JSS 2: ACIDS, BASES AND SALTS

-
                                 ACIDS
An acid is a substance that produces hydrogen ions (H⁺) when dissolved in water.
                        Types of acids
The two types of acids are:
I. Organic acids
II. Inorganic acids
Organic acids occur naturally in plants and animals.
Inorganic acids are called mineral acids, since they are produced from mineral ores. They are man- made.
Examples of inorganic acids are:
1. Hydrochloric acid (HCl)
2. Trioxonitrate(V) acid (HNO₃)
3. Sulphuric acid (H₂SO₄) etc
                  Properties of Acids
1.  Acids have sour taste.
2.  Acids turn blue litmus paper red.
3. Acids react with metals to produce hydrogen gas.
4. They conduct electricity in solution.
5. They have pH values less than 7.
                   Uses of Acids
1. Acids are used for food preservation (e.g. acetic acid).
2. Manufacture of fertilisers.
3. Production of medicines.
4. Cleaning metals.
5. In the production of salts
       
                              BASES
A base is an oxide or hydroxide of a metal. Some bases are soluble in water while some are not soluble in water.
 Alkalis are bases that are soluble in water to produce hydroxide ions (OH⁻).
Examples of alkalis include:
1. Sodium hydroxide (NaOH)
2. Potassium hydroxide (KOH)
3. Calcium hydroxide, Ca(OH)₂ 
4. Magnesium hydroxide, Mg(OH)₂
5. Ammonium hydroxide (NH₄OH)
Examples of bases that are not soluble in water:
1. Sodium oxide (Na₂O)
2. 
          Properties of Bases
1. Bases have  bitter taste e.g. Lime water
2. They are slippery or soapy feel.
3. They turn red litmus paper blue.
4. They conduct electricity in solution.
5. They have pH values greater than 7.

              Uses of Bases
1. Use in making soap and detergents.
2. Used in neutralising acids.
3. For treating acidic soil.
4. For manufacturing paper and textiles.



### 5\. SALTS

### Definition

A salt is a compound formed when an acid reacts with a base.

### Neutralisation Reaction

\\text{Acid}+\\text{Base}\\rightarrow\\text{Salt}+\\text{Water}

### Example

\\text{HCl}+\\text{NaOH}\\rightarrow\\text{NaCl}+\\text{H}_2\\text{O}

Hydrochloric acid + Sodium hydroxide → Sodium chloride + Water

### Common Salts

| Salt | Formula | Use |
| ------------------- | --------- | ---------------- |
| Sodium chloride | NaCl | Table salt |
| Calcium carbonate | CaCO₃ | Cement and chalk |
| Copper(II) sulphate | CuSO₄ | Fungicide |
| Ammonium sulphate | (NH₄)₂SO₄ | Fertiliser |
| Potassium nitrate | KNO₃ | Fertiliser |

### Properties of Salts

* Usually crystalline solids.

* Many dissolve in water.

* Conduct electricity when molten or in solution.

 Uses of Salts

* Cooking and food preservation.

* Agriculture (fertilisers).

* Construction (cement).

* Medicine.

* Water treatment.

Comments

Post a Comment

Popular posts from this blog

SSS 1: ATOMIC STRUCTURE

-
Image
                              Atom An atom is the smallest particle of an element which can take part in a chemical reaction.                 Components of an atom An atom has two main parts: I. The nucleus (made of proton and neutron) II. The shells (electrons) which surrounds the nucleus at definite distance.                   Structure of an atom                    Sub-particles of an atom An atom is made up of three sub-particles namely: I. Proton II. Electron III. Neutron  Proton and neutron are the nuclear particles found in the nucleus, while the electrons are in constant and continuous motion in the shells at various energy levels around the nucleus.         Characteristics of the sub-particles  ...
Read more

SSS 1: CURRICULUM

-
Image
     FIRST TERM   WEEK 1: INTRODUCTION TO CHEMISTRY WEEK 2: NATURE OF MATTER WEEK 3: SEPARATION TECHNIQUES WEEK 4: PARTICULATE NATURE OF MATTER (1) WEEK 5: PARTICULATE NATURE OF MATTER (2) WEEK 6: C.A WEEK 7: ATOMIC STRUCTURE  WEEK 8: CHEMICAL COMBINATION (BONDING) WEEK 9: KINETIC THEORY OF MATTER (I) WEEK 10: HYDROCARBONS  WEEK 11: REVISION  WEEK 12: EXAMINATION  WEEK 13: RESULT/CLOSING                SECOND TERM  WEEK 1: KINETIC THEORY OF MATTER (II) WEEK 2: CARBON AND ITS COMPOUNDS (I) WEEK 3: CARBON AND ITS COMPOUNDS (II) WEEK 4: ACIDS WEEK 5: BASES AND ALKALIS WEEK 6: FIRST C.A WEEK 7: SALTS WEEK 8: PH AND POH WEEK 9: ORGANIC CHEMISTRY (I) WEEK 10: REVISION WEEK 11: EXAMINATION  WEEK 12: EXAMINATION  WEEK 13: RESULT/CLOSING                 THIRD TERM  WEEK 1: INDUSTRIAL CHEMISTRY WEEK 2: KINETIC THEORY OF MATTER (III) WEEK 3: R...
Read more

SSS 1: PARTICULATE NATURE OF MATTER (II)

-
Image
                Relative Atomic Mass The Relative Atomic Mass (RAM) of an element is the average mass of its atoms compared with one-twelfth (¹/₁₂) of the mass of one atom of carbon-12. The carbon-12 isotope (¹²C) is used as the standard for measuring atomic masses. Relative atomic mass of an element  = average mass of one atom of element     ¹/₁₂ × the mass one carbon -12 atom                     Relative Moleculer Mass Relative Molecular Mass ( RMM ), also called Molecular Weight, is the sum of the relative atomic masses (RAM) of all the atoms present in a molecule. The RMM has no unit (it’s a ratio). It shows how heavy a molecule is compared to ¹/₁₂  of the mass of one atom of carbon-12 (¹²C). Examples: 1. Water (H=1, O=16)  H₂O = (2 × H) + (1 × O)          = (2 × 1) + (16)          = 18 ...
Read more