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About This Unit
In this unit, we will study acids and bases by applying what we learned about chemical equilibrium. Acid-base reactions involve the transfer of protons, or H⁺ ions, and many of these reactions are reversible. This means equilibrium ideas can help us explain pH, acid and base strength, and the concentrations of particles in solution.
We will learn how pH is related to the concentration of H⁺ or OH⁻ in a solution. You will compare strong and weak acids and bases, and explain why some acids produce more H⁺ in solution than others. A major focus will be connecting acid and base strength to equilibrium: large K values mean products are strongly favored, while small K values mean reactants are favored.
We will also look at mixtures of acids and bases, including buffer systems. Buffers are important because they resist large changes in pH. This helps explain how your body maintains a stable pH even when acids or bases are added.
On the AP Chemistry Exam students are expected to connect equilibrium constants, particle-level models, and pH calculations. Strong answers should explain what species are present in the greatest amounts at equilibrium and connect those amounts to acid/base strength, pH, and the value of K.
Essential Questions
- How is pH related to the concentration of H⁺ and OH⁻ in a solution?
- How do acid and base strength affect the concentrations of reactants and products at equilibrium?
- Why do strong acids and bases react essentially to completion in water?
- Why are some acids stronger than others?
- How can equilibrium constants help us compare the strength of acids and bases?
- How can particle-level models help us understand what is present in an acid-base solution?
- How do mixtures of acids and bases affect pH?
- What are buffers, and how do they help resist changes in pH?
- How does your body maintain pH balance?
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