Calculation of pH of a Buffer Mixture

For Acidic Buffer mixture( Henderson- Hasselbalch equation)

For Basic Buffer mixture

pOH = pK_b + log [salt] / [Base]

pH + pOH =14

pOH = 14 – pH

pK_a + pK_b = 14

pK_b=14 – pK_a

14 – pH = 14 – pK_a + log [salt) / [base]

pH = pK_a – log [salt] / [base]

pH = pK_a + log [base] / [salt]

where K_a is the ionization constant of the conjugate acid of the base.

For example: In the buffer NH₄OH + NH₄Cl , NH₄⁺ is the conjugate acid of the base, NH₃ and Ka represents the ionization constant of the reaction:

NH₄⁺ (aq) + H₂O (l)  NH₃ (aq) + H⁺ (aq)

pH = pKa + log [NH₃] / [NH₄⁺]

pH = pKa + log [Base] / [conjugate acid]

 

Buffer Capacity

It is defined as the number of moles of an acid or a base required to be added to one litre of the buffer solution so as to change its pH by one unit.

Buffer Capacity = No. of moles of the acid or base added to 1 litre of the buffer / change in pH

Buffer capacity of a buffer is maximum when the concentration of the weak acid and its salt or weak base and its salt are equal i.e. when pH = pK_a  or pOH = pK_b 

Importance of Buffer Solution

(1) In biological processes

The pH of our blood is maintained constant inspite of various acid and base producing reactions going on in our body. The buffer action is due to the presence of carbonic acid , bicarbonate ion and carbon dioxide in the blood.

(2) In industrial processes

The use of buffers is an important part of many industrial processes, e.g.,

in electroplating, in the manufacture of leather, dyes, photographic materials.

(3) In analytical chemistry

(i) in the removal of acid radicals such as phosphate, oxalate and borate which interfere in the precipitation of radicals of group 3.

(ii) in complexometric titration

(iii) to calibrate the pH metres

(4) In bacteriological research, culture media are generally buffered to maintain pH required for the growth of the bacteria being studied.