Grade 10
  1. Matter and its properties  1.1. States of matter  1.2. Physical and chemical properties of matter  1.3. Classification of substances (elements, compounds, mixtures)  1.4. Changes in Matter (Physical and Chemical Changes)  1.5. Law of conservation of mass and law of definite proportions
  2. Atomic Structure  2.1. Historical development of the atomic model  2.2. Subatomic particles (protons, neutrons, electrons)  2.3. Atomic number, mass number and isotopes  2.4. Electronic Configuration and Energy Levels  2.5. Valency, ion formation and oxidation state
  3. Periodic table  3.1. History and Development of the Periodic Table  3.2. Modern Periodic Law and Periodic Trends  3.3. Groups and Periods in the Periodic Table  3.4. Trends in the Periodic Table  3.5. Metals, non-metals, metalloids and their properties  3.6. Noble gases and their chemical inertness
  4. Chemical bond  4.1. Formation of Chemical Bonds (Octet Rule)  4.2. Ionic Bonding and Properties of Ionic Compounds  4.3. Covalent Bond and Properties of Covalent Compounds  4.4. Metallic bond and its properties  4.5. Molecular geometry and VSEPR theory  4.6. Polarity and dipole moment of molecules  4.7. Intermolecular forces
  5. Chemical Reactions and Equations  5.1. Types of Chemical Reactions  5.2. Writing and balancing chemical equations  5.3. Law of conservation of mass in chemical reactions  5.4. Factors Affecting Chemical Reactions  5.5. Catalysts and their role in chemical reactions  5.6. Exothermic and Endothermic Reactions
  6. Stoichiometry and Chemical Calculations  6.1. Mole concept and Avogadro number  6.2. Molar Mass and Gram-Mole Conversions  6.3. Empirical and molecular formula  6.4. Stoichiometric calculations and chemical yield  6.5. Limiting and Excess Reactants
  7. Acids, Bases and Salts  7.1. Properties and Definitions of Acids and Bases (Arrhenius, Bronsted-Lowry, Lewis)  7.2. pH Scale, pOH, and Indicators  7.3. Neutralization reactions and salt formation  7.4. Strength of Acids and Bases (Strong vs. Weak Acids and Bases)  7.5. Common Acids and Bases in Daily Life  7.6. Salts, their solubility and applications
  8. Metals and Nonmetals  8.1. Physical and chemical properties of metals  8.2. Physical and Chemical Properties of Non-Metals  8.3. Reactivity Series of Metals and Displacement Reactions  8.4. Extraction of metals from ores  8.5. Corrosion, its causes and prevention  8.6. Alloys, their composition and uses
  9. Carbon and its compounds  9.1. Allotropes of Carbon  9.2. Hydrocarbons and their classification (alkanes, alkenes, alkynes)  9.3. Functional groups in organic compounds  9.4. Nomenclature of organic compounds (IUPAC system)  9.5. Isomerism in organic chemistry (structural and geometrical)  9.6. Important organic reactions (combustion, addition, substitution, polymerization)  9.7. Applications of organic compounds in industry and daily life
  10. Environmental Chemistry  10.1. Air Pollution (Sources, Effects and Control)  10.2. Water Pollution (Causes, Effects and Remedies)  10.3. Greenhouse effect and global warming  10.4. Ozone layer depletion and its effects  10.5. Green Chemistry and Its Applications  10.6. sustainable chemistry practice
  11. Thermochemistry  11.1. Heat and Energy Changes in Chemical Reactions  11.2. Exothermic and Endothermic Reactions  11.3. Enthalpy, enthalpy change, and heat of reaction  11.4. Specific heat capacity and calorimetry  11.5. Energy Changes in Combustion Reactions
  12. Electrochemistry  12.1. Electrolytes and non-electrolytes  12.2. Electrolysis and its applications (electroplating, extraction of metals)  12.3. Redox reactions (oxidation and reduction)  12.4. Galvanic cell and electrochemical series  12.5. Corrosion and electrochemical prevention methods
  13. Chemical kinetics and equilibrium  13.1. Rate of chemical reactions and its measurement  13.2. Factors affecting the reaction rate (catalyst, temperature, concentration)  13.3. Reversible and irreversible reactions  13.4. Dynamic equilibrium and equilibrium constant  13.5. Le Chatelier's principle and its applications
  14. Gases and Gas Laws  14.1. Properties of gases and kinetic molecular theory  14.2. Boyle's Law (Pressure-Volume Relation)  14.3. Charles's Law  14.4. Gay-Lussac's Law  14.5. Combined Gas Law and Ideal Gas Law  14.6. Real Gases vs Ideal Gases
  15. Nuclear Chemistry  15.1. Introduction to Radioactivity and Nuclear Reactions  15.2. Types of radioactive decay (alpha, beta, gamma)  15.3. Half-life and applications of radioactive isotopes  15.4. Nuclear fission and fusion reactions  15.5. Nuclear power generation and its environmental impact

Grade 10 → Acids, Bases and Salts ↓


Salts, their solubility and applications


Salts play an important role in chemistry and have many applications in everyday life. In this lesson, we will learn what salts are, their solubility and various applications. We will use simple language and examples to help you understand this important topic of chemistry.

What are salts?

In chemistry, a salt is a compound that forms when an acid reacts with a base. This reaction is known as a neutralization reaction. Salts are made up of positive ions (cations) from the base and negative ions (anions) from the acid.

For example, when hydrochloric acid (HCl) reacts with sodium hydroxide (NaOH), the reaction produces sodium chloride (common salt) and water:

HCl + NaOH → NaCl + H2O

Sodium chloride (NaCl) is a classic example of a salt. The sodium ion (Na+) comes from sodium hydroxide, and the chloride ion (Cl -) comes from hydrochloric acid.

Salts can vary widely depending on the acid and base used in the reaction. Below are some more examples:

  • Potassium bromide (KBr) from hydrobromic acid and potassium hydroxide.
  • Calcium sulfate (CaSO 4) from sulfuric acid and calcium hydroxide.

Solubility of salts

Solubility is an important property of salts. It refers to the ability of salts to dissolve in a solvent, usually water. The solubility of salts depends on various factors, including temperature and the nature of the solvent.

Generally salts may be classified as follows:

  • Soluble salts: These salts dissolve easily in water. Examples include sodium chloride (NaCl) and potassium nitrate (KNO3).
  • Sparingly soluble salts: These salts have limited solubility in water. An example of this is calcium sulfate (CaSO 4).
  • Insoluble salts: These salts do not dissolve well in water. Examples include barium sulfate (BaSO4) and lead (II) chloride (PbCl2).

Factors affecting solubility

There are several factors that can affect the solubility of a salt:

  • Temperature: The solubility of most salts increases as temperature increases. This means that salts are generally more soluble in hot water than in cold water.
  • Nature of the solvent: Some salts dissolve better in particular solvents. Salts that are very soluble in water may be less soluble in organic solvents such as alcohols.

Visual example of solubility

Water Salt

Applications of salts

Salt has many applications in many sectors such as medicine, agriculture and industry. Here are some common applications:

1. Cooking and food preservation

Sodium chloride, commonly known as table salt, is widely used in cooking to enhance the taste of food. It is also used as a preservative in making pickles and cooking food as it prevents the growth of bacteria.

2. Medicine

Salts play an important role in medical treatment. For example, magnesium sulfate (MgSO 4), also known as Epsom salt, is used to relieve muscle pain and constipation.

In addition, saline solution (sterile salt water) is used in intravenous drip to replace fluids in patients' bodies.

3. Agriculture

Various salts are used as fertilizers in agriculture. For example, potassium chloride (KCl) provides plants with potassium, which is important for plant growth and development.

4. Industrial applications

Salts play an important role in a variety of industrial processes. Some common applications include:

  • Production of chemicals: Salt is an important ingredient in the manufacture of chlorine and caustic soda.
  • Water softening: Certain salts like sodium carbonate (Na2 CO3) are used to soften hard water by replacing calcium and magnesium ions with sodium ions.

Visual example of industrial application

Industry Salt

5. Removing snow from roads

In cold regions, salts such as calcium chloride (CaCl 2) or sodium chloride (NaCl) are spread on roads to melt ice and snow, ensuring safe travel by lowering the freezing point of water.

Precipitation reactions involving salts

Precipitation reactions occur when two solutions containing soluble salts are mixed, forming an insoluble salt called a precipitate. An example of this kind of reaction is when solutions of silver nitrate (AgNO3) and sodium chloride (NaCl) are mixed together, resulting in the precipitation of silver chloride (AgCl):

AgNO 3 + NaCl → AgCl (precipitate) + NaNO 3

Such reactions are useful for the synthesis of new compounds and for qualitative analysis in laboratories to identify the presence of ions.

Visual example of a precipitation reaction

AgNO3 solution sodium chloride AgCl

Conclusion

Salts are an important class of chemical compounds formed by reactions between acids and bases. Understanding the properties of salts, particularly their solubility and reactivity, is essential in both theoretical and applied chemistry. Their wide range of applications in everyday life, from culinary uses to industrial processes, makes them a widely studied subject.


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