Ch. 5- Soluble Compounds Soluble Compounds 1. Salts of Na+, K+, NH4+ Salts of NO3-, CLO3-, ClO4-, CH3CO2-2. Salts of Cl-, Br-, I- Except: Ag+, Hg22+, Pb2+ 3 . F- Except :Mg2+, Ca2+, Sr2+, Ba2+,Pb 2+ Strong Acids HCl- Hydrochloric HBr- Hydrobromic HI-Hydroiodic acid HNO3-Nitric Acid HClO4- Perchloric Oxidation Rules 1. Pure element=0 2. Monatomic Ions, = to the charge of the ion 3. Fluorine= -1 4. Cl, Br, and I always have -1 except when combined with oxygen or fluorine. 5. H=+1 O=-2 6 . The algebraic sum of in a Ox Redox LEO says GER Losing Electrons Oxidation Gaining Electrons Reduced Chapter 5-Misc Acid=H+ goes up, (0-7) Base=Oh- goes down, <7 Precipitant- Ch 5 Equations pH=-log H+ Ch. 6 Specific Heat Baked Apple Pie- The greater the specific heat and the larger the mass, the more thermal energy a substance can store.
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