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.)

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

Chapter16: Solubility And Precipitation Equilibria

Section: Chapter Questions

Problem 70AP

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