Problem: Calculate the pH of a solution that is 0.111 M CH3COOH and 0.558 M CH3COONa. Ka of CH3COOH is 1.8 x 10-5.a. 5.45b. 5.02c. 5.67d. 6.91e. 6.82

FREE Expert Solution

We’re being asked to calculate the pH of a solution that is 0.111 M CH3COOH and 0.558 M CH3COONa.

In this case, we will be using the Henderson-Hasselbalch equation which can be used for buffer solutions

Recall the Henderson-Hasselbalch equation:

pH=pKa+logconjugate baseweak acid


85% (363 ratings)
View Complete Written Solution
Problem Details

Calculate the pH of a solution that is 0.111 M CH3COOH and 0.558 M CH3COONa. Ka of CH3COOH is 1.8 x 10-5.

a. 5.45

b. 5.02

c. 5.67

d. 6.91

e. 6.82

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 Buffer concept. You can view video lessons to learn Buffer. Or if you need more Buffer practice, you can also practice Buffer practice problems.

What is the difficulty of this problem?

Our tutors rated the difficulty ofCalculate the pH of a solution that is 0.111 M CH3COOH and 0...as medium difficulty.