Experiment 19: Properties of Buffer Solutions for AP Chemistry
For a quick review on equilibrium, refer to the following concepts:
- Le Chatelier's Principle for AP Chemistry
- Acid–Base Equilibrium for AP Chemistry
- Ka, Kw, Kb - The Acid, Water, and Base Dissociation Constant for AP Chemistry
- Buffers for AP Chemistry
- Titration Equilibria for AP Chemistry
- Solubility Equilibria for AP Chemistry
Buffer and non-buffer solutions are prepared. The pHs of these solutions are determined before and after other substances—usually acids or bases—are added.
- pH meter
- volumetric flask
- volumes of the pipeted solutions
- pH of various solutions
The concentrations of the solutions may be calculated by using the dilution equation. Concentrations may then be converted to moles by multiplying the concentration by the liters of solution. This procedure applies to buffer components or any reactant species.
The moles of substances may be determined from the initial moles and stoichiometry. Combined with the liters of solution, these may be used to determine the final concentrations.
The pH values of the solutions may be used in several ways, depending upon the goal of the experiment.
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