Establish the percent ionization equation and determine the acid ionization constant (Ka) for a monoprotic acid (9.0x10-2 M) which has a percent dissociation of 0.60%
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 HA is as follows:
HA(aq) + H2O(l) ⇌ H3O+(aq) + A–(aq)
A 9.0×10−2 M solution of a monoprotic acid has a percent dissociation of 0.60%.
Determine the acid ionization constant (Ka) for the acid.
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