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Conductance Of Electrolytic Solutions
Chapter Name : Electrochemistry
Sub Topic Code : 102_12_03_05_06
Topic Name : Conductance Of Electrolytic Solutions
Sub Topic Name : Kohlrausch's Law And Applications
Introduction

• Kohlrausch gave the law of independent migration of ions. The law states that limiting molar conductivity of an electrolyte can be represented as the sum of the individual contributions of the anion and cation of the electrolyte. • Using Kohlrausch law of independent migration of ions, it is possible to calculate Ëm°, molar conductivity for any electrolyte.

Pre-Requisites:

Electrochemical cell, electrolyte (strong and weak), conductivity, molar conductivity, limiting molar conductivity.

Activity:

Salt solution conducts electricity as it forms a large number of ions in solution in water. Salts are therefore necessary for the human body as well.

Real Life Question:

Why does salt solution conduct electricity but a vinegar solution does not?

Key Words / FlashCards
Key Words Definitions (pref. in our own words)
Electrolyte Electrolyte is a solution which conducts electricity.
Learning aids / Gadgets
Gadgets How it can be used
Salt water, vinegar, bulb with a circuit Dip a circuit bulb in a salt solution and then in normal water. Notice the intensity of the light in the bulb. Now dip the circuit bulb attached to a battery in vinegar and compare it with the intensity of the light bulb with that in salt solution.
Real life uses :

Conductivity of ionic solutions such as important salt, are important for the human body.

Places to visit :

Garage, switchboard

Practical examples around us
Examples Explainations
Salt solution, vinegar A salt solution conducts electricity while vinegar, a diluted form of acetic acid does not as it is a weak electrolyte.
What you learn in Theory:

Using Kohlrausch law of independent migration of ions, it is possible to calculate Ëm° for any electrolyte from the ?o of individual ions.

What you learn in Practice:

For weak electrolytes like acetic acid it is possible to determine the value of its dissociation constant, K, once we know the Ëm° and ?m at a given concentration c.

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