Acids and Bases

Last year, we learned about the nature and reactions of acids and bases. This year, we refine and deepen this understanding, including a better understanding of pH and acid/base strength.

Brønsted-Lowry Acids and Bases

We often simplify our understanding of acids as substance with H⁺ ions, and bases as substance with OH^- ions. Unfortunately, this understanding is inadequate and incorrect.

This year, we use the Brønsted-Lowry definitions. We can use their reactions with water to show the difference between acids and bases:

ACIDS

An acid is a proton donor. This means it loses an H⁺ ion.

HA + H₂O ⇌ H₃O⁺ + A^-

BASES

A base is a proton acceptor. This means it gains an H⁺ ion.

B + H₂O ⇌ OH^- + HB⁺