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What is the pH of a 1.61M solution of carbonic acid? Ka1 = 4.3 x 10-7...

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Chemistry

What is the pH of a 1.61M solution of carbonic acid? Ka1 = 4.3 x10-7 Ka2 = 5.6 x 10-11

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3.7 Ratings (484 Votes)

H2CO3 -----------------------> H + HCO3-

1.61                                      0            0 ---------------------> initial

1.61-x                                   x             x -------------------> equilibrium

Ka1 = [H+][HCO3-]/[H2CO3]

Ka1 = x^2 / 1.61-x

4.3 x 10^-7 = x^2 / 1.61-x

x^2 + 4.3 x 10^-7 x - 6.92 x 10^-7 = 0

x = 8.32 x 10^-4

[H+] = x = 8.32 x 10^-4 M

pH = -log [H+]

pH = -log (8.32 x 10^-4 )

pH = 3.08
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