Deriving Henderson-Hasselbalch Equation Step by Step. The Relationship between pH, pKa, Titration Curve and Buffer Action of a Weak Acid. The Significance. Derivation of the Henderson –Hasselbalch Equation for weak base. B + HOH. BH . +. + OH. – or. B. –. + HOH. BH + OH. –. Either one works, but you have to be. Henderson–Hasselbalch equation describes the derivation of pH as a measure of acidity using the acid dissociation constant (pKa.

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By using this site, you agree to the Terms of Use and Privacy Policy. The above equation is called the Henderson-Hasselbalch equation. You might also like…. Why the pH of water is 7? Henderson-Hasselbalch equation is used mostly to calculate pH of solution which is obtained by eqiation known amount of acid equatiob conjugate base or neutralizing part of acid with strong base.

For the standard base equation: WikiProject Chemistry may be able to help recruit an expert.

This page was last edited on 19 Novemberat Browse more in Easy Biology Class…. Multiply both sides by [HF] and then divide both sides by [F-] to get by itself. The Derivqtion equation derived from the equilibrium expression of hydrofluoric acid.


Henderson–Hasselbalch equation

By our laws of logarithms, when two values are multiplied, it is the same as distributing the log to both values and taking the sum. The Henderson—Hasselbalch is mainly used for calculating the pH or pKa of a solution containing known quantities of a weak acid henderso its conjugate base.

When we prepare a solution by mixing 0.

Henderson-Hasselbalch equation can be also be used for pH calculation of polyprotic acids, as long as the consecutive pKa values differ by at least 2 better 3. More Biochemistry Lecture Notes…. Titration Curve of Weak Acid. A little more manipulation and we can rearrange the part of the equation highlighted in blue.

In the case of solutions containing not-so-weak acids or not-so-weak bases equilibrium concentrations can be far from those predicted by the neutralization stoichiometry. The first step in deriving the Henderson-Hasselbach equation hasselbwlch to set up your equilibrium expression.

From Wikipedia, the free encyclopedia. The more diluted the solution is, the more solution pH is dominated not by the presence of acetic acid hasselbaalch its conjugate base, but by the water auto dissociation. However, this approach is justifiable hasselbalfh many cases, it creates false conviction that the equation could be applied in all the situations which is not true Henderson-Hasselbalch equation is valid only when it contains equilibrium concentrations of acid and conjugate base.

So this equation can be rearranged to give the Henderson-Hasselbalch equation Fig. Using the properties of these terms at 25 degrees Celsius, one can synthesise an equation for pH of basic solutions in terms of p K a and pH: Our next steps are mathematical in nature.



Bracketed quantities such as [base] and [acid] denote the molar concentration of the henderdon enclosed. For ionizable groups that are able to deprotonate to a charge of -1 e.

Acid—base chemistry Equilibrium chemistry Equations Mathematics in medicine Enzyme kinetics. Taking drivation negative log of both sides of the equation gives.

The dissociation of water and relative water concentration itself is neglected as well. Please help improve this article by adding citations to reliable sources. The dissociation constant Ka of the above reaction will be: The equation is also useful for estimating the pH of a buffer solution and to ascertain the equilibrium pH in acid-base reactions which will be of use to calculate the isoelectric point pI of proteins.

We have already stated that hasseelbalch a buffer the best buffering pH is at its pKa.