Problem: Find the percent ionization of a 0.250 M solution of HC2H3O2. (Note: Ka = 1.8×10−5).

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We’re being asked to calculate the percent ionization of a 0.250 M solution of HC2H3O2


Recall that the percent ionization is given by:


% ionization=[H+][HA]initial×100


We know the initial concentration of HA, 0.10 M. 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 = 8.4 × 10–7


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Problem Details

Find the percent ionization of a 0.250 M solution of HC2H3O2. (Note: Ka = 1.8×10−5).

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What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Weak Acids concept. If you need more Weak Acids practice, you can also practice Weak Acids practice problems.