Buffer solutions

The solution whose pH is not altered to any great extent by the addition of small quantities of either sirong acid (H⁺ ions) or a sirong base (OH^- ions) is called the buffer solution. This can also be defined as a solution of reserve acidity or alkalinity which resists change of  upon the addition of small amount of acid or alkali.

(1) Types of buffer solutions : There are two types of buffer solutions,

(i) Solutions of single substances : The solution of the salt of a weak acid and a weak base.

For example ammonium acetate (CH₃COONH₄), NH₄CN act as the buffer.

(ii) Solutions of Mixtures : These are further of two types,

(a) Acidic buffer : It is the solution of a mixture of a weak acid and a salt of this weak acid with a strong base.

Example : CH₃COOH + CH₃COONa

(b) Basic buffer : It is the solution of a mixture of a weak base and a salt of this weak base with a strong acid.

Example : NH₄OH + NH₄Cl

(2) Buffer action : Buffer action is the mechanism by which added H⁺ ions or OH^- ions are almost neutralised; so that pH practically remains constant. The reserved base of buffer neutralises the added H⁺ ions while the reserved acid of buffer neutralises the added OH^- ions.

(3) Examples of buffer solutions

(i) Phthalic acid + potassium hydrogen phthalate

(ii) Citric acid + sodium citrate.

(iii) Boric acid + borax (which is sodium tetraborate).

(iv) Carbonic acid (H₂CO₃) + sodium hydrogen carbonate (NaHCO₃). This system is found in blood and helps in maintaining pH of the blood close to 7.4 (pH value of human blood lies between 7.36 to 7.42; a change in the value of pH by 0.2 units can cause death).

(v) NaH₂PO₄ + Na₃PO₄

(vi) NaH₂PO₄ + Na₂HPO₄

(vii) Glycerine + HCl

(viii) The pH value of gastric juice is maintained between 1.6 to 1.7 due to buffer system 

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