1. Acids and Bases Arrhenius Definitions: – When reacting with water, Acids release hydrogen ions (ex: HNO 3 ) Bases release hydroxide ions (ex: NaOH) Salts are ionic compounds that release neither hydrogen ions nor hydroxide ions Episode 1101

2. 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

3. 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

4. Operational Definition Bases: – Bitter taste – Slippery – Electrolytes – Turn acid – base indicators different colors – React with acids to produce salt and water Episode 1101

5. Naming Bases and Salts To name bases and salts follow the standard rules for naming ionic compounds. NaOH – Sodium hydroxide CaCl 2 – Calcium chloride Episode 1101

6. Naming Acids Binary Acid Only two elements First element is hydrogen Named - - hydro _____ic acid HCl – Hydrochloric acid Episode 1101

7. 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 H 2 SO 4 – Sulfuric acid H 2 SO 3 – Sulfurous acid Episode 1101

8. Examples H 3 PO 4 Phosphoric acid HF Hydrofluoric acid HClO 2 Chlorous acid Name the following acids: HBr HNO 3 HNO 2 HI Episode 1101