pH of a Buffer Solution (Henderson-Hasselbalch)

📊 intermediate

$$pH = pK_a + \log\left(\frac{[Salt]}{[Acid]}\right)$$,

Used to calculate the pH of a buffer solution consisting of a weak acid and its conjugate base.

Variables & Units

$pK_a$

Negative log of acid dissociation constant

Unit: Dimensionless

$[Salt]$

Concentration of conjugate base

Unit: $mol/L$

Key Information

📐 Derived From

Equilibrium constant expression $K_a$.

💡 Example

Calculating pH of an acetic acid/sodium acetate buffer.

🔧 Applications

Biochemical research and blood pH maintenance.

⚠️ Constraints

Assumes [Salt] and [Acid] are equilibrium concentrations.

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