We’re being asked to calculate the percent ionization of a 0.510 M formic acid solution.
Recall that the percent ionization is given by:
We know the initial concentration of formic acid (HCOOH), 0.510 M. We just need to find the concentration of H+ at equilibrium.
We can find the Ka value for formic acid from the textbook or from the internet, it is 1.8x10-4.
Since, its Ka value is less than 1, 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 formic acid (HCOOH) is as follows:
HCOOH(aq) + H2O(l) ⇌ H3O+(aq) +HCOO–(aq); Ka = 1.8x10-4
Calculate the percent ionization of formic acid solutions having the following concentrations.
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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.
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