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Water Electrolysis

Water electrolysis is a popular method used for different applications in various industries, mainly in the food industry, metallurgy, and power plants, amongst others. Besides, the components of water, which include hydrogen and oxygen, have many applications. For instance, hydrogen obtained through electrolysis is a clean, renewable and efficient fuel source.

Water electrolysis is mainly carried out to yield pure hydrogen and oxygen gases. It involves passing an electric current through the water, which results in the decomposition of water into hydrogen and oxygen.

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However, the electrolysis of water is not easy for many reasons.

  • Water is very weakly dissociated into hydrogen and hydroxide ions. The concentration of the ions in neutral water is equal (= moles per litre). Electrolysis involves the charge carriers for the current to flow. So, water with a very small amount of ions is a bad conductor of electricity. Therefore, the electrolysis of pure water will be a very slow process.
  • The hydrogen ion is associated with other water molecules and exists as a hydronium ion. So, any hydroxide ion moving towards the anode will be neutralised by the hydronium ion, even before it reaches the anode, to form oxygen gas. Similarly, any hydrogen present will be neutralised by the hydroxyl ion present near the cathode and will not be reduced to hydrogen. So, the electrolysis of water to hydrogen and oxygen will be very small. Electrolysis also involves the transfer of electrons from the anion to the anode and cathode to cations.
  • In the electrolysis of water, electrodes are inert solids like platinum/palladium, whereas an electrolyte is a solute in a solution, and the product is a gas.

Factors Affecting the Efficiency of Electrolysis

The efficiency of electrolysis or electron transfer depends on many factors, such as

i) The number of available cations and anions in the solution.

ii) Mobility rate of the ions to reach the electrode.

iii) Activation energy that is needed for the electron transfer from the electrode to the electrolyte ions.

iv) The effect of the gas bubble surrounding the electrode on the further electrotransfer, etc.

Crossing over several interfaces (solute-liquid, solute-solid, solid-gas) results in an increase of energy requirements for the electrolysis (overvoltage) than predicted by the thermos-dynamical Gibbs energy.

Also Read: Gibbs Free Energy

Principle of Water Electrolysis

Two electrodes or plates that are made from an inert metal such as platinum or iridium are placed in the water. A DC electrical power source is connected to these plates. At the cathode (where electrons enter the water), part hydrogen will appear. On the anode side, oxygen will appear. If we consider the ideal faradaic efficiency, hydrogen will be produced twice the amount of oxygen. On the other hand, both will be proportional to the total electrical charge conducted by the solution. However, in some cells, side reactions can occur, and different products are formed with less than ideal faradaic efficiency.

Electrolysis of Water-Cell Potential and Thermodynamic Feasibility

Half reactions in the electrolysis of pure water at pH = 7, and at 25°Care-

At cathode: 2H2O(l) + 2e → H2(g) + 2OH E° = -0.42 V

At anode: 2H2O → O2(g) + 4H+ + 4e E° = +0.82 V

The net reaction of electrolysis of water is given as,

2H2O(l) → 2H2(g) + O2(g) E° = -1.24 V

The cell potential of electrolysis of pure water is negative, and hence is thermodynamically unfavourable. Because of the low concentration of ions and the interfaces to be crossed electrons, an extra voltage (Overvoltage) at each electrode is needed to about 0.6V.

In practice, continuous electrolysis of pure water is possible only at an external voltage of 2.4V. Since the electrolysis of pure water is thermodynamically non-feasible, methods to make it kinetically feasible are being investigated.

One of the methods is to increase the conductivity by increasing the number of ions available by adding acid, base, or non-reacting salts.

Electrolyte for Water Electrolysis

It is very important to choose the right electrolyte for water electrolysis. Why is it important? If we look at the anion from the electrolyte, it usually competes with the hydroxide ions to release an electron. If an electrolyte anion has a less standard electrode potential than hydroxide, it will be oxidised instead of the hydroxide. Therefore, oxygen will not be produced. In the case of a cation, if it has a greater standard electrode potential than a hydrogen ion, it will be reduced. In this case, hydrogen gas will not be produced.

Water Electrolysis in the Presence of Acids (pH lower than 7)

Additional hydrogen ions from acid will be reduced at the cathode, while water will be oxidised at the anode. Half reactions in an acid medium are,

At cathode: 2H+ + e → H2 E° = +0.0 V

At anode: 2H2O → O2(g) + 4H+ + 4e E° = +1.23 V

Net reaction is written as 2H2O → O2(g) + 2H2 E° = -1.23 V

The electrolysis takes place at a much lower potential than pure water (2.4V).

Water Electrolysis in the Presence of a Base (pH higher than 7)

Additional hydroxyl ions release their electrons to the anode, while electrons at the cathode oxidize water molecules near it. Half reactions of electrolysis in the presence of a base are as follows:

At cathode: 2H2O(l) + 2e→ H2(g) + 2OH E° = -0.83 V

At anode: 4OH → O2 + 2H2O + 4eE° = +0.4 V

Net reaction is 2H2O → O2(g) + 2H2 E° = -1.23 V

Like electrolysis in an acid medium, electrolysis in the basic medium also needs a much lower potential.

The pourbaix diagram gives the equilibrium regions of water, hydrogen and oxygen at various electrode potentials.

Electrolysis in the Presence of a Base

Water Electrolysis in the Presence of Salts

Salts are 100% dissociate into cations and anions in water, and hence increase the ionic concentration for increasing conductivity. But the cations and anions from the salt also will be attracted towards the electrodes, and hence become competitors to the decomposition of water to produce hydrogen and oxygen. So, the selection of salts with non-competing ions becomes necessary.

Salts containing lesser standard electrode potentials than hydrogen and hydroxide ions are suitable for the electrolysis of water.

Ions of first and second group elements (Li, Na, K, Mg, Ca, Ba, etc.) have lower standard potential than hydrogen ions and will not be reduced and allow hydrogen ions from water to hydrogen.

Non-reactive anions like nitrate and sulphate ions have a lesser standard reduction potential than hydroxide ions. Sulphate oxidation to peroxy-sulphate has a reduction potential of +2.1V.

Non-soluble, solid polymeric ionic compounds (Nafion) have been found to help the electrolysis of water in less than 1.5V.

Electrolysis of Water Using Electro Catalysts

Electro-catalysts are substances that accelerate electrochemical reactions without being consumed in the reaction, like a catalyst in chemical reactions. Catalysts take the reaction through a different path of lower activation energy. High surface area and larger activation centres are the ability of the catalyst to increase reactivity.

The activity of the inert electrode like platinum can be enhanced by modification of the surface by

i) Increasing the surface area with nanoparticles or alloying with catalytic d-block elements and changing the electronic state coated with other catalytic substances to enhance the electrolysis.

ii) Coating the electrode surface with catalytically active substances, like enzymes.


The electrolytic cell used for the electrolysis of water is the electrolyzer. Depending on the transporter of the electrolyte, electrolyzers can be divided into three types:

Polymer Electrolyte Membrane (PEM) Electrolyzer

A polymer such as Nafion separates the electrodes and allows hydrogen ions formed by the oxidation of water at the anode to pass through it to the cathode compartment for discharge and form hydrogen gas.

Alkaline Electrolyzers

Dilute aqueous sodium (or potassium) hydroxide used in the electrolysis provides and movement of hydroxide ions to the anode to form oxygen.

Solid Oxide Electrolyzer

Ceramic oxide separates the electrodes. At the cathode, water is reduced to hydrogen and oxide ions. The oxide ions pass through the ceramic oxide to the anode to become oxygen gas. This is used at high temperatures of 700 to 800°C to reduce the external voltage needed for electrolysis.

Illustration of a PEM electrolyzer

Electrolysis of Pure Water

An excess amount of energy in the form of overpotential (to overcome various activation barriers) is usually required for the electrolysis of pure water. This excess energy is extremely important because, without it, the process occurs very slowly and sometimes not at all. The limited self-ionization of water is also a reason for this. Moreover, the electrical conductivity of pure water is about one millionth less than that of seawater. In such cases, the efficiency of electrolysis can be increased by using a proper electrolyte such as a salt, an acid or a base along with electrocatalysts.

Electrolysis in Molten State

Test your Knowledge on Water electrolysis


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