Henderson-Hasselbalch Equation

📊 intermediate

$$pH = pK_a + \log_{10}\left(\frac{[A^-]}{[HA]}\right)$$

Relates the pH of a buffer solution to the $pK_a$ and the ratio of conjugate base to acid concentrations.

Variables & Units

$pH$

Acidity of the solution

Unit: Dimensionless

$pK_a$

Acid dissociation constant

Unit: Dimensionless

$[A^-]$

Concentration of conjugate base

Unit: molar ($M$)

$[HA]$

Concentration of weak acid

Unit: molar ($M$)

Key Information

📐 Derived From

The acid dissociation constant ($K_a$) expression.

💡 Example

Calculating the pH of a blood buffer system.

🔧 Applications

Biochemistry and pharmaceutical formulation.

⚠️ Constraints

Assumes negligible water dissociation and low concentration.

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