Electrochemistry is the branch of chemistry which deals with the chemical changes caused in the matter by passage of electric current and conversion of chemical energy into electrical energy and vice versa.

Electrochemistry deals with the study of electrical properties of solutions of electrolytes and with the interrelation of chemical phenomenon and electrical energies. It is the study of production of electricity from energy released during spontaneous​chemical reactions and the use of electrical energy to bring about non-spontaneous chemical reactions. Chemical changes involving electric current are called electrochemical changes. 

Cells and Batteries used by us in various instruments and devices, convert chemical energy into electrical energy. Electrochemical reactions taking place in these cells and batteries are energy efficient and cause less pollution.

These electrochemical cells are an important source of energy in today’s time so it becomes very important for us to study electrochemistry for creating new technologies in this field.
Electrochemistry is related to our biological system also. The transmission of sensory signals in our body from brain to other body parts takes place through neurons. This transmission of signals in our body has electrochemical origin. Therefore, electrochemistry is not only limited up to chemistry but its braches extend to physics and biology also. In this chapter we will explore the concepts of electrochemistry in more details under following subtopics:
  • Electrolysis and Electrolytic Cell

  • Faradays Laws of Electrolysis

  • Arrhenius Theory of Electrolytic Dissociation

  • Molar Conductivity

  • Kohlarusch’s Law

  • Electrochemical Cell

  • EMF of Galvanic Cell

  • Electrode Potential

  • Concentration Cells

  • Solved Examples On Electrochemistry

Conductors and Non Conductors

Substances around us can be divided into two classes based on their ability of conduct electricity:

  • Non-Conductors: Those substances which do not allow electric current to pass through them are called non-conductors or insulators. Example: - wood, plastic glass, rubber etc.

  • Conductors: Those substances which allow electric current to flow through tem are called conductors. Examples: Copper, Iron, Gold, Silver, Graphite, salt solution etc.

Conductors can further be divided into two groups

  • Metallic Conductors: These conductors conduct electricity or electric current by movement of electrons without undergoing any chemical change during the process. These conduct electricity in both solid as well as molten state. Example: All the metals and Graphite

  • Electrolytes: Those substances which conduct electricity only when they are present in aqueous solution and not in solid form are called electrolytes. These conduct electricity by movement of ions in solutions.   

For a substance to conduct electricity; it must either have free electrons or ions which carry electricity with them. Electrolytes neither have free electrons nor free ion in solid state although they are ionic compound. This is because the oppositely charged ions are held together by strong electrostatic attraction and are not free to move. But when they are dissolved in water, the two ions split up and become free to move in solution and now they are free to conduct electricity. Examples of electrolytes are: NaCl, KCl, Na2SOetc

Non-ionic compound or covalent compounds do not conduct electricity in aqueous solution and hence they are called non-electrolytes. Examples of non- electrolytes are: Urea, Glucose, Sugar etc.

Electrolytes can further be divided into strong and weak electrolytes:

  • Strong Electrolytes are those electrolytes which dissociate completely in aqueous solution to give constituent ions. For example: Inorganic salts like NaCl, KCl, Strong Acid like HCl, H2SO4, Strong bases like NaOH, KOH etc.

  • Weak Electrolytes are those electrolytes which partially dissociate in aqueous solution to give constituent ions. For example:  weak acid like CH3COOH and Weak bases like NH3.

Comparision of Electrolytic and Metallic Conduction

S.No Metallic Conduction Electrolytic Conduction

Electric current flows by movement of electrons.

Electric current flows by movement of ions.


No chemical change occurs.

Ions are oxidized or reduced at the electrodes.


It does not involve the transfer of any matter.

It involves transfer of matter in the form of ions.


Ohm's law is followed.

Ohm's low is followed.


Resistance increases with increase of temperature.

Resistance decreases with increase of temperature.


Faraday law is not followed.

6Faraday law is followed.


  • Pure water does not conduct electricity. Conductivity of tap water is due to dissolved salts and minerals.
  • Conductivity of metallic conductors increases while that of electrolytes decreases with increase in temperature.
  • Common salt which we use daily in our food is a strong electrolyte.
  • Electrolytes are very important in our biological system. Our body requires electrolytes for functioning of nervous system and other life processes. 

Semiconductors: Semiconductors are those substances whose conductivity is intermediate to those of conductors and insulators i.e.  Conductivity is more than insulator and less then conductors.


Question 1: Substances which do not conduct electricity in solid state but in question solution is known as..

a. insulators

b. conductors

c. electrolytes

d. strong acids

Question 2: Which of the following substances is not an electrolyte?

a. Common salt

b. Sulphuric Acid

c. Acetic Acid

d. Glucose

Question 3: Which of the following substances is not a non-electrolyte?

a. Gold

b. Mercury

c. Graphite

d.Ammonium  Chloride

Question 4: Which of the following compounds will not conduct electricity in its aqueous solution?

a. Carbontetrachloride

b. Silver chloride

c. Sodium acetate

d. Sulphuric Acid

Question 5: Which of the following electrolytes is not strong one?

a. HCl

b. NaCl

c. H2SO4


Q.1 Q.2 Q.3 Q.4 Q.5
c d d a d


Related Resources:- 

Related Resources
Concentration Cells

1 | 2 | Concentration Cells If two plates of the...

Relation-Equilibrium Constant Gibbs free Energy and EMF of Cell

Relation between Equilibrium constant, Gibbs free...

Molar Conductivity

Conductance, Specific conductance and Molar...

Equilibrium Constant-Gibbs free Energy-EMF of Cell

Relation between Equilibrium constant, Gibbs free...

Fuel Cell

FUEL CELL Fuel cells are another means by which...

Commercial Production of Chemicals

Commercial Production of Chemicals The wide...

Arrhenius Theory of Electrolytic Dissociation

Arrhenius Theory of Electrolytic dissociation...

Difference in Electrolytic Cell and Galvanic Cell

Electrochemistry Difference in Electrolytic Cell...

Electrochemical Cell

Electrochemical Cell ELECTROCHEMICAL CELL...

Nernst Equation

1 | 2 | Nernst Equation ELECTRODE AND CELL...

Electrode Potential

Electrode Potential ELECTRODE POTENTIAL When a...

Reversible and Irreversible Cells

Reversible and Irreversible cells REVERSIBLE AND...

Calomel Electrode


Electrochemical Series

Electrochemical Series By measuring the potentials...

Representation of an Electrochemical Cell

Representation of an Electrochemical Cell...

Faradays Laws of Electrolysis

Faraday’s Laws of Electrolysis The...

Daniell Cell

1 | 2 | Daniell Cell DANIELL CELL It is designed...

EMF of Galvanic Cell

EMF of A Galvanic Cell EMF OF A GALVANIC CELL...

Theory of Weak Electrolytes

1 | 2 | 3 | Theory of weak Electrolytes (i) Weak...

Solved Examples

1 | 2 | 3 | Solved Examples on Faraday’s...

Problems on Nernst Equation

Problems on Nernst Equation Example 31: Construct...

Electrolytic and Non-electrolytic Conductors

1 | 2 | Electrolytic and Non-electrolytic...

Prediction for Occurrence of Redox Reaction

Prediction For Occurrence of a Redox Reaction...

Secondary Voltaic Cell


Applications of Electrolysis

1 | 2 | Applications of Electrolysis The...

Solved Examples On Electrochemistry

Download IIT JEE Solved Examples On...

Primary Voltaic Cell


Electrolysis and Electrolytic Cell

Electrolysis and Electrochemical Cells...


1 | 2 | Kohlrausch law KOHLRAUSCH'S LAW "At...

Salt Bridge and its Significance

Salt Bridge and Its Significance SALT BRIDGE AND...