Descriptions & Reactions Acids & Bases Descriptions & Reactions

HCl + H2O  H3O+ + Cl– Descriptions – + Arrhenius - In aqueous solution… Acids form hydrogen ions (H+) or hydronium ions (H3O+) HCl + H2O  H3O+ + Cl– H Cl O – + acid

NH3 + H2O  NH4+ + OH- Descriptions – + Arrhenius - In aqueous solution… Bases form hydroxide ions (OH-) NH3 + H2O  NH4+ + OH- H N O – + base

Another common way to refer to hydrogen ions is to call them “protons” Descriptions Another common way to refer to hydrogen ions is to call them “protons” Brønsted-Lowry Acids are proton (H+) donors. Bases are proton (H+) acceptors. HCl + H2O  Cl– + H3O+ acid conjugate base base conjugate acid Conjugate acid – particle formed when a base gains a H+ Conjugate base – particle that remains when an acid has donated a H+

Descriptions Lewis Lewis base Lewis acid Acids are electron pair acceptors. Bases are electron pair donors. Lewis base Lewis acid

Descriptions Strong Acid/Base Ionize completely in water - + Strong Acid/Base Ionize completely in water strong electrolyte HCl HNO3 H2SO4 HBr HI HClO4 NaOH KOH Ca(OH)2 Ba(OH)2

Descriptions Weak Acid/Base ionize partially in water weak electrolyte - + Weak Acid/Base ionize partially in water weak electrolyte HF CH3COOH H3PO4 H2CO3 HCN NH3

Neutralization Chemical reaction between an acid and a base. Products are a salt (ionic compound) and water.

ACID + BASE  SALT + WATER Neutralization ACID + BASE  SALT + WATER HCl + NaOH  NaCl + H2O strong strong neutral HC2H3O2 + NaOH  NaC2H3O2 + H2O weak strong basic