Grade 6
  1. Introduction to Chemistry  1.1. What is Chemistry?  1.2. Importance of chemistry in daily life  1.3. Branches of chemistry  1.4. Safety rules in chemistry laboratory  1.5. Common Laboratory Equipment and Their Uses
  2. Matter and its states  2.1. Definition of Matter  2.2. Properties of matter  2.3. States of matter  2.4. Solid state  2.5. Fluid state  2.6. Gaseous state  2.7. Plasma state  2.8. Changes in the states of matter  2.9. Melting and freezing  2.10. Evaporation and Condensation  2.11. Sublimation  2.12. Deposit
  3. Physical and chemical changes  3.1. Definition of Physical Change  3.2. Examples of physical change  3.3. Definition of Chemical Change  3.4. Examples of chemical change  3.5. Difference Between Physical and Chemical Changes  3.6. Indicators of Chemical Change
  4. Elements, Compounds, and Mixtures  4.1. Definition of the element  4.2. Classification of elements  4.3. Metals  4.4. Non metallic  4.5. Metalloids  4.6. Noble gases  4.7. Definition of compound  4.8. Properties of Compounds  4.9. Definition of Mixture  4.10. Types of mixtures  4.11. Homogeneous mixture  4.12. Heterogeneous mixtures
  5. Separation of mixtures  5.1. The need for isolation  5.2. Separation methods  5.3. Handpicking and winnowing  5.4. Filtration  5.5. Sedimentation and decantation  5.6. Evaporation  5.7. Crystallization  5.8. Distillation  5.9. Magnetic Separation  5.10. Chromatography
  6. Air and its composition  6.1. Components of air  6.2. Importance of Oxygen  6.3. The importance of nitrogen in the air and its composition  6.4. Carbon dioxide in the atmosphere  6.5. The role of water vapor and other gases in air and its composition  6.6. Properties of Air  6.7. Uses of air  6.8. Air pollution and its effects
  7. Water and its properties  7.1. Importance of Water  7.2. Sources of water  7.3. Properties of water  7.4. Water as the universal solvent  7.5. Water Purification  7.6. Water purification methods (boiling, filtration, chlorination)  7.7. Water cycle  7.8. Water conservation  7.9. Water pollution and its effects
  8. Acids, Bases and Salts  8.1. Definition of Acid  8.2. Properties of Acids  8.3. Examples of Acids  8.4. Definition of Bases  8.5. Properties of bases  8.6. Examples of Bases  8.7. Definition of Salt  8.8. Neutralization reaction  8.9. pH Scale and Indicators  8.10. Uses of Acids, Bases and Salts
  9. Introduction to the Periodic Table  9.1. History of the Periodic Table  9.2. Arrangement of elements in the periodic table  9.3. Groups and periods  9.4. Importance of periodic table  9.5. First 10 elements and their symbols
  10. Metals and Nonmetals  10.1. Properties of Metals  10.2. Properties of Non-Metals  10.3. Difference Between Metals and Nonmetals  10.4. Uses of metals and nonmetals  10.5. Corrosion of metals and its prevention
  11. chemical reactions  11.1. Introduction to Chemical Reactions  11.2. Types of Chemical Reactions  11.3. combustion reaction  11.4. Oxidation and Reduction  11.5. Simple chemical equations  11.6. Rusting of iron
  12. Fuel and energy  12.1. Types of fuel  12.2. Fossil fuels  12.3. Renewable and non-renewable sources of energy  12.4. Energy Conservation  12.5. Alternative sources of energy (solar, wind, hydropower)
  13. Plastic and fiber  13.1. Natural and synthetic fibers  13.2. Properties of plastics  13.3. Advantages and disadvantages of plastic  13.4. Recycling of plastic  13.5. Biodegradable and non-biodegradable materials

Grade 6 ↓


Acids, Bases and Salts


Chemistry is all around us. It's in the air we breathe, the food we eat, and even the cleaning supplies we use around the house. An essential part of chemistry involves acids, bases, and salts. In this lesson, we're going to explore these fascinating substances, which play a big role in chemistry and our daily lives.

What are acids?

Acids are chemicals that taste sour. Did you know that the lemon juice you drink in your lemonade is acidic? It contains citric acid. Other common acids include vinegar, which contains acetic acid, and hydrochloric acid which is found in our stomach and helps us digest food.

 Common acids and their chemical formulas:
- Citric acid: C₆H₈O₇
- Acetic acid: CH₃COOH
- Hydrochloric acid: HCl

Properties of acids

  • Acids generally taste sour.
  • They can turn blue litmus paper red.
  • Acids can conduct electricity when dissolved in water.
  • They can react with metals to produce hydrogen gas.
  • Acids can neutralise bases to form water and salt.
Acid

An important use of acids in everyday life is in the production of fertilizers, which help plants grow. For example, sulfuric acid is used to make phosphate fertilizers.

What are the bases?

Bases are chemicals that taste bitter and are slippery to the touch. They are often found in cleaning products because they can help break down grease and dirt. A common household base is sodium bicarbonate, also known as baking soda.

 Common bases and their chemical formulas:
- Sodium bicarbonate: NaHCO₃
- Ammonia: NH₃
- Sodium hydroxide: NaOH

Properties of bases

  • Bases have a bitter taste.
  • They can turn red litmus paper blue.
  • The base feels slippery or soapy to the touch.
  • They can conduct electricity in solution.
  • Bases can neutralise acids to form water and salt.
Bases

Baking soda or sodium bicarbonate is often used in cooking and cleaning. When used in cakes and cookies, it helps them rise by producing carbon dioxide gas when heated.

What are salts?

Salts are formed when acids and bases react with each other and are neutralized. The process of forming salts is called neutralization. Salts are found everywhere, from the table salt used on chips to Epsom salts dissolved in hot water.

 Common salts and their chemical formulas:
- Table salt: NaCl (formed from hydrochloric acid and sodium hydroxide)
- Epsom salt: MgSO₄ (formed from magnesium and sulfuric acid)

Properties of salts

  • Salts are usually solid and crystalline at room temperature.
  • They can dissolve in water and form ions, allowing the solution to conduct electricity.
  • Unlike acids and bases, salts do not change the colour of litmus paper.
Salts

An everyday example of salt is table salt, and its chemical name is sodium chloride (NaCl). It is used to make food taste good and to preserve it by preventing bacteria from growing.

Fail

The reaction between an acid and a base to form salt and water is called neutralization. This reaction is important because it can help balance or neutralize the pH level, which measures how acidic or alkaline a substance is.

 Example of neutralization:
HCl + NaOH → NaCl + H₂O (Hydrochloric acid + Sodium hydroxide → Sodium chloride + Water)

Ph scale

The pH scale measures how acidic or alkaline a solution is. The scale runs from 0 to 14, with 7 being neutral. Substances with a pH less than 7 are acidic, while substances with a pH greater than 7 are alkaline.

0 7 14 Acidic Basic Neutral

For example, lemon juice has a pH of about 2, which is acidic, and household ammonia has a pH of about 11, which is alkaline. Pure water is neutral with a pH of 7.

Practical applications in everyday life

Acids, bases and salts have various uses in our daily life. Here are some examples:

  • Acids: Used in food preservation (vinegar), cleaning products and car batteries (sulfuric acid).
  • Alkali: Used in household cleaners, soap making, and baking (baking soda).
  • Salts: Used as Epsom salts for cooking, water softening, and muscle relaxation.

Conclusion

Understanding acids, bases, and salts is very important in chemistry because they are part of countless reactions. These substances are important not only in laboratories and industries but also in our homes. By learning more about how they work and their properties, we can better understand the chemistry around us in our daily routine.


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Acids, Bases and Salts

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