LESSON OBJECTIVE: Investigate the relationship between concentration and cell potential both qualitatively and, using the Nernst equation, quantitatively Learning Outcomes: (taken from the Cambridge International AS and A Level Chemistry curriculum) 24.2 Standard electrode potentials E⦵; standard cell potentials E⦵cell and the Nernst equation 6 deduce from E values the relative reactivity of elements, compounds and ions as oxidising agents or as reducing agents 7 construct redox equations using the relevant half-equations 8 predict qualitatively how the value of an electrode potential, E, varies with the concentration of the aqueous ions 9 use the Nernst equation, e.g. E = E⦵ + (0.059/z) log [oxidised species]/[reduced species] to predict quantitatively how the value of an electrode potential varies with the concentrations of the aqueous ions; examples include Cu2+(aq) + 2e- ⇌ Cu(s), Fe3+(aq) + e- ⇌ Fe2+(aq)

LESSON OBJECTIVE: Understand the use of electrolysis quantitatively using changes in electrode mass. Learning Outcomes: (taken from the Cambridge International AS and A Level Chemistry curriculum) 24.1 Electrolysis 2 state and apply the relationship F = Le between the Faraday constant, F, the Avogadro constant, L, and the charge on the electron, e 3 calculate: the quantity of charge passed during electrolysis, using Q = It the mass and/or volume of substance liberated during electrolysis 4 describe the determination of a value of the Avogadro constant by an electrolytic method

LESSON OBJECTIVE: Calculate standard cell potentials (E⦵cell) and use E⦵ values to determine the feasibility of a reaction Learning Outcomes: (taken from the Cambridge International AS and A Level Chemistry curriculum) 24.2 Standard electrode potentials E⦵; standard cell potentials E⦵cell and the Nernst equation 4 calculate a standard cell potential by combining two standard electrode potentials 5 use standard cell potentials to: (a) deduce the polarity of each electrode and hence explain/deduce the direction of electron flow in the external circuit of a simple cell (b) predict the feasibility of a reaction

LESSON OBJECTIVE: Understand how to measure the standard electrode potentials of a half-cell relative to the standard hydrogen electrode. Learning Outcomes: (taken from the Cambridge International AS and A Level Chemistry curriculum) 24.2 Standard electrode potentials E⦵; standard cell potentials E⦵cell and the Nernst equation 2 describe the standard hydrogen electrode 3 describe methods used to measure the standard electrode potentials of: (a) metals or non-metals in contact with their ions in aqueous solution (b) ions of the same element in different oxidation states

LESSON OBJECTIVE: Investigate reaction spontaneity by linking the concepts ΔG⦵ and E⦵cell Learning Outcomes: (taken from the Cambridge International AS and A Level Chemistry curriculum) 24.2 Standard electrode potentials E⦵; standard cell potentials E⦵cell and the Nernst equation 10 understand and use the equation ΔG⦵ = –nE⦵cellF

LESSON OBJECTIVE: Investigate the concept of electrode potential and describe galvanic cells. Learning Outcomes: (taken from the Cambridge International AS and A Level Chemistry curriculum) 24.2 Standard electrode potentials E⦵; standard cell potentials E⦵cell and the Nernst equation 1 define the terms: (a) standard electrode (reduction) potential (b) standard cell potential

LESSON OBJECTIVE: Understand and apply the concepts of solubility products, Ksp, the common ion effect and partition coefficients, Kpc, to a system at equilibrium Learning Outcomes: (taken from the Cambridge International AS and A Level Chemistry curriculum) 25.1 Acids and bases 7 understand and use the term solubility product, Ksp 8 write an expression for Ksp 9 calculate Ksp from concentrations and vice versa 10 a) understand and use the common ion effect to explain the different solubility of a compound in a solution containing a common ion b) perform calculations using Ksp values and concentration of a common ion 25.2 Partition coefficients 1 state what is meant by the term partition coefficient, Kpc 2 calculate and use a partition coefficient for a system in which the solute is in the same physical state in the two solvents 3 understand the factors affecting the numerical value of a partition coefficient in terms of the polarities of the solute and the solvents used

LESSON OBJECTIVE: Understand pH changes in acid-base titrations and how to select an appropriate indicator for certain reactions. Learning Outcomes: (taken from the Cambridge International AS and A Level Chemistry curriculum) 7.2 Brønsted-Lowry theory of acids and bases 9 sketch the pH titration curves of titrations using combinations of strong and weak acids with strong and weak alkalis 10 select suitable indicators for acid-alkali titrations, given appropriate data (pKa values will not be used) 25.1 Acids and bases 4 calculate [H+(aq)] and pH values for: a) strong acids b) strong alkalis c) weak acids

LESSON OBJECTIVE: Describe how buffer solutions regulate pH, calculate buffer solution pH and investigate their applications. Learning Outcomes: (taken from the Cambridge International AS and A Level Chemistry curriculum) 25.1 Acids and bases 5 a) define a buffer solution b) explain how a buffer solution can be made c) explain how buffer solutions control pH; use chemical equations in these explanations d) describe and explain the use of buffer solutions, including the role of HCO3- in controlling pH in blood 6 calculate the pH of buffer solutions, given appropriate data