• HF is a weak acid
• the anion in KF is the conjugate base
▪ F- → anion → conjugate base
- concentration of F- = concentration of KF
• The solution is composed of a weak acid and its conjugate base, therefore we have a buffer.
We can use the Henderson-Hasselbalch Equation to solve for pH.
Substitute in the Henderson-Hasselbalch equation:
Calculate the pH of a buffer that is 0.058 M HF and 0.058 M LiF. The Ka for HF is 3.5 x 10-4.
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