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A large volume of 0.1560 M H₂SO3(aq) is treated with enough NaOH(s) to adjust the pH of the solution to 5.43. Assuming that the addition of NaOH(s) does not significantly affect the volume of the solution, calculate the final molar concentrations of H₂SO₂ (aq), HSO (aq), and SO2 (aq) in solution given that the Kai and K₁2 values are 1.50 × 10-² and 1.20 x 10-7, respectively.

A large volume of 0.1560 M H₂SO3(aq) is treated with enough NaOH(s) to adjust the pH of the solution to 5.43. Assuming that the addition of NaOH(s) does not significantly affect the volume of the solution, calculate the final molar concentrations of H₂SO₂ (aq), HSO (aq), and SO2 (aq) in solution given that the Kai and K₁2 values are 1.50 × 10-² and 1.20 x 10-7, respectively.

Chemistry & Chemical Reactivity
Chemistry & Chemical Reactivity
9th Edition
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter16: Principles Of Chemical Reactivity: The Chemistry Of Acids And Bases
Section: Chapter Questions
Problem 106GQ: The hydrogen phthalate ion, C8HsO4, is a weak acid with Ka = 3.91 106....
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A large volume of 0.1560 M H₂SO3(aq) is treated with enough NaOH(s) to adjust the pH of the solution to 5.43. Assuming that the addition of NaOH(s) does not significantly affect the volume of the solution, calculate the final molar concentrations of H₂SO3(aq), HSO3(aq), and SO3(aq) in solution given that the Kal and K₁2 values are 1.50 × 10-² and 1.20 x 10-7, respectively. [H₂SO3] = [HSO3] = [SO] = 1.54006 ×10-3 Incorrect M M M
Transcribed Image Text:A large volume of 0.1560 M H₂SO3(aq) is treated with enough NaOH(s) to adjust the pH of the solution to 5.43. Assuming that the addition of NaOH(s) does not significantly affect the volume of the solution, calculate the final molar concentrations of H₂SO3(aq), HSO3(aq), and SO3(aq) in solution given that the Kal and K₁2 values are 1.50 × 10-² and 1.20 x 10-7, respectively. [H₂SO3] = [HSO3] = [SO] = 1.54006 ×10-3 Incorrect M M M
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