Buffer Solution
| Formula / Notation | pH = pKa + log([A⁻]/[HA]) (Henderson-Hasselbalch equation) |
|---|---|
| Also Known As | pH buffer, buffer system, acid-base buffer, biological buffer |
What is Buffer Solution?
A buffer solution is an aqueous solution that resists changes in pH upon addition of small amounts of acid or base. It consists of a weak acid and its conjugate base (or a weak base and its conjugate acid) in similar concentrations. Buffer solutions are critical in biological systems (blood pH ≈ 7.4), analytical chemistry, and fermentation processes.
Formula & Notation
Other Names / Synonyms: pH buffer, buffer system, acid-base buffer, biological buffer
Properties & Characteristics
Uses & Applications
Safety Information
Always consult the SDS/MSDS before handling any chemical. This information is for educational purposes only.
Key Facts
Frequently Asked Questions
A buffer solution is an aqueous solution that resists changes in pH upon addition of small amounts of acid or base. It consists of a weak acid and its conjugate base (or a weak base and its conjugate acid) in similar concentrations. Buffer solutions are critical in biological systems (blood pH ≈ 7.4), analytical chemistry, and fermentation processes.
Buffer solutions are used in analytical chemistry (calibrating pH meters), biochemistry (enzyme assays, cell culture media), pharmaceutical formulations, food preservation, and industrial fermentation. The Sørensen phosphate buffer and TRIS buffer are standard laboratory reagents.
Buffer components themselves are generally of moderate toxicity, but concentrated strong acid or base used to prepare buffers are corrosive. Some biological buffers (e.g., TRIS) can interfere with certain assays. Always label buffer concentrations and pH; do not confuse with other solutions.
The formula or notation for Buffer Solution is: pH = pKa + log([A⁻]/[HA]) (Henderson-Hasselbalch equation)