a. Calculate the pH of a 0.0813M solution of hydrogen sulfide (H2S) where:H2S(ag) > H*(ag) + HS (ag)Ka1 = 1.0 x 107HS jag) > H*(ag)+ s2,(aa)Ka2 = 1.0 x 1019b. Calculate [S2] in the solution.1.

pH is defined as negative logarithm of hydrogen ion concentration and it is represented as pH =…

а. Calculate the pH of a 0.0813M solution of hydrogen sulfide (H2S) where: H2Stag) > H*(ag) + HS jag) HS (ag) > H*(ag) + s² iaa) Ka1 = 1.0 x 107 Ka2 = 1.0 x 1019 b. Calculate [S?] in the solution.

а. Calculate the pH of a 0.0813M solution of hydrogen sulfide (H2S) where: H2Stag) > H(ag) + HS jag) HS (ag) > H(ag) + s² iaa) Ka1 = 1.0 x 107 Ka2 = 1.0 x 1019 b. Calculate [S?] in the solution.

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter15: Solutions Of Acids And Bases

Section: Chapter Questions

Problem 15.124QE

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a. Calculate the pH of a 0.0813M solution of hydrogen sulfide (H2S) where:
H2S(ag) > H*(ag) + HS (ag)
Ka1 = 1.0 x 107
HS jag) > H*(ag)
+ s2,
(aa)
Ka2 = 1.0 x 1019
b. Calculate [S2] in the solution.
1.

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