# 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:

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?

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