B.sc 2nd year Book
Advance Inorganic Chemistry
(Page 1)

Electrodes

Reference electrodes:
(1) Hydrogen electrode:

In this chapter, the topic of Electrodes is explained through the concept of hydrogen electrodes. This electrode is built by bubbling H₂ gas in acid (such as HCl, H₂SO_4, or another mineral acid) as shown in figure 1.01.

The equilibrium in this case is represented as-

H⁺_(aq)   +  e^– ↔ 1 / 2 H_2(g)

In this case, the electrode is reversible with respect to the H⁺ ion. H₂ gas is non-conducting in nature hence noble metal like Pt is used for making electrical contact in the circuit and therefore the electrode is represented as-

Pt ; H₂(g) | H⁺

and the electrode reaction is written as

2H⁺ (aq)   +  2e^–—————–> H₂(g)

If the acid in Pt foil dipped contains 1-mole concentration of (H⁺) ion at 25°C then the electrode is called hydrogen electrode.

(i) Gases are difficult to handle

(ii) It is difficult to maintain the H⁺ ion concentration as 1M and the pressure of the gas at 1 atm.

(iii) The electrode is poisoned even by the presence of traces of impurities.

(2) Calomel electrode Hg- Hg₂ Cl₂ electrode:

Calomel electrode is simple and reliable. It is also used as reference electrode for determining electrode potentials and pH of the supplied solutions. This electrode consists of Hg, solid mercurous chloride; Hg₂Cl₂, and a saturated solution of KCl. This electrode is represented as-

Hg(I), Hg₂Cl₂(s); KCl (solution)

It is built by placing mercury of high degree of purity at the bottom of a glass tube having a side tube on either side. Hg is covered by a paste Hg₂Cl₂ (calomel). The saturated solution of KCl is introduced above the paste through the side tube. A platinum wire sealed into a glass tube serves to make electrical contact of the electrode with the circuit. The set up of calomel electrode is shown in figure 1.02.

This electrode is reversible with respect to Cl^– ions, i.e. when it acts as anode, the electrode reaction is written as

2Hg (1)  +  2 Cl (aq)——————————  Hg₂Cl₂(s)  +  2 e^–

and when it acts as the cathode, the reverse reaction takes place. If the electrode reaction involves reduction, the Hg²(ous) ion derived by Hg₂Cl2 would be discharged at the electrode, hence more and more of calomel would pass into the solution.

Its reduction potential depends upon the concentration of KCl solution used as given below-

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