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### 22 Cards in this Set

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 Molality m = moles of solutes/ kilograms of solvent mole fraction X = moles of substance/ total moles in solution Van't Hoff Factor i= how many ions one unit of a substance will dissociate into in a solution Boiling point elevation delta T = i(Kb)m Kb= boiling point elevation constant m= molality Freezing point depression delta T = i(Kf)m Kf= freezing point depression constant m= molality Raoult's law (vapor pressure lowering) P = XP^o P= vapor pressure of soln P^o = vapor pressure of pure solvent X = mole fraction of pure solvent Osmotic Pressure eqn lambda = (nRT/V)i = MRTi R= .08201 Latm/molK M= molarity= n/V Density m/V Solubility rule: Alkali Metals Li+, Na+, K+, Rb+, Cs+ are all soluble Solubility rule: All ammonium salts, NH4+ are soluble Solubility rule: Alkaline Earths and Transition metals depends on identity of atom Solubility rule: Nitrate, NO3- soluble Solubility rule:Acetate, C2H3O2- soluble Solubility rule: Cl-, Br-, I- soluble except Ag+, Pb2+, Hg2+2 Solubility rule: Sulfate, (SO4)2- soluble, Except Ag+, Pb2+, Hg2+2, Ca2+, Sr2+, Ba2+ Solubility rule: Hydroxide, OH- insoluble, except w/ alkali metals, Ca2+, Sr2+, and Ba2+ Solubility rule: Carbonate, (CO3)2- insoluble except w/ alkali metals and ammonium Solubility rule: Phosphate, (PO4)3- Insoluble except w/ alkali metals and ammonium Solubility rule:Sulfite, (SO3)2- insoluble except w/ alkali metals and ammonium Solubility rule: Sulfide, S2- insoluble except w/ alkali metals, alkaline earths, ammonium. At lower temp, gas will be....soluble more At higher pressure, gas will be....soluble more