chemistry

posted by .

Calculate the concentrations of all species in a 1.67 M Na2SO3 (sodium sulfite) solution. The ionization constants for sulfurous acid are Ka1 = 1.4× 10–2 and Ka2 = 6.3× 10–8.

I know how to find the Na^+ and SO3^-2 but I don't know how to find molarity of rest of it. Can you show me how to find molarity please? Show me how to find molarity for HSO3^- and I will do the rest of them when I get it.

[Na^+] = 3.34M
[SO3^-2] = 1.67M
[HSO3^-] =
[H2SO3] =
[OH^-] =
[H^+] =

  • chemistry -

    HSO3^- comes from the hydrolysis of SO3^2-.
    ..........SO3^2- + H2O ==> HSO3^- + OH^-
    I.........1.67...............0.......0
    C...........-x...............x.......x
    E........1.67-x..............x.......x

    Kb for SO3^2- = Kw/Ka2 for H2SO3 = (x)(x)/(SO3^2-)
    Substitute and solve for x = (OH^-) = (HSO3^-)

  • chemistry -

    I found all concentrations of all species except H2SO3. I keep getting wrong. The balanced equation is

    H2SO3 ---> H^+ + HSO3

    Is that correct?

  • chemistry -

    I would look at this. Yes, your equation is right and I think if you substitute the values for H^+ and HSO3^- you will get H2SO3. An easier way may be this way. Try it and let me know
    H2SO3 ==> 2H^+ + SO3^2- which isn't the way it ionizes BUT this can be used when one knows H^+ and SO3^2- as in this case.
    k1k2 = 0.014*6.3E-8 = (H^+)^2(SO3^=)/(H2SO3) and solve for (H2SO3).

  • chemistry -

    I finally got H2SO3 right.
    H2SO3 ---> 2H^+ + SO3^-2 is work this way finding the H2S03. Thank you so much for your help. I appreciated your help.

Respond to this Question

First Name
School Subject
Your Answer

Similar Questions

  1. Chemistry

    Calculate the concentrations of all species in a 0.810 M Na2SO3 (sodium sulfite) solution. The ionization constants for sulfurous acid are Ka1 = 1.4 x 10^-2 and Ka2 = 6.3 x 10^-8 so I'm trying to find Na, SO3 2-, HSO3-, H2SO3, OH-, …
  2. Chemistry

    Calculate the concentrations of all species in a 0.810 M Na2SO3 (sodium sulfite) solution. The ionization constants for sulfurous acid are Ka1 = 1.4 x 10^-2 and Ka2 = 6.3 x 10^-8 I calculated SO32- = 0.8096 M, HSO3- = 3.58E-4, H2SO3 …
  3. Chemistry

    Calculate the concentrations of all species in a 1.41 M Na2SO3 (sodium sulfite) solution. The ionization constants for sulfurous acid are Ka1 = 1.4× 10–2 and Ka2 = 6.3× 10–8. Na^+ = 2.82M SO3^2- = 1.40M HSO3^- = 0.00047M H2SO3 …
  4. Chemistry

    Calculate the concentrations of all species in a 1.41 M Na2SO3 (sodium sulfite) solution. The ionization constants for sulfurous acid are Ka1 = 1.4× 10–2 and Ka2 = 6.3× 10–8. Na^+ = 2.82M SO3^2- = 1.40M HSO3^- = 0.00047M H2SO3 …
  5. chemistry

    Calculate the concentrations of all species in a 0.690 M Na2SO3 (sodium sulfite) solution. The ionization constants for sulfurous acid are Ka1 = 1.4× 10–2 and Ka2 = 6.3× 10–8.
  6. Chemistry

    Consider a 0.10 M solution of a weak polyprotic acid (H2A) with the possible values of Ka1 and Ka2 given below, calculate the contributions to [H3O+] from each ionization step. Part 1: Ka1=1.0*10^-4 Ka2=1.0*10^-5 Part 2: Ka1=1.0*10^-4 …
  7. Chemistry

    Calculate the concentrations of all species in a 0.390 M Na2SO3 (sodium sulfite) solution. The ionization constants for sulfurous acid are Ka1 = 1.4× 10–2 and Ka2 = 6.3× 10–8. Species: Na+ SO3 2- HSO3 - H2SO3 OH- H+ Thanks! The …
  8. Chemistry

    Calculate the concentrations of all species in a 1.17 M Na2SO3 (sodium sulfite) solution. The ionization constants for sulfurous acid are Ka1 = 1.4× 10–2 and Ka2 = 6.3× 10–8. I found Na+ = 2.34 SO3^2- = 1.17 H2SO3 = 7.14 x10^-13 …
  9. chemistry

    Calculate the concentrations of all species in a 1.22 M Na2SO3 (sodium sulfite) solution. The ionization constants for sulfurous acid are Ka1 = 1.4× 10–2 M and Ka2 = 6.3× 10–8 M.
  10. chemistry

    Calculate the concentrations of all species present in a 0.100 M solution of weak polyprotic acid H3PO4. Ka1=7.5 x 10 ^-3, ka2 = 6.2 x 10 ^-8, Ka3= 3.6 x 10^-13 How the heck do I do this

More Similar Questions