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