Align each lab with each unit. 
UNIT 01 - ATOMS, ELEMENTS & PERIODICITY
TOPIC 1A (LO 1.1): The Mole
TOPIC 1B (LO 1.2): Isotopes and Mass Spectrometry
TOPIC 1C (LO 1.3): Empirical & Molecular Formula
TOPIC 1D (LO 1.4): Pure & Impure
TOPIC 1E (LO 1.5): Atoms & Electronic Configuration
TOPIC 1F (LO 1.6): Photoelectron Spectroscopy
TOPIC 1G (LO 1.7): Periodicity
TOPIC 1H (LO 1.8): Formation of Ions
UNIT 02 - CHEMICAL BONDING I
TOPIC 2A (LO 2.1): Sliding Scale of Bond Type
TOPIC 2B (LO 2.2): Bond Length & Strength
TOPIC 2C (LO 2.3): The Ionic Lattice
TOPIC 2D (LO 2.4): Metallic Bonding & Alloys
TOPIC 2E (LO 2.5): Lewis Structures
TOPIC 2F (LO 2.6): Resonance & Formal Charge
TOPIC 2G (LO 2.7): VSEPR & Hybridization
UNIT 03 - CHEMICAL BONDING II & GASSES
TOPIC 3A (LO 3.1): IMFs & Ion-dipole Forces
TOPIC 3B (LO 3.2): Types of Solids & Properties
TOPIC 3C (LO 3.3): States of Matter
TOPIC 3D (LO 3.4): Ideal Gases
TOPIC 3E (LO 3.5): Gases and Kinetic Molecular Theory
TOPIC 3F (LO 3.6): Deviations from Ideal Behavior
TOPIC 3G (LO 3.7): Solutions & Concentration
TOPIC 3H (LO 3.8): Particulate Diagrams of Solutions
TOPIC 3I (LO 3.9): Chromatography and Distillation
TOPIC 3J (LO 3.10): Solubility of Solutes in Solvents
TOPIC 3K (LO 3.11): Effect of Radiation on Matter
TOPIC 3L (LO 3.12): Photons
TOPIC 3M (LO 3.13): Beer’s Law
UNIT 04 - CHEMICAL REACTIONS
TOPIC 4A (LO 4.1): Chemical & Physical Change
TOPIC 4B (LO 4.2): Equations & Net Ionic Equations
TOPIC 4C (LO 4.3): Particulate Representations of Equations
TOPIC 4D (LO 4.4): Chemical & Physical Change in Terms of Bonds & Forces
TOPIC 4E (LO 4.5): Stoichiometry
TOPIC 4F (LO 4.6): Titrations I
TOPIC 4G (LO 4.7): Types of Chemical Reaction
TOPIC 4H (LO 4.8): Acid-Base Reactions
TOPIC 4I (LO 4.9): REDOX Reactions
UNIT 05 - CHEMICAL KINETICS
TOPIC 5A (LO 5.1): Factors Affecting Rates
TOPIC 5B (LO 5.2): Rate Laws
TOPIC 5C (LO 5.3): Rates, Graphs & Half-Life
TOPIC 5D (LO 5.4): Elementary Steps
TOPIC 5E (LO 5.5): Collision Theory
TOPIC 5F (LO 5.6): Energy Profiles I
TOPIC 5G (LO 5.7): Mechanisms
TOPIC 5H (LO 5.8): Mechanisms & Rate Law
TOPIC 5I (LO 5.9): Intermediates in Rate Determining Steps
TOPIC 5J (LO 5.10): Energy Profiles II
TOPIC 5K (LO 5.11): Catalysts
UNIT 06 - CHEMICAL THERMODYNAMICS I
TOPIC 6A (LO 6.1): Endothermic & Exothermic Reactions
TOPIC 6B (LO 6.2): Energy Diagrams
TOPIC 6C (LO 6.3): Heat
TOPIC 6D (LO 6.4): Calorimetry
TOPIC 6E (LO 6.5): Heating & Cooling Curves
TOPIC 6F (LO 6.6): Enthalpy
TOPIC 6G (LO 6.7): Bond Enthalpy
TOPIC 6H (LO 6.8): Enthalpy of Formation
TOPIC 6I (LO 6.9): Hess’s Law
UNIT 07 - CHEMICAL EQUILIBRIUM
TOPIC 7A (LO 7.1): Dynamic Equilibrium I
TOPIC 7B (LO 7.2): Dynamic Equilibrium II
TOPIC 7C (LO 7.3): Q & K
TOPIC 7D (LO 7.4): Kc & Kp
TOPIC 7E (LO 7.5): Large K & Small K
TOPIC 7F (LO 7.6): Mathematical Manipulation of Q & K
TOPIC 7G (LO 7.7): ICE Tables
TOPIC 7H (LO 7.8): Particulate Representation of Equilibrium
TOPIC 7I (LO 7.9): Le Châtelier’s Principle
TOPIC 7J (LO 7.10): Q versus K and Equilibrium Shifts
TOPIC 7K (LO 7.11): Ksp
TOPIC 7L (LO 7.12): Common Ion Effect
TOPIC 7M (LO 7.13): pH & Equilibrium Shifts
TOPIC 7N (LO 7.14): ∆G°, ∆H°, ∆S° and Solubility
UNIT 08 - ACIDS & BASES
TOPIC 8A (LO 8.1): pH, pOH & Kw
TOPIC 8B (LO 8.2): Strong Acids & Bases
TOPIC 8C (LO 8.3): Weak Acids & Bases, Ka & Kb
TOPIC 8D (LO 8.4): Neutralization, and Partial Neutralization to create a Buffer
TOPIC 8E (LO 8.5): Titrations II
TOPIC 8F (LO 8.6): Structure of Acids & Bases
TOPIC 8G (LO 8.7): pH of Buffers Relative to pKa
TOPIC 8H (LO 8.8): Introduction to Buffers
TOPIC 8I (LO 8.9): Henderson-Hasselbalch
TOPIC 8J (LO 8.10): Capacity of Buffers
UNIT 09 - CHEMICAL THERMODYNAMICS II & ELECTROCHEMISTRY
TOPIC 9A (LO 9.1): Entropy Introduction
TOPIC 9B (LO 9.2): Absolute Entropy & ∆S°
TOPIC 9C (LO 9.3): Gibbs Free Energy & Thermodynamic Favorability
TOPIC 9D (LO 9.4): Kinetic Control
TOPIC 9E (LO 9.5): The Relationship between ∆G° and K
TOPIC 9F (LO 9.6): Coupling
TOPIC 9G (LO 9.7): Electrochemistry I
TOPIC 9H (LO 9.8): Electrochemistry II
TOPIC 9I (LO 9.9): Electrochemistry III,  Non-Standard Conditions
TOPIC 9J (LO 9.10): Quantitative Aspects of Electrolytic Cells
1.   How does the concentration of a colored solution relate to absorbance?
A = ε b c
There is a linear relationship between A and c
That the optimum wavelength to use in a colorimeter or spectrophotometer is that of the complementary color to the color of the solution (i.e., the color that gives the highest absorbance)
The procedure for diluting solutions including appropriate glassware (buret, pipet, volumetric flask, safety)
That this procedure is only useful for colored solutions, often those of transition metals
2.   What is the composition of an alloy?
That alloys are mixtures of metals
That an alloy can be dissolved in an acid to produce a solution of metals ions, and that if the resulting solution is colored, then it can be analyzed using the Beer-Lambert law as outlined 
in experiment 1., above
3.   How can we determine the concentration of an aqueous ion in solution?
Solubility rules
The theory of double displacement precipitation reactions, and how to write a net ionic equation
Simple stoichiometry of solutions
Procedures for simple gravimetric analysis including adding excess reactant to ensure all target ions are precipitated, correct filtering procedure, and the need for washing, drying and careful weighing of precipitates
4.   What is the concentration of an acid?
Neutralization reactions, i.e., acid + base → salt + water
Titration procedure including washing and filling burets and pipets, selection of indicators
How to prepare a standard solution
Titration curves including pH and buffer implications
6.   How can we relate bonding to properties?
The general properties and characteristics associated with ionic, covalent and metallic materials
7.   How efficient are chemical processes?
Solubility rules, precipitation reactions and how to write a net ionic equation
Simple stoichiometry of solutions
Procedures for simple gravimetric analysis including adding excess reactant to ensure all target ions are precipitated, correct filtering procedure, and the need for washing, drying and careful weighing of precipitates
Percentage yield calculations
Atom Economy calculations (% atom economy = [mass of desired product/mass of all products]*100)
How to perform a calculation relating to decomposition of hydrated salts
8.   How can we quantitatively analyze substances using a reduction-oxidation reaction?
A definition and understanding of oxidation and reduction
How to write and combine half-reactions
Common oxidizing and reducing agents and their half-reactions
A procedure for titration
9.   Separation of Mixtures 
That ionic salts will tend to dissolve in polar solvents such as water
That large, covalent molecules (often organic in nature) will tend to dissolve in non-polar (often organic) solvents
Simple filtration techniques
Simple liquid-liquid separation techniques including knowledge of a separating funnel and its use
Basic, gravimetric analysis including filtering, drying and massing
10. How do factors like particle size, concentration and temperature affect the speed of a chemical reaction?
How factors such as particle size, temperature, concentration and catalysts, affect the rate of a reaction
How those factors are explained at the microscopic level based on chemistry concepts (collision theory, activation energy etc.)
Dilution techniques and procedures
11. How can we deduce a rate law experimentally? 
That rate laws can be determined by the initial rate method
The relationship between changes of rate and orders of reaction
The shape and interpretation of graphs as they relate to zeroth, first and second order reactions
12. What is the energy change during the process of dissolving a salt in water?
The application of q = m c ∆T
The relationship between q and enthalpies measured in kJ/mol
A procedure for calorimetry
The energy changes associated with dissolving an ionic solid
That certain glassware offers certain degrees of precision
13. What causes the equilibrium position to shift?
Le Châtelier’s principle, and be able to predict how changes in conditions (stresses) affect the position of an equilibrium
That macroscopic observations such as color changes, pH changes etc., can be used to determine the shift in an equilibrium position
14. What do titration curves tell us about reactions?
The shapes of titration curves for any combination of weak and strong acid
What the dominant species are, in solution, at all points on the curve (including when titrating weak acids and weak bases, halfway to the equivalence point)
That when dealing with weak acids and weak bases in titrations with strong bases and strong acids respectively that buffer solutions are produced
The Henderson-Hasselbalch equation
The difference between equivalence point and end point
15. What makes a good buffer?
What a buffer is
How a buffer works and how to write equations to show the buffering action
The factors that affect a buffers capacity
The factors that affect a buffers pH (i.e., the application of the Henderson-Hasselbalch equation)
Where solutions are buffered in relation to titration curves
The definition of a polyprotic acid
That pH = pKa halfway to the equivalence point
16. What affects the pH and capacity of a buffer?
How to interpret the Henderson-Hasselbalch equation in terms of buffer capacity (the concentration of each component) and the desired pH (ratio of each component)