Unit 8: Acids and Bases
Acids and bases are essential concepts in chemistry, influencing numerous reactions and biological processes. This chapter discusses various theories of acids and bases, including Arrhenius, Brønsted-Lowry, and Lewis theories, and covers pH calculations, as well as the behavior of strong and weak acids and bases. The chapter concludes with methods for acid-base titrations and the practical applications of these concepts in experimental contexts.
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What we have learnt
- Acids and bases can be defined through various theoretical models that reflect their behaviors in different environments.
- pH calculations for various types of acids and bases allow chemists to predict the outcomes of reactions and the nature of solutions.
- Titrations are quantitative methods for determining the concentration of unknown solutions, using known standards.
Key Concepts
- -- Arrhenius Theory
- Defines acids as substances that increase H+ ions in aqueous solutions and bases as those that increase OH- ions.
- -- BrønstedLowry Theory
- Defines acids as proton donors and bases as proton acceptors, introducing the concept of conjugate acid-base pairs.
- -- Lewis Theory
- Broadens the definition of acids and bases to electron pair acceptors and donors, respectively.
- -- pH Scale
- A logarithmic scale measuring the hydrogen ion concentration of a solution, indicating its acidity or basicity.
- -- AcidBase Titration
- A laboratory method used to determine the concentration of an acid or base by neutralizing it with a base or acid of known concentration.
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