Experiment 8: Oxidation–Reduction Titration for AP Chemistry
For a quick review on stoichiometry, refer to the following concepts:
- Moles, Molar Mass, and Molarity for AP Chemistry
- Percent Composition and Empirical Formulas for AP Chemistry
- Reaction Stoichiometry for AP Chemistry
- Limiting Reactants for AP Chemistry
- Percent Yield for AP Chemistry
The concentration of either an oxidizing or a reducing agent may be determined by titrating a solution of an unknown concentration versus a solution of a known concentration or containing a known mass of solute.
- analytical balance
- drying oven
- Erlenmeyer flask
- pH meter
- support stand
- wash bottle
- volumetric flask
- the volume of a solution of an oxidant or reductant using a pipet
- the initial reading of the buret
- the final reading of the buret at the endpoint of the titration
The volume of titrant added is calculated by the difference between measurements 2 and 3.
The volume of titrant is then converted to liters.
The pipeted volume is converted to moles by multiplying the liters of solution by its molarity. The moles of titrant are determined from the mole ratio in the balanced chemical equation for the reaction. The molarity of the solution is calculated by dividing the moles of titrant by the liters of titrant used.
Common oxidants are potassium permanganate and potassium dichromate.
- Iron(II) and oxalates are commonly chosen as reductants.
Refer to Figure 19.3 for general titration set-up.
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