Question

aalso, is there a way to figure this out without Ka and Kb values?

Consider the reaction shown. Using your knowledge of relative acid-base strengths and equilibrium, determine what you can about the size of Kc for the reaction. H3ASO3(aq) + HSO3(aq) <=> H2A503 (aq) + H2SO3(aq) Selected Answer: Correct Answer: Kc<1 Kc<1

Answer 1

Two acids used here > H₂S ez H₂ Seoz and and H₂ Asz se tyt HO OH Acid - H₂ Seuz Conjugate base -H Seoz HO TOH AS THt electron Acid - H₂ Asoz conjugate base = H2A39 Now, for H₂ Sez, due to the presence of a double bonded Oxygen which is highly withdra- -wing , its conjugate base is more stabilized as are charge is dispersed in H se on No such double bonded onggen is present for H₂ Asz. So are charge is not dispersed in its conjugate base. Ha Asog. So, H₂ Se ₂ is stronger Acid than to Also, H se oz is weaker base than H₂ A3 07 Now; from Bronsted- Lowery theory of Acid-base we know, reaction always proceeds from the direction of stronger Acid and bases towar warto weaker Acid and bases.

so favourable reaction , на Seo, + H, Aso, , H5eo, на A50 9 Backward reaction will be un favourable. to Asaz (aq) + It se og caq.) H₂ A 30₃ cag) + H₂Sea (aq.). will be unfavourable reaction.

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