Topic Name
10 Haloalkanes and Haloarenes
10.1 Classification
10.2 Nomenclature
10.3 Nature of C–X Bond
10.4 Methods of Preparation of Haloalkanes
10.5 Preparation of Haloarenes
10.6 Physical Properties
10.7 Chemical Reactions
Topic Name
11 Alcohols, Phenols and Ethers
11.1 Classification
11.2 Nomenclature
11.3 Structures of Functional Groups
11.4 Alcohols and Phenols
11.5 Some Commercially Important Alcohols
11.6 Ethers
Topic Name
13 Amines
13.1 Structure of Amines
13.2 Classification
13.3 Nomenclature
13.4 Preparation of Amines
13.5 Physical Properties
13.6 Chemical Reactions
13.7 Method of Preparation of Diazonium Salts
13.8 Physical Properties
13.9 Chemical Reactions
13.10 Importance of Diazonium Salts in Synthesis of Aromatic Compounds
Topic Name
15 Polymers
15.1 Classification of Polymers
15.2 Types of Polymerisation Reactions
15.3 Molecular Mass of Polymers
15.4 Biodegradable Polymers
15.5 Polymers of Commercial Importance
Topic Name
16 Chemistry in Everyday Life
16.1 Drugs and their Classification
16.2 Drug-Target Interaction
16.3 Therapeutic Action of Different Classes of Drugs
16.4 Chemicals in Food
16.5 Cleansing Agents
Class 12th Chemistry Online Class: Excelling in CBSE Board Exams
Strong electrolytes
A solute or substances that completely ionize or dissociates in a solution are known as strong electrolyte. These ions are good conductors of electricity in the solution.
For example, HCl, HBr, HI, HNO3, NaOH, KOH, etc.
For strong electrolytes, Λm increases slowly with dilution and can berepresented by the equation:
Kohlrausch law of independent migration of ions
The Kohlrausch law of independent migration of ions 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.
Weak electrolytes
A substance which forms ions in an aqueous solution do not dissociate completely at moderate concentrations is known as weak electrolyte.
For example, HC2H3O2 (acetic acid), H2CO3 (carbonic acid), etc.
The conductance of the solution increases with dilution of solution.
The interionic forces of attraction are not strong at a low concentration.
The slope for Λm vs c1/2 is not linear even at a lower concentrations.
These electrolytes have lower degree of dissociation at higher concentrations.
The value of Λm changes with dilution due to increase in the degree of dissociation.
Ëmincreases sharply on dilution exclusively at lower concentrations.
At infinite dilutionwhen concentration approaches to zero, the electrolyte dissociates completely. But at lower concentration the conductivity of a solution is low to an extent that cannot be even measured.
