Calculate the concentrations of all species in a 0.760 M Na2SO3 (sodium sulfite) solution. The ionization constants for sulfurousacid are Ka₁ = 1.4 × 10-2 and Ka2 = 6.3 × 10-8.© Macmillan Learning[Na] == 1.520[HSO3] =[OH-] =Σ[so] = 0.760Σ[H₂SO3] =Σ[H+] =×10TOOLSΣMΣ

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Answered: Calculate the concentrations of all…

Chemistry & Chemical Reactivity

10th Edition

ISBN:9781337399074

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 110GQ

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[OH-] = = [+H] M M
Calculate the concentrations of all species in a 0.940 M Na, SO, (sodium sulfite) solution. The ionization constants for sulfurous acid are Ka = 1.4 × 10-2 and K2 = 6.3 x 10-8. [Na*] = 1.88 M [so}] = 0.94 M –16 [HSO;] = 3.8 x10¬4 2.7 x10- M [H,SO,] M Incorrect [OH] = 3.8 x10 -4 [H*] = 11 2.6 x10 M M
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Calculate the concentrations of all species in a 0.940 M Na, SO, (sodium sulfite) solution. The ionization constants for sulfurous acid are Kal = 1.4 × 10-2 and K42 = 6.3 × 10–8. [Na*] = 1.88 [so}] = 0.94 M M [HSO;] = 3.8 x10 -4 1.65 x10-8 M [H,SO,] M Incorrect [OH] = 3.8 x10¬4 [H*] = 2.6 x10-11 M M
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Calculate the concentrations of all species in a 0.760 M Na2SO3 (sodium sulfite) solution. The ionization constants for sulfurous acid are Ka₁ = 1.4 × 10-2 and Ka2 = 6.3 × 10-8. © Macmillan Learning [Na] = = 1.520 [HSO3] = [OH-] = Σ [so] = 0.760 Σ [H₂SO3] = Σ [H+] = ×10 TOOLS Σ M Σ