Problem: Calculate the percent ionization of propionic acid (C2H5COOH) in solutions of each of the following concentrations (Ka is given in Appendix D in the textbook).0.260 M

FREE Expert Solution

We’re being asked to calculate the percent ionization of a 0.260 M aqueous solution of C2H5COOH.


Recall that the percent ionization is given by:


% ionization=[H+][HA]initial×100


We're given the initial concentration, we need to solve for [H+] or [H3O+].


For this problem, we need to do these steps:

Step 1: Write an equation for the dissociation of C2H5COOH

Step 2: Set up an ICE table to calculate the H3O+ ion concentration.

Step 3: Write the Ka expression

Step 4: Calculate the percent ionization of C2H5COOH


Step 1: Since C2H5COOH has a low Ka value (1.3 x 10-5) , 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:

 C2H5COOH(aq) + H2O(l)  H3O+(aq) + C2H5COO(aq)Ka = 1.3 × 10–5


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Problem Details

Calculate the percent ionization of propionic acid (C2H5COOH) in solutions of each of the following concentrations (Ka is given in Appendix D in the textbook).

0.260 M

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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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