Question #25163

What are the equilibrium concentrations of H2SO3, H+, HSO3−, and SO32−in a 0.050 M solution of sulfurous acid H2SO3 at 25 oC? For H2SO3 at 25 oC, Ka1 = 1.5×10−2 and Ka2 = 1.0×10−7

Expert's answer

Concentration of H_{2}SO_{3} is 0.050 M

Concentration of HSO_{3}^{-} is next:

K_{1}=[H^{+}][HSO_{3}^{-}]/[H_{2}SO_{4}][H^{+}]=[HSO_{3}^{-}]

K_{1}=[HSO_{3}^{-}]^2/[H_{2}SO_{4}]

[HSO_{3}^{-}]^2=K_{1}*[H_{2}SO_{4}]

[HSO_{3}^{-}]=(K_{1}*[H_{2}SO_{4}])^1/2

[HSO_{3}^{-}]=(0.015*0.05)^1/2=2.77*10^-2

The same with [SO_{4}^{2-}]

[SO_{3}^{2-}]=(K_{2}*[SO_{4}^{2-}])^1/2 = 5.26*10^-5

[H^{+}] is the sum of this two results

Concentration of HSO

K

K

[HSO

[HSO

[HSO

The same with [SO

[SO

[H

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