Summary
Highlights
Acids and bases are fundamental to many everyday products and biological processes. Historically, before atomic theory, acids were identified by their sour taste and corrosive properties, while bases were known for their slippery feel and ability to neutralize acids.
At a molecular level, acids and bases interact by exchanging protons (hydrogen ions) and electrons. Molecules willing to donate protons (or accept electrons) become more negatively charged, while those willing to accept protons (or donate electrons) become more positively charged.
Strong acids aggressively donate all their protons to water, and strong bases aggressively accept protons from water. Weak acids and bases, however, only exchange a few protons with water, reaching an equilibrium where most molecules remain unchanged. Examples of weak acids and bases include vinegar and ammonia, respectively.
Water plays a crucial role in acid-base chemistry, acting as both an acid and a base, facilitating the exchange of protons. When an acid (proton donor) and a base (proton acceptor) interact in water, their effects can cancel each other out, a process known as neutralization.