CHEM 131 Lecture Notes - Lecture 19: Nitric Acid, Oxidation State, Barium Hydroxide
31 Oct 2016
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Solubility rules: compounds that are generally soluble: k+, na+, li+, nh4+, no3-, c3h3o2-, cl-, Br-, i-, so4-2: compounds that are generally insoluble: oh-, s-2, co3-2, po4-3. 00021: solubility decreases with cation size, large cations can interact with more sulfate ions, greater than or equal to 35g/100ml is soluble, less than or equal to . 3g/100ml is insoluble. Ionize in water and are electrolytes: acids are proton donors, make h+ in water, two types: binary acids ex. Hno3, h2so4, hclo4: nearly all the rest are weak acids. Base: produces oh- in water, water soluble hydroxides, reactive ions (high enough charge density, ammonia (proton acceptor) and amines. Common acids and bases: strong acids- hcl, hbr, hno3, h2so4, hclo4, weak acids- hc2h3o3, hf, bases- naoh, lioh, koh, ca(oh)2, ba(oh)2, nh3(weak) Electron density push/pulled to oxygen makes h-o bond highly polar, h ionizes easily: sulfurous acid- weak h2so3, sulfuric acid- strong h2so4.
