One use of conjugate acids and bases lies in buffering systems, which include a
buffer solution. In a buffer, a weak acid and its conjugate base (in the form of a salt), or a weak base and its conjugate acid, are used in order to limit the pH change during a titration process. Buffers have both organic and non-organic chemical applications. For example, besides buffers being used in lab processes, human blood acts as a buffer to maintain pH. The most important buffer in our bloodstream is the
carbonic acid-bicarbonate buffer, which prevents drastic pH changes when is introduced. This functions as such: CO2 + H2O H2CO3 HCO3^- + H+ Furthermore, here is a table of common buffers. A second common application with an organic compound would be the production of a buffer with acetic acid. If acetic acid, a weak acid with the formula , was made into a buffer solution, it would need to be combined with its conjugate base in the form of a salt. The resulting mixture is called an acetate buffer, consisting of aqueous and aqueous . Acetic acid, along with many other weak acids, serve as useful components of buffers in different lab settings, each useful within their own pH range.
Ringer's lactate solution is an example where the conjugate base of an organic acid,
lactic acid, is combined with sodium, calcium and potassium cations and chloride anions in distilled water which together form a fluid which is
isotonic in relation to human blood and is used for
fluid resuscitation after
blood loss due to
trauma,
surgery, or a
burn injury. ==Table of acids and their conjugate bases==