Grade 7
  1. Introduction to Chemistry  1.1. What is Chemistry?  1.2. Importance of chemistry in daily life  1.3. Branches of chemistry  1.4. Scientific Method in Chemistry  1.5. Laboratory Safety Rules and Precautions  1.6. Common Laboratory Equipment and Their Uses  1.7. Units of measurement in chemistry
  2. Matter and its properties  2.1. Definition of Matter  2.2. Classification of matter  2.3. Properties of matter  2.3.1. Physical properties  2.3.2. Chemical properties  2.4. States of matter  2.4.1. Solid state  2.4.2. Fluid state  2.4.3. Gaseous state  2.4.4. Plasma and Bose–Einstein condensates  2.5. Changes in the states of matter  2.5.1. Melting and freezing  2.5.2. Evaporation and Condensation  2.5.3. Sublimation and deposition  2.6. Density and its applications  2.7. Diffusion and its importance
  3. Elements, Compounds, and Mixtures  3.1. Definition of the element  3.2. Classification of elements  3.3. Metals, Nonmetals and Metalloids  3.4. Noble gases and their properties  3.5. Introduction to the Periodic Table  3.6. Definition of Compound  3.7. Properties of Compounds  3.8. Introduction to Chemical Formulas  3.9. Definition of Mixture  3.10. Types of mixtures  3.10.1. Homogeneous mixture  3.10.2. Heterogeneous mixtures  3.11. Difference Between Compounds and Mixtures  3.12. Solutions, Colloids and Suspensions
  4. Separation of mixtures  4.1. Need for separation of mixtures  4.2. Separation methods  4.2.1. Filtration  4.2.2. Sedimentation and decantation  4.2.3. Evaporation  4.2.4. Crystallization  4.2.5. Distillation  4.2.6. Chromatography  4.2.7. Magnetic Separation  4.2.8. Centrifugation
  5. Atomic Structure  5.1. Introduction to Atoms  5.2. Structure of the atom  5.2.1. Nucleus and electron cloud  5.3. Subatomic particles  5.3.1. Proton  5.3.2. Neutron  5.3.3. Electrons  5.4. Atomic number and mass number  5.5. Isotopes and their uses  5.6. Ions and ion formation
  6. Periodic table  6.1. Introduction to the Periodic Table  6.2. Groups and periods  6.3. Trends in the Periodic Table  6.3.1. Atomic Size  6.3.2. Metallic and non-metallic character  6.3.3. Electronegativity  6.3.4. Reactivity of the elements  6.4. Alkali metals and their properties
  7. Chemical bond  7.1. Why do atoms form bonds?  7.2. Types of chemical bonds  7.2.1. Ionic bond  7.2.2. Covalent bond  7.2.3. Metal Bond  7.3. Properties of Ionic and Covalent Compounds  7.4. Intermolecular forces
  8. Chemical reactions  8.1. Introduction to Chemical Reactions  8.2. Signs of a chemical reaction  8.3. Types of Chemical Reactions  8.3.1. Combination Reactions  8.3.2. Decomposition reactions  8.3.3. Displacement reactions  8.3.4. Double displacement reactions  8.3.5. Combustion reactions  8.4. Law of conservation of mass  8.5. Balancing simple chemical equations
  9. Acids, Bases and Salts  9.1. Definition of Acid and Base  9.2. Properties of Acids  9.3. Properties of bases  9.4. pH Scale and Indicators  9.5. Neutralization reactions  9.6. Common Acids and Bases in Everyday Life  9.7. Preparation and use of salts  9.8. Strong and weak acids and bases
  10. Solutions and Solubility  10.1. Definition of Solution  10.2. Components of the solution  10.2.1. Solvent  10.2.2. solute  10.3. Factors Affecting Solubility  10.4. Concentration of solutions  10.5. Saturated and unsaturated solutions  10.6. Colloids and suspensions  10.7. Solubility curve and its interpretation
  11. Air and atmosphere  11.1. Composition of air  11.2. Properties of gases in the air  11.3. Importance of Oxygen and Carbon Dioxide  11.4. Air pollution and its effects  11.5. Greenhouse effect and global warming  11.6. Ways to reduce air pollution  11.7. Ozone layer and its importance
  12. Water and its importance  12.1. Properties of Water  12.2. Water as the universal solvent  12.3. Importance of water for life  12.4. Water pollution and its effects  12.5. Water Purification  12.5.1. Filtration  12.5.2. boil  12.5.3. Chlorination in water purification  12.5.4. reverse osmosis  12.6. Hard and soft water  12.7. Water cycle and its importance
  13. Fuel and energy  13.1. Types of fuel  13.1.1. Fossil fuels  13.1.2. Renewable energy sources  13.2. Combustion and energy release  13.3. Global warming and its effects  13.4. Alternative sources of energy  13.5. Ways to conserve energy
  14. Metals and Nonmetals  14.1. Physical and chemical properties of metals  14.2. Physical and Chemical Properties of Non-Metals  14.3. Difference Between Metals and Nonmetals  14.4. Uses of metals and nonmetals  14.5. Corrosion of metals and its prevention  14.6. Alloys and their importance
  15. Plastics and polymers  15.1. Natural and synthetic polymers  15.2. Properties of plastics  15.3. Biodegradable and Non-Biodegradable Plastics  15.4. Environmental impact of plastic  15.5. Recycling and waste management in plastics and polymers  15.6. Daily Uses of Polymers
  16. Introduction to Organic Chemistry  16.1. Basic definitions of organic chemistry  16.2. Carbon Compounds in Daily Life  16.3. Hydrocarbons  16.4. Simple functional groups (alcohols and carboxylic acids)  16.5. Importance of organic compounds in industry

Grade 7 → Solutions and Solubility ↓


Definition of Solution


The concepts of solution and solubility are fundamental parts of chemistry and help us understand how substances interact in different environments. In chemistry, a solution is a homogeneous mixture made up of two or more substances. In a solution, the substance present in the largest amount is known as the solvent, and the substances present in smaller amounts are known as solutes.

Understanding the solution

At its core, a solution is a mixture where the solute is evenly dispersed within the solvent. The solute particles are broken up into smaller pieces and seamlessly integrated with the particles within the solvent. This integration means that solutions are homogeneous on a molecular level, meaning that their properties are the same no matter where you sample within the mixture.

Components of the solution

  • Solvent: The component of a solution that is present in the greatest quantity and serves as the medium in which the solute dissolves. For example, in a salt water solution, water is the solvent.
  • Solute: The substance that is dissolved in the solvent. Continuing the salt water example, the salt is the solute.

Types of solutions

Solutions can be classified in different ways depending on the state of matter of the solvent and the solute:

1. Solid solution

These solutions are formed when two or more solid substances mix together. An example of a solid solution is steel, which is made by dissolving carbon in iron.

Fe + C = steel

2. Liquid solution

These are probably the most well-known type of solutions. When a solid substance, such as salt, dissolves in a liquid, such as water, the resulting mixture is a liquid solution.

Visual example:

solute Solvent

3. Gaseous solutions

Mixing gases can also form solutions, in which gases dissolve in one another. Earth's atmosphere is a classic example of this, where nitrogen acts as a solvent and oxygen and other gases act as solutes.

Example of chemical representation:

N₂ (solvent) + O₂ (solute) + other gases = atmosphere

Properties of solution

Solutions exhibit several special properties that distinguish them from other types of mixtures:

  • Homogeneity: The solution is homogeneous throughout, that is, a sample taken from any part of the solution will have the same composition.
  • Particle size: Solute particles in a solution are at the molecular or ionic level, typically less than 1 nanometer in diameter.

Solubility

The concept of solubility deals with the extent to which a solute can dissolve in a solvent at a given temperature and pressure. Solubility is an important property that can affect how solutions behave:

  1. Temperature dependence: For many solutes, solubility increases with temperature. For example, sugar dissolves more easily in hot water than in cold water.
  2. Pressure dependence: Solubility applies especially to gases; for example, carbon dioxide is more soluble in cold water at high pressure, which is why soda drinks contain carbonated substances.

Visual representation:

Cold water Hot water Sugar Solubility

The importance of the solution

Solutions play an important role in various natural processes, industrial applications, and daily life activities. Chemical reactions, biological functions, and manufacturing processes often occur in the form of solutions. For example:

  • Plants absorb nutrients dissolved in water.
  • Blood is a fluid that carries nutrients and oxygen to the body's tissues.

In summary, the study of solutions and solubility is essential for a better understanding of chemical interactions and is important in many scientific and practical applications.


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Definition of Solution

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