Chem - Acids and Bases

Arrhenius acid

dissociates to form an excess of H⁺ in solution, easily identified by H at beginning of formula (i.e. HCl, HNO₃, …)

Arrhenius base

dissociates to form an excess of OH^- in solution, easily identified by OH at end of formula (i.e. NaOH, Ca(OH)₂ …)

Bronsted - Lowry acid

donates hydrogen ions H⁺

Bronsted - Lowry base

accepts hydrogen ions H⁺

Lewis acid

an electron pair acceptor

Lewis base

an electron pair donor

Amphoteric

reacts like an acid in basic environment and like base in acidic environment

Autoionization of water

water reacts with itself to produce hydronium ion and hydroxide ion

Strong acids and bases

completely dissociate into component ions in aqueous solutions (generally written with single-head arrow → to indicate irreversibility)

Weak acids and bases

partially dissociate in aqueous solutions

acid dissociation constant

K_a = [H₃O]⁺ [A^-] / [HA]

Base dissociation constant

K_b = [B⁺] [OH^-] / [BOH]

Neutralization reaction

acids and bases react to form a salt (and often water)

Hydrolysis

salt ions react with water to give back acid or base

Polyvalent

acid or base liberates more than one acid or base equivalent

equivalence point of strong acid/strong base

7

equivalence point of strong acid/weak base

< 7

equivalence point of weak acid/strong base

> 7