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Acids and Bases
Acids: Properties: Sour taste
Change color of acid-base indicators
Release hydrogen gas
React with bases to produce salt and water
Types: Binary acid: only two elements; hydrogen and another one (HF, HCl)
Oxyacid: Hydrogen, oxygen, and a third element (HNO3, HClO)
-Sulfuric Acid: dehydration, burning
-Nitric Acid: Very volatile, used to make plastics
-Phosphoric Acid: fertilizers
-Hydrochloric Acid: digestion
-Acetic Acid: synthesize chemicals.
Bases: Properties: Bitter taste Change color in acid-base indicators Slippery Also produce salt and water Arrhenius Acids and Bases Acid: increases concentration of H+ ions (protons) Base increases concentration of hydroxide ions (OH-) Strength Strong acids: ionizes completely in aqueous solution Strong polarity Strong Bases: same as acids Alkaline: when a base dissociates to yield aqueous OH- ions Theories Bronsted Lowry: acid: proton donor Base: proton acceptor Reaction: protons are transferred to reach neutralization Monoprotic acid: can donate one proton per molecule Polypotric acid: can donate more than one proton per molecule Dipotric: can donate two per molecule Triprotic: three per molecule Lewis acid and bases Lewis acid: molecule that accepts an electron pair to form covalent bond Lewis base: molecule that donates electron pair Reactions Terms: Conjugate: what remains AFTER the reaction occurs The stronger the acid/base is, the weaker the conjugate will be Amphoteric: Can work as a base or an acid (water) OH-: hydroxyl group. Hydronium and Hydroxide Self-ionization of water: H2O + H20 -> H30 + OH Ph Scale Ph= -log(H3O) Poh= -log(OH) Titration Acid base indictors: compounds whose color is sensitive to Ph cases

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