Problem: The acid-dissociation constant for benzoic acid (C6H5COOH) is 6.3x10 –5. Calculate the equilibrium concentration of C6H5COOH in the solution if the initial concentration of C6H5COOH is 0.061 M.

FREE Expert Solution

We’re being asked to calculate the equilibrium concentration of CH3COOH when its initial concentration is 0.061 M.


To solve this problem, we need to:

Step 1. Determine the dissociation of the acid in water.

Step 2. Construct the ICE chart.

Step 3. Determine the equilibrium concentration of CH3COOH



Step 1Since CH3COOH has a low Ka value, 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 CH3COOH is as follows:

90% (91 ratings)
View Complete Written Solution
Problem Details
The acid-dissociation constant for benzoic acid (C6H5COOH) is 6.3x10 –5. Calculate the equilibrium concentration of C6H5COOH in the solution if the initial concentration of C6H5COOH is 0.061 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 Jackson's class at SHC.