# Concentrations of acids and bases?

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Calculate the concentrations of all species in a 1.70 M Na2SO3 (sodium sulfite) solution. The ionization constants for sulfurous acid are Ka1 = 1.4× 10–2 and Ka2 = 6.3× 10–8.

Na+

SO3^2-

HSO3^-

H2SO3

OH-

H+

Any help would be appreciated

Calculate the concentrations of all species in a 1.70 M Na2SO3 (sodium sulfite) solution. The ionization constants for sulfurous acid are Ka1 = 1.4× 10–2 and Ka2 = 6.3× 10–8.

Na+

SO3^2-

HSO3^-

H2SO3

OH-

H+

Any help would be appreciated

##### 1 Answer

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#### Explanation

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See Below

#### Explanation:

Ok, I'll start with the easy one.

[Na+] = 2x1.7M = 3.4M

Now you have

You are given the Ka values, but for this instance, you need the Kb (using Ka2)

ICE table

I 1.7 0 0

C -x +x +x

E 1.7(assumption) +x +x

x = 0.000519

The next step is sort of strange. I don't really know any better way to determine this other than using the Henderson Hasselbalch equation (don't want to break out my Quantitative Analysis book)

I'm going to pretend that

This is obviously a very small amount of

All the Parts

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