Unit 2: Ionic Equilibrium
2.1 Explain the limitations of Arrhenius's concepts of acid
and bases.
2.2 Define Bronsted and Lowry's concepts for acids and
bases.
2.3 Define conjugate acids and conjugate bases.
2.4 Identify conjugate acid-base pairs of Bronsted acid and
base
2.5 Define and explain Lewis acids and bases.
2.6 Use the extent of ionization and dissociation constant
of acid (Ka) and base (Kb)
2.7 Explain the ionization constant of water and calculate
pH and pOH in an aqueous medium using Kw values.
2.8 Show understanding of, and use, the concept of
solubility product Ksp.
2.9 Calculate Ksp from concentrations and vice versa.
2.10 Show understanding of the common ion effect.
2.11 Describe the application of the solubility product
principle and common ion effect in precipitation reactions.
2.12 Define a Buffer and show with equations how a Buffer
system works.
2.13 Explain the choice of suitable indicators for acid-base
Titrations and describe the changes in pH during acid-base Titrations.
2.14 Define and differentiate different types of salts
(simple salts, double salts, complex salts, acidic salts, basic salts, and
neutral salts).
2.15 Explain hydrolysis of salts (salts of strong acid and
strong base, salts of weak acid and strong base, and salts of weak base and
strong acid)
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December 16, 2023
