We’re being asked to calculate the equilibrium constant of HA if a 0.0538 M solution is 3.57% 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 HNO2 is as follows:
HA(aq) + H2O(l) ⇌ H3O+(aq) + A–(aq)
When a 0.0538 M solution of an unknown weak acid, HA, is made, only 3.57% acid ionized. What is the Ka of the unknown acid?
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