Posted by **Sarah** on Sunday, April 6, 2008 at 10:53pm.

Calculate the pH of the following aqueous solution:

1.00 mol/L sulfuric acid, H2SO4(aq)

H2SO4 ==> H^+ + HSO4^- 100%

HSO4^- ==> H^+ + SO4^= not 100%

(H^+) = 1.00 M for the first ionization.

The second one is guided by k2.

k2 = (H^+)(HSO4^-)/(HSO4^-)

Plug into k2 as follows:

(H^+) = 1.00 + x

(SO4^=) = x

(HSO4^-) = 1.00 - x

Solve for x.

k2 = (H^+)(HSO4^-)/(HSO4^-)

= (1.00 + x)(1.00 - x)/(1.00 -x)

=Im guessing the 1.00 cancels out?

.

- chemistry -
**DrBob222**, Sunday, April 6, 2008 at 11:27pm
You've omitted k2 for H2SO4. You must look up k2 and add it to the equation. And no, the 1+x and 1-x don't necessarily cancel.

- chemistry -
**DrBob222**, Sunday, April 6, 2008 at 11:34pm
If you work the quadratic (it can be done with successive approximations), the answer comes out to be (H^+) = 1.1072 which I would round to 1.11 M and take - log that for pH of about 1.97.

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