We’re being asked to calculate the percent ionization of a 0.10 M and 0.010 M aqueous solution of HA.
Recall that the percent ionization is given by:
We know the initial concentration of HA. We just need to find the concentration of H+ at equilibrium.
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:
HA(aq) + H2O(l) ⇌ H3O+(aq) + A–(aq); Ka = 9.5 × 10–7
A certain weak acid, HA, has a Ka value of 9.5×10–7.
Calculate the percent dissociation of HA in a 0.10 M solution?
Calculate the percent dissociation of HA in a 0.010 M solution?
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