Acids and Bases Arrhenius Definitions When reacting with
Acids and Bases • Arrhenius Definitions: – When reacting with water, • Acids release hydrogen ions (ex: HNO 3) • Bases release hydroxide ions (ex: Na. OH) • 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. • Na. OH – Sodium hydroxide • Ca. Cl 2 – 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 H 2 SO 4 – Sulfuric acid • H 2 SO 3 – Sulfurous acid Episode 1101
Examples • • • H 3 PO 4 Phosphoric acid HF Hydrofluoric acid HCl. O 2 Chlorous acid • Name the following acids: • HBr • HNO 3 • HNO 2 • HI Episode 1101
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