SPM Chemistry (KSSM) Paper 1

05 Chemical Bonds
5.1 Formation of Compounds
1 Lesson
5.1.1 Formation of Compounds
5.2 Ionic Bonds
2 Lessons
5.2.1 Formation of Ion
5.2.2 Ionic Bonding
5.3 Covalent Bonds
1 Lesson
5.3.1 Covalent Bonding
5.4 Hydrogen Bonds
5.5 Dative Bonds
5.6 Metallic Bonds
5.7 Ionic and Covalent Compounds
1 Lesson
5.7.1 Properties of Ionic and Covalent Compounds
5.8 Chemical Bonds - Practices (Coming Soon)
06 Acids, Bases and Salts
6.1 The Role of Water in Acidic and Basic Properties
3 Lessons
6.1.1 Acids
6.1.2 Bases and Alkali
6.1.3 The Role of Water in Acidic and Basic Properties
6.2 Meaning of pH and Determination of pH
1 Lesson
6.2.1 Meaning of pH and Determination of pH
6.3 Strength of Acids and Alkalis
1 Lesson
6.3.1 Strength of Acids and Alkalis
6.4 Chemical Properties of Acids and Alkalis
3 Lessons
6.4.1 Chemical Properties of Acids
6.4.2 Chemical Properties of Alkalis
6.4.3 Writing Ionic Equation of The Reaction of Acids and Alkalies
6.5 Concentration of Aqueous Solution
2 Lessons
6.5.1 Concentration of Aqueous Solution
6.5.2 Molarity and Number of Moles
6.6 Standard Solution
2 Lessons
6.6.1 Standard Solution
6.6.2 Dilution
6.7 Neutralisation
2 Lessons
6.7.1 Neutralisation
6.7.2 Acid-Base Titration
6.8 Salts, Crystals and Their Uses in Daily Life
1 Lesson
6.8.1 Introduction to Salts
6.9 Preparation of Salts
4 Lessons
6.9.1 Solubility of Salts, Oxide and Hydroxide
6.9.2 Preparing Salts
6.9.3 Preparing Soluble Salts
6.9.4 Preparing Insoluble Salts
6.10 Action of Heat on Salts
2 Lessons
6.10.1 Identifying Gases
6.10.2 Effect of Heat on Salts
6.11 Qualitative Analysis
3 Lessons
6.11.1 Colour of Salts
6.11.2 Identifying Anions
6.11.3 Identifying Cations
6.12 Acids, Bases and Salts - Practices (Coming Soon)
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6.4.1 Chemical Properties of Acids

SPM Chemistry (KSSM) Paper 1 6.4 Chemical Properties of Acids and Alkalis 6.4.1 Chemical Properties of Acids
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Chemical Properties of Acids

  1. Acids have the following chemical properties:
    1. Acid + Reactive Metal → Salt + Hydrogen gas
    2. Acid + Metal Carbonate → Salt + Water + Carbon Dioxide gas
    3. Acid + Base oxide → Salt + Water
    4. Acid + Alkali → Salt + Water

Acid + Reactive Metals

  1. Acids react with metals that is more electropositive than hydrogen in the electrochemical series to produce salt and hydrogen gas.
  2. Acids do not react with copper and silver.
  3. This is actually a displacement, where the metals that are placed above hydrogen in Electrochemical Series displace hydrogen from acid.
Acids + Reactive Metal → Salt + Hydrogen Gas

Example:

Sulphuric acid + Zinc
H2SO4 + Zn → ZnSO4 + H2
Nitric acid + Lead
2HN3 +Pb→Pb (NO3)2 + H2

Example of Experiment

Procedure

  1. About 5 cm³ of dilute sulphuric acid is poured into a test tube.
  2. One spatula of zinc powder is added into the acid.
  3. A burning wooden splinter is placed at the mouth of the test tube.
  4. The observations are recorded.


Observation
Colourless gas is released. A “pop” sound produced when the wooden splinter is placed at the mouth of the test tube.


Inference
Hydrogen gas is released

Chemical Equation
H2SO4 + Zn → ZnSO4 + H2

Acid + Carbonate

Acids react with metal carbonates produces salt, water and carbon dioxide

Acids + Metal Carbonate → Salt + Water + Carbon Dioxide Gas

Example:

Sulphuric acid + Lime Stone
H2SO4 +CaCO3 → CaSO4 + CO2 + H2O
Nitric acid + Copper(II) Carbonate
2HNO3 +CuCO3 → Cu(NO3)2 +CO2 + H2O

 

Example of Experiment

Procedure

  1. About 5 cm³ of dilute sulphuric acid is poured into a test tube.
  2. One spatula of calcium carbonate powder is added into the test tube.
  3. The gas released is passed through lime water as shown in the diagram above.
  4. The observations are recorded

Observation
Colourless gas is released. The gas turn lime water chalky.

Inference
Sulphuric acid reacts with calcium carbonate.
The gas released is carbon dioxide.

Chemical Equation:
H2SO4 +CaCO3 → CaSO4 +CO2 + H2O

Acid + Base Oxide

Acids react with bases produces salt and water

Acids + Base Oxide → Salt + Water (Neutralisation)


Example:

Sulphuric acid + Iron(II) Oxide
H2SO4 + FeO→FeSO4 + H2O

Hydrochloric acid + Magnesium Oxide

2HCl + MgO → MgCl2 + H O

Example of Experiment

Procedure

  1. One spatula of copper(II) oxide powders is added to 5cm³ of hydrochloric acid in a test tube.
  2. The mixture is heated slowly and stirred with a glass rod.
  3. The observations are recorded.


Observation

  1. The black solid dissolves.
  2. The colourless solution turns blue.

Inference

  1. The copper(II) oxide powder (the black powder) has reacted with the hydrochloric acid.
  2. The blue colour solution contain copper(II) ions.


Chemical Equation

2HCl + CuO → CuCl2 + H2O

Acid + Alkali​

  1. Acids react with alkali produces salt and water only.
  2. This is called a neutralisation reaction.
Acids + Alkali → Salt + Water (Neitralisation)

Example:

Ethanoic Acid + Sodium Hydroxide

CH3COOH + NaOH → CH3COONa + H2O

Hydrochloric Acid + Ammonia Solution

HCl + NH3 → NH4Cl

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