Asked by Anonymous

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?
Answered by DrBob222
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.
Answered by bobpursley
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.
Answered by Anonymous
how do i reach the answer then? what are my k values if i need to use a ice table
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