Buffer solution
Buffer Solution
A buffer solution (pronounced: /ˈbʌfər səˈluːʃən/) is a type of chemical solution that is capable of maintaining a nearly constant pH level, even when exposed to small amounts of an acid or base. This is achieved through the presence of a weak acid and its corresponding conjugate base or a weak base and its corresponding conjugate acid.
Etymology
The term "buffer" comes from the word "buffet," which means to lessen the impact. In the context of chemistry, a buffer solution lessens the impact of added acids or bases on the pH of the solution.
Composition
A buffer solution is composed of a mixture of a weak acid and its salt (which forms the conjugate base) or a weak base and its salt (which forms the conjugate acid). The most common examples of buffer solutions are acetate buffer (a weak acid and its salt) and ammonia buffer (a weak base and its salt).
Function
The primary function of a buffer solution is to resist changes in pH when small amounts of an acid or base are added. This is crucial in many biological systems, such as the human blood, where maintaining a constant pH is vital for proper physiological function.
Related Terms
- Acid: A substance that donates protons or hydrogen ions and/or accepts electrons.
- Base: A substance that can accept protons or donate a pair of valence electrons.
- pH: A measure of the hydrogen ion concentration of a solution.
- Conjugate acid: The species created when a base accepts a proton.
- Conjugate base: The species created when an acid donates a proton.
- Acetate buffer: A buffer solution composed of acetic acid and its conjugate base, acetate.
- Ammonia buffer: A buffer solution composed of ammonia and its conjugate acid, ammonium.
External links
- Medical encyclopedia article on Buffer solution
- Wikipedia's article - Buffer solution
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