Unit 3: Equilibrium, Acids and Redox

The shape of titration curves for strong and weak acid-base combinations, equivalence point versus end point, and choosing an indicator by pKa.

The Bronsted-Lowry model, conjugate acid-base pairs, strong versus weak acids and bases, the self-ionisation of water, and pH and pOH calculations.

Writing half-equations, balancing atoms and charge in acidic solution, and combining oxidation and reduction halves into a full ionic equation.

How a weak acid and its conjugate base resist pH change, the action of buffers when acid or base is added, and calculating buffer pH.

How catalysts lower activation energy, the difference between homogeneous and heterogeneous catalysts, enzymes, and the effect on the energy profile and Maxwell-Boltzmann distribution.

Dynamic equilibrium, the equilibrium constant Kc, the reaction quotient Q, and using Le Chatelier's principle to predict how concentration, pressure and temperature changes shift a system.

Collision theory, activation energy, the Maxwell-Boltzmann distribution, and how concentration, temperature, surface area and pressure change the rate of reaction.

The electrochemistry of rusting, the roles of oxygen and water, and prevention methods including barriers, sacrificial anodes and cathodic protection.

Galvanic and electrolytic cells, electrodes and salt bridges, the standard electrode potential table, calculating cell EMF, and predicting spontaneity.

Quantitative electrolysis using charge equals current times time, the Faraday constant, and calculating mass or gas volume from charge passed.

Exothermic and endothermic reactions, enthalpy change, energy profile diagrams, and calorimetry calculations using q equals mcT.

Writing the equilibrium constant expression, calculating Kc from equilibrium concentrations, interpreting its magnitude, and the effect of temperature on Kc.

The ideal gas equation, molar gas volume at standard conditions, and using gas data in stoichiometric calculations.

Hess's law, energy cycles, calculating enthalpy changes from enthalpies of formation, and estimating enthalpy from average bond enthalpies.

Oxidation numbers, the meaning of oxidation and reduction as electron transfer, identifying oxidants and reductants, and balancing redox half-equations and full ionic equations.

The solubility product Ksp, relating Ksp to molar solubility, the common ion effect, and predicting whether a precipitate forms.

The mole, molar mass, the Avogadro constant, mole-ratio calculations from balanced equations, limiting reagent, and percentage yield.

Using titration data to find an unknown concentration, the mole-ratio method, standard solutions, and back titration.

The acid dissociation constant Ka and pKa, calculating the pH of a weak acid solution, and the relationship between Ka and acid strength.