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Get the buffer definition and examples in chemistry. Learn how to choose buffers and calculate their pH range.
Buffers: Overview Buffers are aqueous solutions that can resist pH changes when acidic or basic components are added to a given solution. It is essential to maintain the pH (or hydrogen ion concentration) of the solution to carry out reactions or processes that demand specific pH ranges — pH is the negative logarithm of the hydrogen ion concentration. By definition, buffers are a mixture of ...
Buffers usually consist of a weak acid and its conjugate base, in relatively equal and "large" quantities. Calculations are based on the equation for the ionization of the weak acid in water forming the hydronium ion and the conjugate base of the acid. "HA" represents any weak acid and "A - " represents the conjugate base.
How Buffers Work To illustrate the function of a buffer solution, consider a mixture of roughly equal amounts of acetic acid and sodium acetate. The presence of a weak conjugate acid-base pair in the solution imparts the ability to neutralize modest amounts of added strong acid or base. For example, adding strong base to this solution will neutralize hydronium ion and shift the acetic acid ...