Sulfuric acid, H2SO4, readily dissociates into H* and HSO, ions: H2SO4 H† + HSO7. The hydrogen sulfate ion, in turn, can dissociate again: HSO, H* + so?-. The equilibrium constants for these reactions, in aqueous solutions at 298 K, are approximately 102 and 10-1.9, respectively. (For dissociation of acids it is usually more convenient to look up K than AG°. By the way, the negative base-10 log- arithm of K for such a reaction is called pK, in analogy to pH. So for the first reaction pK = -2, while for the second reaction pK = 1.9.)
Sulfuric acid, H2SO4, readily dissociates into H* and HSO, ions: H2SO4 H† + HSO7. The hydrogen sulfate ion, in turn, can dissociate again: HSO, H* + so?-. The equilibrium constants for these reactions, in aqueous solutions at 298 K, are approximately 102 and 10-1.9, respectively. (For dissociation of acids it is usually more convenient to look up K than AG°. By the way, the negative base-10 log- arithm of K for such a reaction is called pK, in analogy to pH. So for the first reaction pK = -2, while for the second reaction pK = 1.9.)
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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At what pH would dissolved sulfate be equally distributed between HSO4 and SO24- ?
Transcribed Image Text:Sulfuric acid, H2SO4, readily dissociates into H* and HSO, ions:
H2SO4 H† + HSO7.
The hydrogen sulfate ion, in turn, can dissociate again:
HSO,
H* + so?-.
The equilibrium constants for these reactions, in aqueous solutions at 298 K, are
approximately 102 and 10-1.9, respectively. (For dissociation of acids it is usually
more convenient to look up K than AG°. By the way, the negative base-10 log-
arithm of K for such a reaction is called pK, in analogy to pH. So for the first
reaction pK = -2, while for the second reaction pK = 1.9.)
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