Align each lab with each unit. Each Unit can have only 2 labs max aligned to it. 
UNIT 01 - ATOMS, ELEMENTS & PERIODICITY
UNIT 02 - CHEMICAL BONDING I
UNIT 03 - CHEMICAL BONDING II & GASES
UNIT 04 - CHEMICAL REACTIONS
UNIT 05 - CHEMICAL KINETICS
UNIT 06 - CHEMICAL THERMODYNAMICS I
UNIT 07 - CHEMICAL EQUILIBRIUM
UNIT 08 - ACIDS & BASES
UNIT 09 - CHEMICAL THERMODYNAMICS II & ELECTROCHEMISTRY
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?(Unit 3)
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?(Gravimetric Analysis)
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?(Titration)
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?(Bonding in Solids)
The general properties and characteristics associated with ionic, covalent and metallic materials
7.   How efficient are chemical processes? (Stoichiometry)
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?(Redox Titration)
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 (Physical and Chemical Changes)
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? (Kinetics: Rate of 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? (Kinetics: Rate Laws)
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?(Calorimetry)
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?(Equilibrium)
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? (Acid-Base Titration)
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)