(First part of the question, this is just for reference: We want to calculate th

Question

(First part of the question, this is just for reference:

We want to calculate the concentrations of all species in a 0.56 M Na2SO3 (sodium sulfite) solution. The ionization constants for sulfurous acid are Ka1 = 1.4× 10–2 and Ka2 = 6.3× 10–8. Let's start by first calculating the concentration of the spectator ion, Na+ = ? )

Second part of the question: Write the appropriate equilibria and associate the correct Kb values. Remember we will want to calculate the concentrations of all species in a 1.02 M Na2SO3 (sodium sulfite) solution. The ionization constants for sulfurous acid are Ka1 = 1.4× 10–2 and Ka2 = 6.3× 10–8.

SO32-(aq) + H2O yields HSO3-(aq) + OH-(aq)

Kb value (25 degrees) = ?

HSO3-(aq) + H2O yields H2SO3(aq) + OH-(aq)

Kb value (25 degrees) = ?

NOTE: Please answer only the second part of the question. What are the Kb values for the given concentrations?

Explanation / Answer

SO32-(aq) + H2O yields HSO3-(aq) + OH-(aq)

Kb = Kw/Ka2

      = 1*10-14/6.3*10-8    = 1.58*10-6

HSO3-(aq) + H2O yields H2SO3(aq) + OH-(aq)

Kb = Kw/Ka1

      = 1*10-14/1.4*10-2    = 7.14*10-13

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