Chemistry
posted by Brian .
For a solution of 3.3 M H2CO3 (Ka = 4.4 × 107), calculate:
(a) [H+] ____?______M
(b) pH _____??______
(c) percent ionization ______?______%

Chemistry 
DrBob222
I don't think it wise to write the Ka for H2cO3 as 4.4E7 because it has TWO ionization constants. It is correct to write k1 = 4.4E7.
...........H2CO3 ==> H^+ + HCO3^
I.........3.3M.......0.......0
C.........x.........x.......x
E.........3.3x.......x......x
k1 = 4.4E7 = (H^+)(HCO3^)/(H2CO3)
Substitute into k1 exprsession and solve for x = (H^+) and convert that to pH.
% ion = [(H^+)/(H2CO3)]*100 = ?
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For a solution of 3.3 M H2CO3 (Ka = 4.4 × 107), calculate: (a) [H+] ____?