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An aqueous solution contains a mixture of .175 M HF (Ka = 7.2 x 10-4) and...

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Chemistry

An aqueous solution contains a mixture of .175 M HF(Ka = 7.2 x 10-4) and .250 M HNO2(Ka = 4.0 x 10-4). Calculate the pH of thissolution (express your pH to the hundredth position).

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4.4 Ratings (751 Votes)

-log Ka = pKa

For HF, pKa = - log (7.2 x 10-4) = 3.142

For HNO2, pKa = - log (4 x 10-4) = 3.397

HF is the deciding reagent for pH.

             HF       ---->      H+     +    F-

Initial         0.175 M                 0                0

Change      -x                      +x               +x

Equilibrium        0.175 - x                 x                  x

Ka = [H+][F-] / [HF]

7.2 x 10-4 = x2 / (0.175 - x)

0.00072 (0.175 - x) = x2

x = 0.0112 M

[H+] = 0.0112 M

pH = -log [H+] = 1.95
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