Topics
Some Basic Concepts of Chemistry
- Introduction of Some Basic Concepts of Chemistry
- Nature of Chemistry
- Properties of Matter and Their Measurement
- Laws of Chemical Combination
- Dalton's Atomic Theory
- Atomic and Molecular Masses
- Mole Concept
- Moles and Gases
Introduction to Analytical Chemistry
- Introduction of Analytical Chemistry
- Analysis
- Mathematical Operation and Error Analysis
- Determination of Molecular Formula
- Chemical Reactions and Stoichiometric Calculations
- Limiting Reagent
- Concentration of a Solution
- Use of Graph in Analysis
Basic Analytical Techniques
- Introduction of Some Analytical Techniques
- Purification of Solids
- Crystallisation Method
- Fractional Crystallization
- Simple Distillation Method
- Solvent Extraction
- Chromatography Method
- Adsorption Chromatography
- Partition Chromatography
Structure of Atom
- Subatomic Particles
- Atomic Number and Atomic Mass Number
- Isotopes, Isobars and Isotones
- Drawbacks of Rutherford Atomic Model
- Bohr’s Atomic Model
- Bohr’s Model for Hydrogen Atom
- Quantum Mechanical Model of Atom
Chemical Bonding
- Introduction of Chemical Bonding
- Kossel-lewis Approach to Chemical Bonding - Octet Rule
- Kossel and Lewis Approach to Chemical Bonding
- Kossel-lewis Approach to Chemical Bonding - Formal Charge
- Kossel-lewis Approach to Chemical Bonding - Limitations of the Octet Rule
- Valence Shell Electron Pair Repulsion Theory (VSEPR)
- Valence Bond Theory
- Molecular Orbital Theory
- Parameters of Covalent Bond
- Dipole Moment
- Resonance
Redox Reactions
- Introduction of Redox Reactions
- Oxidation Number
- Balancing Redox Reactions in Terms of Loss and Gain of Electrons
- Redox Reaction and Electrode Potential
Modern Periodic Table
- Introduction of Periodic Table
- Structure of the Modern Periodic Table
- Periodic Table and Electronic Configuration
- Blockwise Characteristics of Elements
- Periodic Trends in Elemental Properties
Elements of Group 1 and 2
- Hydrogen
- Alkali Metals and Alkaline Earth Metals
- Some Important Compounds of Elements of S-block
Elements of Group 13, 14 and 15
- Electronic Configuration of Elements of Groups 13, 14 and 15
- Trends in Atomic and Physical Properties of Elements of Groups 13, 14 and 15
- Chemical Properties of the Elements of the Groups 13,14 and 15
- Catenation
- Allotropy and Allotropes of Carbon
- Molecular Structures of Some Important Compounds of the Group 13, 14 and 15 Elements
- Chemistry of Notable Compounds of Elements of Groups 13, 14 and 15
States of Matter
- Introduction of States of Matter: Gaseous and Liquid States
- Intermolecular Forces
- Characteristic Properties of Gases
- The Gas Laws
- Ideal Gas Equation
- Kinetic Molecular Theory of Gases
- Deviation from Ideal Behaviour
- Liquefaction of Gases and Critical Constant
- Liquid State
Adsorption and Colloids
- Introduction of Adsorption
- Adsorption
- Types of Adsorption
- Factors Affecting Adsorption of Gases on Solids
- Adsorption Isotherms (Freundlich and Langmuir Adsorption Isotherm)
- Applications of Adsorption
- Catalysis
- Adsorption Theory of Heterogeneous Catalysis
- Colloids
Chemical Equilibrium
- Introduction of Chemical Equilibrium
- Equilibrium in Physical Processes
- Equilibrium in Chemical Processes - Dynamic Equilibrium
- Law of Mass Action and Equilibrium Constant
- Homogeneous and Heterogenous Equilibria
- Characteristics of Equilibrium Constant
- Applications of Equilibrium Constants
- Le Chaterlier's Principle and Factors Altering the Composition of Equilibrium
- Industrial Application
Nuclear Chemistry and Radioactivity
- Introduction: Nuclear Chemistry is a Branch of Physical Chemistry
- Classification of Nuclides
- Nuclear Stability
- Radioactivity
- Radioactive Decays
- Modes of Decay
- Nuclear Reactions
- Applications of Radio Isotopes
Basic Principles of Organic Chemistry
- Introduction of Basic Principles of Organic Chemistry
- Structural Representation of Organic Molecules
- Classification of Organic Compounds
- Nomenclature of Organic Compounds
- Isomerism
- Theoretical Basis of Organic Reactions
Hydrocarbons
- Alkanes
- Alkenes
- Alkynes
- Aromatic Hydrocarbons
Chemistry in Everyday Life
- Chemistry in Everyday Life
- Basics of Food Chemistry
- Compounds with Medicinal Properties
- Cleansing Agents
- Reactions in solutions
- Mass percentage
- Mole fraction
- Molarity
- Molality
- Volume percentage
Definition
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Unsaturated solution: If the amount of solute contained in a solution is less than the saturation level, it is called an unsaturated solution. (till it is dissolving).
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Saturated solution: When no more solute can be dissolved in a solution at a given temperature, it is called a saturated solution.
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Solubility: The amount of the solute present in the saturated solution at this temperature is called its solubility.
Notes
Concentration of a Solution:
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Take salt and dissolve it in water.
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Keep adding and stir.
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After a time, it won’t be soluble.
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Heat it and try dissolving.
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It will dissolve!
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Try adding more and dissolve it.
From the about activity, the following can be inferred!
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Unsaturated solution: If the amount of solute contained in a solution is less than the saturation level, it is called an unsaturated solution. (till it is dissolving).
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Saturated solution: When no more solute can be dissolved in a solution at a given temperature, it is called a saturated solution.
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Solubility: The amount of the solute present in the saturated solution at this temperature is called its solubility.
How will you decide how concentrated the solution is?
Concentration of solution = `" Amount of solute"/"Amount of solution" "or" "Amount of solute"/"Amount of solvent"`
There are various ways of expressing the concentration of a solution
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`"Mass by mass percentage of a solution" = "Mass of solute"/"Mass of solution" xx 100`
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`"Mass by volume percentage of a solution" = "Mass of solute"/"Volume of solution" xx 100`.
Example
Example
To make a saturated solution, 36 g of sodium chloride is dissolved in 100 g of water at 293 K. Find its concentration at this temperature.
Mass of solute (sodium chloride) = 36 g (Given)
Mass of solvent (water) = 100 g (Given)
Then, the mass of solution = Mass of solute + Mass of solution
= (36 + 100) g
= 136 g
Therefore, concentration (mass by mass percentage) of the solution
= `"Mass of solute"/"Mass of solution"xx100%`
= `36/136xx100%`
= 26.47 % (w/w)
