We’re being asked to calculate the equilibrium constant of an acid if a 0.010 M solution of an acid is 8.0% ionized.
Recall that the percent ionization is given by:
Remember that weak acids partially dissociate in water and that acids donate H+ to the base (water in this case).
The dissociation of the general acid HA is as follows:
HA(aq) + H2O(l) ⇌ H3O+(aq) + A–(aq)
A 0.010 M solution of an acid is 8.0% ionized. What is Ka for this acid?
A. 3.2 x 10-6
B. 2.8 x 10-5
C. 6.4 x 10-6
D. 7.0 x 10-5
E. 1.6 x 10-4
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