Problem: Calculate the pH of a solution that is 1.00 M HF and 0.20 M KF. Ka = 7.24 x 10-4a. 2.44b. 3.84c. 0.70d. 3.14e. 2.84

FREE Expert Solution

We’re being asked to calculate the pH of a solution that is 1.00 M HF and 0.20 M KF.

A solution that contains a weak acid and its conjugate base is a buffer solution. The pH of a buffer solution can be determined using the Henderson-Hasselbalch equation.

pH=pKa+log (conjugate baseweak acid)


Given solution:

The solution is composed of 1.00 M HF and 0.20 M KF.

 HF is a weak acid
 the anion in KF is the conjugate base

92% (25 ratings)
View Complete Written Solution
Problem Details

Calculate the pH of a solution that is 1.00 M HF and 0.20 M KF. Ka = 7.24 x 10-4

a. 2.44
b. 3.84
c. 0.70
d. 3.14
e. 2.84

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.