We’re being asked **to determine the pH** of a **0.28 M weak acid that is 3.5% ionized**.

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

$\overline{){\mathbf{\%}}{\mathbf{}}{\mathbf{ionization}}{\mathbf{=}}\frac{\mathbf{\left[}{\mathbf{H}}_{\mathbf{3}}{\mathbf{O}}^{\mathbf{+}}\mathbf{\right]}}{\mathbf{[}\mathbf{HA}{\mathbf{]}}_{\mathbf{initial}}}{\mathbf{\times}}{\mathbf{100}}}$

Also recall that ** pH** is given by:

$\overline{){\mathbf{pH}}{\mathbf{=}}{\mathbf{-}}{\mathbf{log}}{\mathbf{\left[}}{{\mathbf{H}}}_{{\mathbf{3}}}{{\mathbf{O}}}^{{\mathbf{+}}}{\mathbf{\right]}}}$

A 0.28 M solution of a weak acid is 3.5% ionized. What is the pH of the solution?

1. 3.17

2. 1.46

3. 0.55

4. 2.01

5. 5.25

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