We’re being asked **to calculate the percent ionization** of a **0.260 M aqueous solution of C _{2}H_{5}COOH**.

Recall that the ** percent ionization **is given by:

$\overline{){\mathbf{\%}}{\mathbf{}}{\mathbf{ionization}}{\mathbf{=}}\frac{\mathbf{\left[}{\mathbf{H}}^{\mathbf{+}}\mathbf{\right]}}{\mathbf{[}\mathbf{HA}{\mathbf{]}}_{\mathbf{initial}}}{\mathbf{\times}}{\mathbf{100}}}$

We're given the initial concentration, we need to solve for [H^{+}] or [**H _{3}O**

**For this problem, we need to do these steps:**

*Step 1:** Write an equation for the dissociation of C _{2}H_{5}COOH*

**Step 2****:** *Set up an ICE table to calculate the H _{3}O^{+}*

**Step 3****:** *Write the K _{a}*

**Step 4****:** Calculate the percent ionization of *C _{2}H_{5}COOH*

**Step 1**: Since **C _{2}H_{5}COOH** has a low K

The dissociation of HA is as follows:

C_{2}H_{5}COOH(aq) + H_{2}O(l) ⇌ H_{3}O^{+}(aq) + C_{2}H_{5}COO^{–}(aq); **K _{a} = 1.3 × 10^{–5}**

Calculate the percent ionization of propionic acid (C_{2}H_{5}COOH) in solutions of each of the following concentrations (K_{a} is given in Appendix D in the textbook).

0.260 *M*

Frequently Asked Questions

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.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Hurst's class at LSU.