0%2Fc0ae46f2-4723-4f67-99e6-ea093b3e002d%2Fohbpyrr_processed.png&w=3840&q=75)
Transcribed Image Text:The image depicts a chemical equilibrium equation:
\[ \text{H}_2\text{A} \rightleftharpoons 2\text{H}^+ + \text{A}^{2-} \]
This equation represents the dissociation of a generic diprotic acid (H₂A) into two hydrogen ions (H⁺) and a divalent anion (A²⁻) in an aqueous solution. The double arrow indicates that the reaction is in equilibrium, meaning it can proceed in both forward and reverse directions under certain conditions.
Understanding this equation is essential in studying acid-base chemistry, particularly in analyzing how diprotic acids dissociate in solutions and affect pH levels.
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