Question

You need a strong acid for an experiment, and you are given a bottle that you are told contains a strong acid at 15.0 M concentration. (The name of the acid on the label was rubbed off, so you are not sure of the identity of the acid.) You make a 0.1 M solution and you want to know if you can assume that the [H+] will be 0.1 M since the acid is a strong acid and thus should (so you have been told) completely dissociate. You see that the label on the bottle lists a pKa for the acid of -6.9. A pKa. You decide that you better calculate the relative error that will result when you make the assumption that a 0.1 M solution of the strong acid will result in a 0.1 M [H+] versus the concentration that you obtain when you properly treat the dissociation using the listed pKa value. Normally, the relative error is expressed as follows: Er = ((xi – xt)/xt) × 100; where xi is the value under the assumption that complete dissociation occurs and xt is the true or actual value obtained when the pKa of the acid is taken into account. Now, the units for an answer that is expressed as a percent could equivalently be stated as “parts per hundred”. Because the value of ((xi – xt)/xt) is likely to be a small number, I want you to multiply this value by 109 rather than 102 (as shown in the above equation). Thus, your answer will be in terms of parts per billion (ppb), and you should report your answer in these terms to the nearest ones

*For this problem, you can ignore the contribution of H+ ions due to the autoproteolysis of water.

Answer 1

Let the acid is HA

The pKa = -6.9

Ka = 7.94 X 10⁶

It will dissociate as

                   HA ---> H+ + A-

Initial          0.1 M        0      0

Change      -x            x        +x

Equilibrium    0.1-x       x      x

Ka = 7.94 X 10⁶ =x² / (0.1-x)

7.94 X 10⁵ - 7.94 X 10⁶x = x²

x = 0.0999999987

xi = 0.1

xt = x = 0.0999999987

Er = ((xi – xt)/xt) × 10⁹ = 0.1 - 0.0999999987 X 10⁹/ 0.0999999987 = 13 ppb