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What is the pH of a solution of 3.4 M H2A (Ka1 = 1.0 × 10^-6...

What is the pH of a solution of 3.4 M H2A (Ka1 = 1.0 × 10^-6 and Ka2 is 1.0 × 10^-10)?

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Answer #1

H2A concentration = 3.4 M

H2A -----------------> H+ + HA-

3.4                            0         0

3.4 - x                       x          x

Ka1 = x^2 / 3.4 - x

1.0 × 10^-6 = x^2 / 3.4 - x

x = 1.84 x 10^-3

[H+] = 1.84 x 10^-3 M

pH = -log [H+] = -log (1.84 x 10^-3)

      = 2.74

pH = 2.74

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