In many chemical reactions, especially in biological systems, it
is important to keep the pH or acidity within defined limits. The
bloodstream of humans is kept at pH = 7.4 + / - 0.2, and acidosis
or alkalosis outside this range can be fatal. (Those of you who
read Michael Crichton's novel The Andromeda Strain may recall that
the plot hinged on the alien life form in the victims' bloodstreams
being even more sensitive to pH than the infected humans were.)
pH control also is important in rontrolling enzyme activity. Most
enzymes have an optimum pH range in which they function best, with
sharply reduced efficiency outside this range. At too high or too
low pH, acidic and basic groups on the enzyme or on its substrate
molecules may pick up or lose extra protons, thereby altering the
charge distribution at the molecular surface and possibly making
a mating of enzyme and substrate difficult or impossible (see above).
Many industrial processes go most efficiently, or most rapidly,
at certain pH values. It is important to have some way of keeping
pH changes to a minimum. The answer is the use of acid-base buffers.
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