Lesson Notes By Weeks and Term v4 - SHS 3
EQUILIBRIA
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EQUILIBRIA
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Subject: Chemistry
Class: SHS 3
Term: 2nd Term
Week: 5
Grade code: 1.1.1.LI.3
Strand code: 1
Sub-strand code: 2
Content standard code: 1.1.2.CS.1
Indicator code: 1.1.1.LI.3
Theme: PHYSICAL CHEMISTRY
Subtheme: EQUILIBRIA
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This lesson delves into the practical side of chemical equilibria, specifically focusing on solubility equilibria. We will explore how the principles of solubility can be used as a powerful tool in qualitative analysis to identify unknown ions in a solution. This skill is not just for the examination hall; it is fundamental in many real-world applications in Ghana, such as testing the quality of our drinking water from boreholes or sachet water to detect harmful metal ions, assessing soil samples for farming, and in medical laboratory diagnostics. By understanding how different ions react to form precipitates, we can systematically uncover the chemical composition of substances around us.
A. The Link to Equilibria: Solubility Product (Ksp)
Qualitative analysis is a direct application of the principles of solubility equilibria. For a sparingly soluble salt like Silver Chloride (AgCl), an equilibrium exists in a saturated solution:
AgCl(s) ⇌ Ag⁺(aq) + Cl⁻(aq)
The solubility product constant, Ksp, is the product of the ion concentrations at equilibrium: Ksp = [Ag⁺][Cl⁻].