Question

Calculate the concentrations of all species in a 1.23 M Na2SO3 (sodium sulfite) solution. The ionization constants for sulfurous acid are Ka1 = 1.4× 10–2 and Ka2 = 6.3× 10–8.

Answer #1

First you need to calculate the final pH

Since you are adding the conjugate base lets do de analysis as a base:

the mass action equation, remember since it is for the base is Kb and

At the equilibrium the concentration of the OH is equal to
HSO_{3}^{-}

X=[OH]

C0=concentration added

Solving for X you get a quadratic equation that can be solved:

X=4.36x10^{-4}=OH

Remember

so H+=2.29x10-11

pH=10.64

Now using both mass action equations you can find the concentrations of the other compounds:

Calculate the concentrations of all species in a 0.470 M Na2SO3
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acid are Ka1 = 1.4× 10–2 and Ka2 = 6.3× 10–8.

Calculate the concentrations of all species in a 1.12 M Na2SO3
(sodium sulfite) solution. The ionization constants for sulfurous
acid are Ka1 = 1.4� 10�2 and Ka2 = 6.3� 10�8.
NA+ =
SO32- =
HSO3- =
H2SO3 =
OH- =
H+ =

Calculate the concentrations of all species in a 0.470 M Na2SO3
(sodium sulfite) solution. The ionization constants for sulfurous
acid are Ka1 = 1.4× 10–2 and Ka2 = 6.3× 10–8.
NA+
SO32-
HSO3-
H2SO3
OH-
H+

Calculate the concentration of all species in a 0.520 M solution
of H2SO3. The acid ionization constants for the acid are
Ka1=1.6×10−2 and Ka2=6.4×10−8.

Calculate the concentration of all species in a 0.490 M solution
of H2SO3. The acid ionization constants for the acid are
Ka1=1.6×10−2 and Ka2=6.4×10−8. Express your answer using two
significant figures. Enter your answers numerically separated by
commas. [H2SO3], [HSO−3], [SO2−3], [H3O+], [OH−] =

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of significant figures.

Calculate the concentrations of
H2C2O4,
HC2O4−,
C2O42−,
and H+ species in a 0.370
M oxalic acid solution
(Ka1 = 6.5
×10−2,
Ka2 = 6.1
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