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Calculate the [H3O+] of each of the following H2SO4 solutions.
For a 0.50 M soln
How do I reach the answer? Do I have to use a ice table?

  • Chemistry -

    Not for the first H^+ since it is 100% ionized. The second H^+ is not 100% ionized (k2 is about 10^-2) and you need an ICE table for that. But it's a little more complicated than that.

  • Chemistry -

    As dilute as that is, assume all dissociation has taken place (you get two protons for each H2SO4 molecule)

    So the concentration of the H ions is 2*.5=1M
    and the answer.

    Now for more concentrated solutinos, you would have to use Keq and an ice table. I would do that for anything over 8M solutions.

    Remember: STrong acids (HCl, HNO3, H2SO4) "completely" dissociate in water solutions. IT is not exactly so, but it is very close.

  • Chemistry -

    how do i reach the answer then? what are my k values if i need to use a ice table

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