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You are given 10.00mL of a solution of an unknown acid. The pH of this solution...

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Chemistry

You are given 10.00mL of a solution of an unknown acid. The pHof this solution is exactly 5.62. You determine that theconcentration of the unknown acid was 0.1224 M. You also determinedthat the acid was monoprotoic (HA). What is the Ka andpKa of your unknown acid?

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3.7 Ratings (386 Votes)

Given, 10.0 mL of 0.1224 M monoprotic acid

So, [HA] = 0.1224 M

pH = -log [H+] = 5.62

[H+] = 10^(-5.62)

[H+] = 2.4 x 10^-6 M

Now, let us put ICE table for the acid.

             HA   <-----------> A- +   H+

I          0.1224                 0         0

C          -x                       +x       +x

E         0.1224-x               +x       +x

But, [H+] = x = 2.4 x 10^-6

So, [HA] = 0.1224 - (2.4 x 10^-6) = 0.1223 M

[A-] = 2.4 x 10^-6 M

[H+] = 2.4 x 10^-6 M

Ka = [A-][H+] / [HA]

Ka = (2.4 x 10^-6)^2 / 0.1224

Ka = 4.70 x 10^-11

Pka = -log Ka

= -log (4.70 x 10^-11)

= 10.33
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