We’re being asked to calculate the acid ionization constant (Ka) for a monoprotic acid if a 0.142 M solution has a percent dissociation of 1.60%.
Recall that the percent ionization is given by:
(Let HA → monoprotic acid)
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 0.142 M solution of a monoprotic acid has a percent dissociation of 1.60%. Determine the acid ionization constant (Ka) for the acid.
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