CHEMISTRY FORM 2
- 1.1 Structure of the atom
- 1.2 Atomic Number and Mass Number
- 1.3 Isotopes
- 1.4 Energy levels and electron arrangement
- 1.5 Development of the Periodic Table
- 1.6 Relative Atomic Mass and Isotopes
- 1.7 Ion Formation
- 1.8 Chemical Formulae
- 1.9 Chemical Equations
- 2.1 Alkali metals (Group I elements)
- 2.2 Alkali Earth Metals (Group II elements)
- 2.3 Halogens (Group VII elements)
- 2.4 Noble gases (Group VIII elements)
- 2.5 Properties and Trends Across the Periodic Table
- 3.1 Bond
- 3.2 Ionic bond
- 3.3 Giant ionic structure
- 3.4 Covalent bond
- 3.5 Co-ordinate bond
- 3.6 Molecular structures
- 3.7 Giant covalent structures
- 3.8 Metallic Bond
- 3.9 Types of bond across a period
- 3.10 Oxides of elements in Period 3
- 3.11 Chlorides of Period 3 elements
- 4.1 What is a salt?
- 4.2 Types of salt
- 4.3 Solubility of salts in water
- 4.4 Methods of preparing salts
- 4.4.1 Reacting a Metal with an Acid
- 4.4.2 Reacting an Acid with a Base (Neutralization)
- 4.4.3 Reacting an Acid with a Carbonate (or hydrogencarbonate of metal)
- 4.4.4 Combining elements Directly (Direct Combination of elements)
- 4.4.5 Precipitation (Double decomposition)
- 4.5 Action of heat on salts
- 4.6 Uses of salts
- 5.1 Electrical conduction
- 5.2 Electrical conductivity of molten substances
- 5.3 Electrical conductivity of substances in aqueous state
- 5.4 Electrolysis
- 5.5 Applications of electrolysis
- 6.1 Allotropes of carbon
- 6.2 Chemical properties of carbon
- 6.3 Carbon (IV) oxide
- 6.4 Carbon (II) oxide (CO)
- 6.5 Large scale production of sodium carbonate and sodium hydrogencarbonate
- 6.6 Effect of carbon (II) oxide and carbon (IV) oxide on the environment
- 6.7 Carbon cycle
Salts: Solubility of salts in water
4.0 Salts
4.3 Solubility of salts in water
Observe the photographs on solubility of salts to classify them as soluble and insoluble salts.
Questions 4.3(a)
- Referring to Table 4.3, indicate whether a salt is soluble (Yes) or not soluble (No).
Table 4.3: List of selected salts
- What is the conclusion about the solubility of sodium, potassium and ammonium salts?
- What is true about chlorides? State the exception?
- What can you say about the solubility of nitrates?
- What can you say about the solubility of sulphates? What are the exceptions?
- What is true about the solubility of carbonates? What are the exceptions?
- What is true about the solubility of hydrogencarbonates?
- Are majority of salts soluble or insoluble?
- Make one or two statements that can help us identify a salt as soluble or insoluble.
Answers to Questions 4.3(a)
Conclusion
Sulphates of lead and barium, silver chloride, and all carbonates except of sodium, potassium and ammonium ion are insoluble. All the other salts are soluble.
Figure 4.3: Summary of solubility of salts
This conclusion can help us classify a given salt as soluble or insoluble.
NB: Hydrogencarbonates exist for sodium, potassium, calcium, magnesium and ammonium ions only. Aluminium carbonate does not exist.
Questions 4.3(b)
Predict the solubility of the following salts, using YES to indicate soluble and NO to mean insoluble. Give a reason for each answer.
Table 4.3(b): Predicted solubility
Answers to Questions 4.3(b)