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Calculate the [H3O+] of the following polyprotic acid solution: 0.135 M H3C6H5O7. Express your answer using...

Calculate the [H3O+] of the following polyprotic acid solution: 0.135 M H3C6H5O7.

Express your answer using two significant figures.

Calculate the pH of this solution

Express your answer to two decimal places.

Expert Solution

For H₃C₆H₅O₇,

We have, ka1 = 7.5 x 10^-4 > ka2 = 1.7 x 10^-5 > ka3 = 4.0 x 10^-7

Here, the second and third dissociations are negligible when compared to the first one

H₃C₆H₅O₇ + H₂O H₂C₆H₅O₇- + H₃O+

Initial 0.135 M 0 0

Change -x x x

Equilibrium 0.135-x x x

Ka1 = 7.5 x 10^-4 = x²/(0.135-x) (x in the denominator can be neglected in comparison with 0.135 M)

Therefore,

x² = 1.08 x 10^-4

x = [H₃O⁺] = 0.01 M

pH = -log[H₃O⁺] = -log(0.01) = 2

pH = 2

queen_honey_blossom answered 1 year ago

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