final_study_guide_for_chemistry_(prioritized)

final_study_guide_for_chemistry_(prioritized) - Qsp > Ksp...

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Q sp > K sp rxn will go towards products Q sp < K sp rxn will go towards reactants Q sp = K sp it’s in equilibrium K p = K c (RT) Δn where n is the mol (gases) products – reactants T is temp in K Le Châter’s principle if you add more conc. into reactants, it’ll shift toward the products and vice versa inc. pressure, the rxn will shift toward the side w/ the fewest mol of gas dec. pressure, the rxn will shift toward the side w/ the most mol of gas for exothermic rxn (ΔH < 0), increase in temp results in a dec. in K sp and shift towards reactants for endothermic rxn (ΔH > 0), increase in temp results in a inc. in K sp and shift towards products catalyst only speeds up rxn inert gases don’t do anything solubility is expressed in mol/L K sp is the product constant the smaller Ksp is, the less soluble it is if there are 2 salts with the same formula, the one with the smaller Ksp will precipitate first precipitation will occur if the Ksp value of the salt is exceeded complex ions consists of a metal ion surrounded by two or more anions or molecules
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This note was uploaded on 10/17/2009 for the course BIO 1100 taught by Professor Becker during the Spring '08 term at St. Louis College of Pharmacy.

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final_study_guide_for_chemistry_(prioritized) - Qsp > Ksp...

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