Which of the following represents the relative fraction of species as a function of pH for the diprotic acid H2A with Ka1 = 7.9 x 10-6 and Ką2 = 6.3 x 10-8?Oa.H2AНА-A2-100755025O 2 46 8 10 12 14pHOb.НаА НА- А-1007550252 46 8 10 12 14pHC.H2AНА-A2-100755025O 2 4 6 8 10 12 14pHOd.H2AHA-A2-1007550250 2 4 6 8 10 12 14pHRelative fraction (%)Relative fraction (%)Relative fraction (%)Relative fraction (%)

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Which of the following represents the relative fraction of species as a function of pH for the diprotic acid H2A with Ka1 = 7.9 x 10-6 and Ka2 = 6.3 x 10-8? Oa. H2A НА- A2- S 100 75 50 25 4 8 10 12 14 pH Ob. НаА НА- А2- 100 75 50 25 6 8 10 12 14 pH 0 2 4 с. H2A НА- A2- S 100 75 50 25 O 2 4 6 8 10 12 14 pH d. H2A НА- A2- S 100 75 50 25 0 2 4 6 8 10 12 14 pH Relative fraction (%) Relative fraction (%) Relative fraction (%) Relative fraction (%)

Which of the following represents the relative fraction of species as a function of pH for the diprotic acid H2A with Ka1 = 7.9 x 10-6 and Ka2 = 6.3 x 10-8? Oa. H2A НА- A2- S 100 75 50 25 4 8 10 12 14 pH Ob. НаА НА- А2- 100 75 50 25 6 8 10 12 14 pH 0 2 4 с. H2A НА- A2- S 100 75 50 25 O 2 4 6 8 10 12 14 pH d. H2A НА- A2- S 100 75 50 25 0 2 4 6 8 10 12 14 pH Relative fraction (%) Relative fraction (%) Relative fraction (%) Relative fraction (%)

General, Organic, and Biological Chemistry

7th Edition

ISBN:9781285853918

Author:H. Stephen Stoker

Publisher:H. Stephen Stoker

Chapter10: Acids, Bases, And Salts

Section: Chapter Questions

Problem 10.30EP: Classify each of the acids in Problem 10-20 as a strong acid or a weak acid. a. H2SO4 (sulfuric...

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The pH of a 0.10-M solution of caffeine is 11.16. Determine Kb for caffeine from these data: C8H10N4O2(aq)+H2O(l)C8H10N4O2H+(aq)+OH(aq)
Two students were asked to determine the Kb of an unknown base. They were given a bottle with a solution in it. The bottle was labeled aqueous solution of a monoprotic strong acid. They were also given a pH meter, a buret, and an appropriate indicator. They reported the following data: volume of acid required for neutralization = 21.0 mL pH after 7.00 mL of strong acid added = 8.95 Use the students' data to determme the Kb of the unknown base.

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