We’re being asked to calculate pH of a 0.013 M solution of HF.
Since HA has a low Ka value, it’s a weak 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:
HF(aq) + H2O(l) ⇌ H3O+(aq) + F–(aq); Ka = 3.5×10-4
Find the pH of a 0.013 M solution of HF. (The value of Ka for HF is 3.5×104)
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