# Problem: ​Consider the titration of 100.0 mL of 0.200 M acetic acid (Ka = 1.8 x 10  -5) by 0.100 M KOH. Calculate the pH of the resulting solution after the following volumes of KOH have been added.b. 50.0 mL​

###### FREE Expert Solution

Step 1. Calculate the initial amounts.

molarity (volume) → moles

Recall:

$\mathbf{M}\mathbf{=}\frac{\mathbf{mol}}{\mathbf{L}}$

100 mL of 0.200 M CH3COOH

moles CH3COOH = 0.02 mol

93% (102 ratings) ###### Problem Details

Consider the titration of 100.0 mL of 0.200 M acetic acid (Ka = 1.8 x 10  -5) by 0.100 M KOH. Calculate the pH of the resulting solution after the following volumes of KOH have been added.

b. 50.0 mL

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 Acid Strong Base Titrations concept. You can view video lessons to learn Weak Acid Strong Base Titrations. Or if you need more Weak Acid Strong Base Titrations practice, you can also practice Weak Acid Strong Base Titrations practice problems.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Giles' class at VCU.

What textbook is this problem found in?

Our data indicates that this problem or a close variation was asked in Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition. You can also practice Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition practice problems.