A Buffer Solution is one which resists changes in pH when small quantities of an acid or an alkali are added to it. A buffer solution (more precisely, pH buffer or hydrogen ion buffer) is an aqueous solution consisting of a mixture of a weak acid and its conjugate base, or vice versa. Its pH changes very little when a small amount of strong acid or base is added to it. Buffer solutions are used as a means of keeping pH at a nearly constant value in a wide variety of chemical applications. Buffer solutions are necessary to keep the correct pH for enzymes in many organisms to work. Many enzymes work only under very precise conditions; if the pH moves outside of a narrow range, the enzymes slow or stop working and can denature. In many cases denaturation can permanently disable their catalytic activity.[3] A buffer of carbonic acid (H2 CO3) and bicarbonate (HCO−3) is present in blood plasma, maintaining a pH between 7.35 and 7.45 Industrially, buffer solutions are used in fermentation processes and in setting the correct conditions for dyes used in coloring fabrics.
General characteristics of a buffer solution
- It has a definite pH, i.e., it has reserve acidity or alkalinity.
- Its pH does not change on standing for long.
- Its pH does not change on dilution.
- Its pH is slightly changed by the addition of small quantity of an acid or a base.
Buffer capacity is maximum:
1When [Salt] = [Acid], i.e., pH = pKa for acid buffer
2When [Salt] = [Base], i.e., pOH = pKb for base buffer under above conditions, the buffer is called efficient.
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