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After rearranging the expression defining the acid dissociation constant, and putting pH = −log 10 [H +], one obtains pH = pK a – log ( [AH]/[A −] ) This is a form of the Henderson-Hasselbalch equation. It can be deduced from this expression that when the acid is 1 % dissociated, that is, when [AH]/[A −] = 100, pH = pK a − 2
The Henderson–Hasselbalch equation was developed by two scientists, Lawrence Joseph Henderson and Karl Albert Hasselbalch. [2] Lawrence Joseph Henderson was a biological chemist and Karl Albert Hasselbalch was a physiologist who studied pH. [2] [3] In 1908, Lawrence Joseph Henderson [4] derived an equation to calculate the hydrogen ion ...
Lawrence Joseph Henderson (June 3, 1878 – February 10, 1942) was an American physiologist, chemist, biologist, philosopher, and sociologist. He became one of the leading biochemists of the early 20th century. His work contributed to the Henderson–Hasselbalch equation, used to calculate pH as a measure of acidity.
The pK a 1 ⁄ 2 is equal to the Henderson–Hasselbalch pK a (pK HH a ) if the titration curve follows the Henderson–Hasselbalch equation . [ 14 ] Most p K a calculation methods silently assume that all titration curves are Henderson–Hasselbalch shaped, and p K a values in p K a calculation programs are therefore often determined in this way.
This is the Henderson–Hasselbalch equation, from which the following conclusions can be drawn. At half-neutralization the ratio [A − ] / [HA] = 1 ; since log(1) = 0 , the pH at half-neutralization is numerically equal to p K a .
Karl Albert Hasselbalch (Danish pronunciation: [ˈkʰɑˀl ˈælˀpɐt ˈhæsl̩ˌpælˀk]; 1 November 1874 – 19 September 1962) was a Danish physician and chemist known for his work on the Henderson–Hasselbalch equation.
That is, when several buffers are present together in the same solution, they are all exposed to the same hydrogen ion activity. Hence, the pK of each buffer will dictate the ratio of the concentrations of its base and weak acid forms at the given pH, in accordance with the Henderson-Hasselbalch equation.
The pH can be calculated approximately by the Henderson–Hasselbalch equation: [1] = + where K a is the acid dissociation constant. 3. The pH at the equivalence point depends on how much the weak acid is consumed to be converted into its conjugate base.