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CBSE Class 12 Chemistry

Class 12 · CBSEChemistry50 notes in 11 folders, 352 KB

Notes for CBSE Class 12 Chemistry (043), in a folder for each of the syllabus's ten units in its order, with one note for each chapter or group of related topics and the practicals gathered in a final folder. They follow the 2026-27 syllabus, so topics it removed or assesses only formatively are not included. Delete any folder your course leaves out once the notes are yours.

Adding them puts a copy in your notes, in a folder of its own with the folders below, for you to change and turn into flashcards or a question deck. Download gives you a zip of markdown files, which opens in any notes app.

What is inside

  • Solutions
    • Types of solutions and concentration6 KB
    • Solubility and Henry's law6 KB
    • Vapour pressure, Raoult's law and non-ideal solutions7 KB
    • Colligative properties, molar mass and the van't Hoff factor12 KB
  • Electrochemistry
    • Galvanic cells and electrode potentials8 KB
    • The Nernst equation, Gibbs energy and concentration cells6 KB
    • Conductance of electrolytic solutions and Kohlrausch's law8 KB
    • Electrolysis and Faraday's laws7 KB
    • Batteries, fuel cells and corrosion8 KB
  • Chemical kinetics
    • Rate of reaction and the factors affecting it6 KB
    • Rate law, order and molecularity7 KB
    • Integrated rate equations and half-life6 KB
    • Temperature dependence, Arrhenius equation and collision theory7 KB
  • d- and f-block elements
    • Position, electronic configuration and trends of the d-block7 KB
    • Oxidation states, colour, magnetism, catalysis, interstitial compounds and alloys8 KB
    • Potassium dichromate and potassium permanganate6 KB
    • Lanthanoids and actinoids7 KB
  • Coordination compounds
    • Werner's theory and the terms used7 KB
    • Nomenclature of coordination compounds5 KB
    • Isomerism in coordination compounds5 KB
    • Bonding in coordination compounds9 KB
    • Importance and applications of coordination compounds4 KB
  • Haloalkanes and haloarenes
    • Classification, nomenclature and the carbon-halogen bond6 KB
    • Preparation and physical properties of haloalkanes and haloarenes7 KB
    • Nucleophilic substitution, stereochemistry and other reactions of haloalkanes9 KB
    • Haloarenes and polyhalogen compounds8 KB
  • Alcohols, phenols and ethers
    • Classification, nomenclature, structure and preparation of alcohols8 KB
    • Properties and reactions of alcohols9 KB
    • Preparation, properties and reactions of phenols7 KB
    • Preparation, properties and reactions of ethers6 KB
  • Aldehydes, ketones and carboxylic acids
    • Nomenclature, structure and preparation of aldehydes and ketones6 KB
    • Physical properties and nucleophilic addition of aldehydes and ketones6 KB
    • Oxidation, reduction, alpha-hydrogen reactions and tests for aldehydes and ketones7 KB
    • Nomenclature, structure and preparation of carboxylic acids5 KB
    • Properties, reactions and uses of carboxylic acids8 KB
  • Amines
    • Structure, classification, nomenclature and preparation of amines6 KB
    • Physical properties and basicity of amines6 KB
    • Chemical reactions and identification of amines8 KB
    • Diazonium salts6 KB
  • Biomolecules
    • Classification of carbohydrates, glucose and fructose8 KB
    • Disaccharides, polysaccharides and the role of carbohydrates6 KB
    • Amino acids and proteins7 KB
    • Enzymes, vitamins, nucleic acids and hormones8 KB
  • Practicals
    • Preparing sols, dialysis and emulsions7 KB
    • Experiments on reaction rate, enthalpy change and cell potential9 KB
    • Paper chromatography5 KB
    • Preparing inorganic and organic compounds7 KB
    • Finding the molarity of potassium permanganate by titration6 KB
    • Tests for functional groups, carbohydrates, fats and proteins8 KB
    • Qualitative analysis of salts10 KB

The first note

Solutions / Types of solutions and concentration

## Solutions and their types A **solution** is a homogeneous mixture of two or more substances, meaning that its composition and properties are the same throughout. The component present in the largest amount is the **solvent** and determines the physical state of the solution; the others are **solutes**. A solution of two components is a binary solution. Any of the three states of matter can act as solvent or solute, so there are nine combinations. The ones a student meets most often are these. | Solute | Solvent | Example | |---|---|---| | gas | gas | air (oxygen in nitrogen) | | gas | liquid | oxygen dissolved in water, carbon dioxide in a soft drink | | gas | solid | hydrogen absorbed in palladium | | liquid | liquid | ethanol in water | | liquid | solid | mercury in sodium (an amalgam) | | solid | liquid | sugar or salt in water | | solid | solid | brass (zinc in copper), a substitutional alloy | The notes that follow deal mostly with liquid solutions, in which the solvent is a liquid, because that is where concentration, vapour pressure and colligative properties are measured. ## Expressing concentration The **concentration** of a solution is the amount of solute present in a given amount of solution or solvent. It can be stated in several ways, and the choice depends on whether temperature will change. ### Mass percentage $$ \text{mass \%} = \frac{\text{mass of solute}}{\text{total mass of solution}} \times 100 $$ A solution that is 10% glucose by mass holds 10 g of…

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