Acids and Bases • Arrhenius Definitions: – When reacting with water, • Acids release hydrogen ions (ex: HNO3) • Bases release hydroxide ions (ex: NaOH) • Salts are ionic compounds that release neither hydrogen ions nor hydroxide ions Episode 1101 Expanded Definitions • Bronsted-Lowery Definition: – Acids donate hydrogen ions – Bases receive hydrogen ions – Ampherteric: serves as both an acid and a base • Lewis Definition: – Acids receive electron pairs – Bases donate electron pairs Episode 1101 Operational Definitions • Acids: – Sour taste – React with metals to produce hydrogen gas – Electrolytes – Turn acid – base indicators different colors – React with bases to produce salt and water Episode 1101 Operational Definition • Bases: – Bitter taste – Slippery – Electrolytes – Turn acid – base indicators different colors – React with acids to produce salt and water Episode 1101 Naming Bases and Salts • To name bases and salts follow the standard rules for naming ionic compounds. • NaOH – Sodium hydroxide • CaCl2 – Calcium chloride Episode 1101 Naming Acids • • • • • Binary Acid Only two elements First element is hydrogen Named - - hydro _____ic acid HCl – Hydrochloric acid Episode 1101 Naming Acids • • • • • • • • Ternary Acids Three elements First element is hydrogen Other elements are part of a polyatomic ion Naming does not require a prefix ATE IC ITE OUS H2SO4 – Sulfuric acid • H2SO3 – Sulfurous acid Episode 1101 Examples • • • • • • H3PO4 Phosphoric acid HF Hydrofluoric acid HClO2 Chlorous acid • Name the following acids: • HBr • HNO3 • HNO2 • HI Episode 1101