Question

Derive Henderson equation .​

Answer 1

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$\huge \mathbb\fcolorbox{black}{lavenderblush}{Answer : ♡}$

Hendreson Equation :

• The equation that relates the pH of an aqueous solution of an acid to the acid dissociation constant of the acid, is known as the Henderson-Hasselbach equation. pH=pkA+log10[conjugate base][weak acid].

Importance :

• The Henderson-Hasselbalch equation describes the relationship between blood pH and the components of the H2 CO3 buffering system. This qualitative description of acid/base physiology allows the metabolic component to be separated from the respiratory components of acid/base balance.

Derivation :

1. Take the ionization reaction of a weak acid (HA):
2. ionization of acid
3. The dissociation constant Ka of the above reaction will be:
4. proton donor and proton acceptor
5. Dissociation constant is the ratio of the concentration of products by the concentration of reactants. The square brackets, [ ], denote ‘concentration’.
6. Then from the equation (2) take out the [H⁺] to the left side (solve for H⁺):
7. ph pka and buffer actionThen take the negative logarithm of both sides:
8. titration curve of weak acid
9. We know that the – log [H⁺] is pH and the – log Ka is pKa.
10. Substitute the pH and pKa in the equation (4):
11. what is pKa and ka
12. Now invert the -log [HA]/[A¯], which involves changing its sign to obtain the Henderson-Hasselbalch equation.
13. buffer action

[A¯] is the concentration of proton acceptor (it can accept the proton in a buffer.

[HA] is the concentration of proton donor (it can donate a proton in the buffer)

Thus the equation (6) can be better stated as:Hasselbalch equationThe above equation is called the Henderson-Hasselbalch equation.

Refer the attachment for the equations !

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