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32 Cards in this Set
- Front
- Back
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Equilibrium Constant
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products over reactants, each raised to coefficients from the balanced equation and ignoring pure liquids and solids
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Manipulating Equilibrium Constants
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1) when reaction is reversed, value of Kc is inverted (1/K)
2) when coefficients are multiplied by common factor, Kc is raised to corresponding power 3) when coefficients are divided by common factor, Kc is taken to corresponding root 4) if two reactions are added, new K is product of individual K's |
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Enthalpy Change
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(ΔH) the heat absorbed or released when reaction takes place under constant pressure
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Endothermic Reaction
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ΔH is positive, heat is absorbed, heat is 'reactant'
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Exothermic Reaction
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ΔH is negative, heat is liberated, heat is 'product'
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Entropy
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(S) a measure of the disorder
(+) : products are more disordered than reactants (-) : products are less disordered than reactants |
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Gibbs Free Energy
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(ΔG) determines if there is a net driving force for reactants or products to be formed
ΔG = ΔH - TΔS (-) : spontaneous (+) : nonspontaneous |
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Le Chatlelier's Principle
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when a system at equilibrium is disturbed, the system will react to get back to equilibrium
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Reaction Quotient
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(Q) same form as K, but can be calculated at any time (not just @ equilibrium)
if Q>K : reactants are produced if Q=K : at equilibrium if Q<K : products are produced |
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Solubility Product
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(Ksp) the equilibrium constant for the reaction in which a solid salt dissolves to give its constituent ions in solution
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Common Ion Effect
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a salt will be less soluble if one of its constituent ions is already present in solution
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Coprecipitation
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when a substance whose solubility is not exceeded precipitates along with another substance whose solubility is exceeded
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Complex Ions
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any ion containing two or more ions or molecules that are stable by themselves
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Ligand
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any atom or group of atoms attached to the species of interest
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Lewis Acid
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electron pair acceptor
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Lewis Base
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electron pair donor
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Adduct
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the product of the reaction between a Lewis acid and a Lewis base
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Arrhenius Acid
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produces H3O+, hydronium ion in aqueous solutions
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Arrhenius Base
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produces OH- in aqueous solutions
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Bronsted-Lowry Acid
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H+ donor
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Bronsted-Lowry Base
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H+ acceptor
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Salt
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an ionic compound
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Autoprotolysis
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the reaction of a neutral solvent, in which two molecules of the same species transfer a proton from one to the other thereby producing ions
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Protic Solvents
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have a reactive H+
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Aprotic Solvents
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have no reactive H+
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pH and pOH
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pH = -log[H+]
pOH = -log[OH-] pH + pOH = pKw = 14.00 at 25 C |
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if [H+] > [OH-]
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solution is acidic
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if [H+] < [OH-]
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solution is basic
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if [H+] = [OH-]
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solution is neutral
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Strong acids and bases ...
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are completely dissociated in aqueous solutions
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Weak acids and bases ...
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only partially break apart in water
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Polyprotic Acids and Bases
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can donate or accept more than one proton
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