# Electrolytic Conductance

When a certain volt is applied to the electrodes dipped into an electrolyte solution, ions of electrolyte moves and electric current flows through the electrolytic solution. This is called electrolytic conductance.

**Terms used in electrolytic conduction: **

**Conductance:** It is the property of a conductor which indicates the ease with which the conductor permits the flow of electricity through it. It is denoted by C. Conductance is the reciprocal of resistance.

C = 1/R

**Specific conductance:** The conductance of a conductor having unit length and unit area is called as specific conductivity. It is denoted by ${\kappa}$(Kappa). It is defined as the reciprocal of resistivity.

$$i.e., \kappa = \frac{1}{ \rho}$$

$$or, \kappa = \frac{1}{ \frac{RA}{l}}$$

$$or, \kappa = \frac{1}{R} \times \frac{1}{A}$$

$$or, \kappa = C \times \frac{l}{A}$$

when, l = 1 cm and A = 1 cm^{2}

$$ \text{K = C}$$

So, in case of electrolytic solution, specific conductivity is defined as the conductance of the solution enclosed between two parallel electrodes having unit area separated by a distance of unit length.

**Equivalent conductance: **The conductance of a solution containing one gram equivalent of the electrolyte in the given volume of solution is called equivalent conductance. It is denoted by ${\wedge}$ (wedge).

It is related with specific conductance as:

${\wedge = \kappa \times V}$

Where, V is the volume containing one gram equivalent of electrolyte.

Let us consider an electrolytic solution having normality 1. Then,

N gram equivalent of the electrolytes are present in 1000 cc of solution.

1 gram of electrolyte are present in 1000/N cc of solution.

Unit of equivalent conductance: $\Omega^{-1} cm^{-1} equiva^{-1} $

**Molar conductance: **The conductance of the solution containing one mole of electrolyte in the given volume of solution is called molar conductance. It is denoted by $(\mu)$. It is relatd with specific conductance as:

${\mu = \kappa \times V}$

Where, V is the solution containing one mole of the electrolye.

Let us consider a electrolytic solution having molarity M. Then,

M mole of solution are present in 1000 CC of solution.

1 mole of electrolyte is present in 1000/M cc of solution.

Unit: $\Omega^{-1} cm^{-1} mol^{-1} $

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