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 ↓


Examples of Bases


Bases are an essential part of chemistry and play a key role in various chemical reactions and processes. Let's take a deeper look at what bases are, explore their properties and look at some common examples. This explanation will help you understand bases in a simple and easy to understand way, with visual and text examples.

What are the bases?

Bases are substances that can accept hydrogen ions (H + ) or, more commonly, donate a pair of valence electrons to form a bond. In simple terms, bases are the opposite of acids. While acids are sour and can donate hydrogen ions, bases are bitter and slippery and can accept those ions.

Chemical properties of bases

Bases have specific chemical properties that distinguish them from other substances. Here are some of the main properties:

  • Bases have a bitter taste.
  • They feel slippery or soapy to the touch.
  • Bases change the colour of indicators. For example, they turn red litmus paper blue.
  • Bases can conduct electricity in aqueous solution.
  • They react with acids to form salt and water in neutralization reactions.

Examples of common bases

Let's take a look at some common bases that you may encounter in everyday life and in the laboratory:

Sodium hydroxide (NaOH)

Sodium hydroxide is one of the most commonly used alkalis. It is also known as lye or caustic soda. Sodium hydroxide is used in a variety of industries and households:

  • It is used in making soap.
  • It is used in making paper and clothes.
  • In homes, sodium hydroxide is often found in drain cleaners.
NaOH
NaOH

Calcium hydroxide (Ca(OH) 2 )

Calcium hydroxide is commonly known as slaked lime or lime water.

  • It is used in the construction industry to make mortar and plaster.
  • It is used in agriculture to treat acidic soils.
  • Calcium hydroxide is used in the food industry to process water for soft drinks and alcoholic beverages.
Ca(OH)₂
Ca(OH)₂

Ammonium hydroxide (NH4OH)

Ammonium hydroxide is a solution of ammonia in water. It is often used for cleaning and has many other applications:

  • It is used as a cleaning agent in homes.
  • It is used in the manufacture of fertilizers.
  • It is used as a leavening agent in the food industry.
NH₄OH
NH₄OH

Magnesium hydroxide (Mg(OH) 2 )

Magnesium hydroxide is commonly known as milk of magnesia.

  • It is used as an antacid to relieve heartburn and indigestion.
  • It is also used as a laxative.
Mg(OH)₂
Mg(OH)₂

Visual illustration of the reaction of bases and acids

Bases react with acids to form salt and water, which is called neutralization. Here is a simplified visualization to understand this reaction:

Example reaction: sodium hydroxide and hydrochloric acid

NaOH + HCl → NaCl + H₂O
NaOH , HCl sodium chloride , H₂O

This equation shows how the base NaOH (sodium hydroxide) reacts with the acid HCl (hydrochloric acid) to form the salt NaCl (sodium chloride) and water H₂O.

Interaction of bases and acids with indicators

Bases interact with indicators to produce a change in colour, which helps us to identify them in the laboratory:

  • Litmus Paper: Red litmus paper turns blue in alkaline solution.
  • Phenolphthalein: Phenolphthalein turns pink in alkaline solution.
  • Methyl orange: Turns yellow in alkaline solution.
Red litmus (in acid) Blue litmus (in base)

These color changes are important for experiments and help chemists identify the nature of unknown substances.

Natural alkalis found in daily life

Bases aren't just confined to the laboratory; they're also found in nature and in everyday materials:

  • Baking soda (sodium bicarbonate): A common base used in baking and cleaning.
  • Ammonia: Used in many household cleaning products.
  • Toothpaste: It contains a mild base for cleaning teeth.
NaHCO₃

Sodium bicarbonate (NaHCO₃), commonly known as baking soda, is a mild alkali that reacts with acids to produce carbon dioxide gas, which is useful in making baked goods rise during baking.

NaHCO₃

Conclusion

Bases are a fascinating group of chemical compounds used in a variety of applications, from household cleaning to important industrial processes. By understanding their properties, reactions, and everyday examples, you can better understand the role of chemistry in the natural and industrial world.


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Properties of bases
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Examples of Bases

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