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 ↓


Factors Affecting Solubility


Solubility is an important concept in chemistry, especially when studying solutions. A solution is a mixture in which one substance, known as the solute, is dissolved in another substance, known as the solvent. When you mix things together, some substances dissolve better than others. Let's find out why this is and what factors affect the solubility of substances.

What is solubility?

Solubility is the maximum amount of a substance that can dissolve in a given amount of solvent at a specified temperature. It is usually expressed in grams of solute per 100 grams of solvent.

Solubility = (grams of solute) / (100 grams of solvent)

For example, if you can dissolve 36 grams of sodium chloride in 100 grams of water, then the solubility of sodium chloride in water would be 36 g/100 g.

Factors affecting solubility

Solubility can be affected by a number of factors. Let's look at each of these factors in more detail:

1. Temperature

Temperature is an important factor affecting solubility. In most cases, the solubility of a solid in a liquid solvent increases with an increase in temperature. This is because higher temperatures provide more energy to break the bonds between particles in the solute, making it easier for them to diffuse between solvent particles.

+ heat solute Solvent

For example, sugar dissolves better in hot water than in cold water.

However, the effect of temperature on the solubility of gases is the opposite. The solubility of gases decreases with increasing temperature. This is why hot soda fizzes more than cold soda – gases escape more easily from hot liquids.

2. Pressure

While pressure does not significantly affect the solubility of solids and liquids, it has a major effect on gases. According to Henry's Law, the solubility of a gas in a liquid is directly proportional to the pressure of that gas above the liquid:

C = kP

where C is the solubility of the gas, k is a constant, and P is the pressure of the gas.

This is why carbonated beverages are bottled at high pressure; increasing the pressure increases the solubility of the carbon dioxide gas in the liquid.

3. Nature of solute and solvent

The nature of both the solute and the solvent can significantly affect solubility. Generally, the rule of thumb is "like dissolves like": polar substances will dissolve in polar solvents, and nonpolar substances will dissolve in nonpolar solvents.

Let's consider water and oil. Water is a polar solvent, and oil is nonpolar. Because of their different nature, oil and water do not mix.

Oil Water

Salt, on the other hand, is ionic and dissolves easily in water, as water can stabilize the ions due to its polarity.

4. Particle size

The size of the solute particles can also affect solubility. Smaller particles have more surface area than larger particles, which means that smaller particles will dissolve faster than larger ones.

For example, granulated sugar dissolves faster in water than sugar cubes because granulated sugar has a larger surface area in contact with the solvent.

5. Stir and mix

Agitation or stirring increases the solubility of a substance. When you stir a solution, it causes the solvent to come into contact with the solute more often, speeding up the dissolving process.

However, it is important to note that stirring does not increase solubility, but only speeds up the rate at which the solute dissolves.

Practical example: What affects solubility in everyday life?

Understanding solubility can help us understand everyday phenomena. Here are some examples:

Sugar in tea or coffee: When you add sugar to hot tea or coffee, it dissolves faster than in a cold drink due to the increased temperature.

Soft drinks: Carbonated beverages are made by dissolving carbon dioxide gas in a liquid under high pressure. When you open a soda can, the pressure is released and the gas escapes, causing fizzing.

Salt in cooking: When you cook pasta or rice, salt dissolves better in boiling water because of the increased temperature.

Understanding these factors can help you predict how well substances will dissolve under different conditions, which is important in scientific experiments as well as in everyday tasks.

Conclusion

In short, solubility is affected by many factors such as temperature, pressure, and the nature of the solute and solvent. By controlling these factors, we can influence the ability of a substance to dissolve in a solvent, making it an essential concept for both scientific and practical applications.

Understanding solubility and the factors that affect it can provide information about many different processes in chemistry and help us manipulate conditions to achieve desired results in various applications.


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Factors Affecting Solubility

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