The Henderson–Hasselbalch equation was developed by Lawrence Joseph Henderson and Karl Albert Hasselbalch. [2] Henderson was a biological chemist and Hasselbalch was a physiologist who studied pH. [2][3] In 1908, Henderson [4] derived an equation to calculate the hydrogen ion concentration of a bicarbonate buffer solution, which rearranged looks like this:
The Henderson–Hasselbalch equation describes the derivation of pH as a measure of acidity (using pKa, the negative log of the acid dissociation constant) in biological and chemical systems. The …
Get the Henderson Hasselbalch equation and examples showing how to use it to calculate the pH of weak acids or weak bases.
What is the Henderson-Hasselbalch equation. How to use it. Learn its derivation, along with its limitations and a few example problems.
Explore the Henderson Hasselbalch Equation, how it links pH and pKa, and its practical uses in acid-base chemistry. Learn key steps and real-world examples.
2.2.1 Henderson–Hasselbalch equation The Henderson–Hasselbalch equation was developed independently by the American biological chemist L. J. Henderson and the Swedish physiologist K. A. Hasselbalch, for relating the pH to the bicarbonate buffer system of the blood (see next). In its general form, the Henderson–Hasselbalch equation is a useful expression for buffer calculations.
Learn the Henderson-Hasselbalch equation, its derivation, and how to calculate buffer pH with simple steps and real-life examples.
Take a look at the Henderson-Hasselbalch equation and a worked example that explains how to apply the equation.
AP Chemistry Topic 8.9 – Henderson–Hasselbalch Equation: calculate buffer pH from pKa and the [A−]/ [HA] ratio; understand why buffers keep pH nearly constant after small additions of acid or base.