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27 Cards in this Set
- Front
- Back
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Electrolytes
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Produce ions in solution
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Strong electrolytes
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Completely ionize in solution
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Weak electrolytes
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Partially ionize in solution
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Nonelectrolytes
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Do not ionize in solution
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Dipole
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Molecule has a positive and a negative pole
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Solubility
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Depends on the relative strengths of the attractive forces between its ions or molecules and the forces of hydration
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Overall "Molecular" Equation
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All reactants and products in their undissociated form
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Complete Ionic Equation
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All strong electrolytes are completely dissociated to ions in aqueous solutions
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Spectator Ions
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Present on both sides of the equation (can be canceled)
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Net Ionic Equation
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No spectator ions
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Precipitate
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Insoluble product (salt)
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Driving force of Precipitation Reactions
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The elimination of ions from the solution by formation of an insoluble product
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Arrhenius acids
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Release hydrogen ions H+
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Arrhenius bases
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Release hydroxide ions OH-
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Strong acids
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Almost completely ionized in aq solution
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Strong bases
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Almost completely ionized in aq solutions
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Salt
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An ionic compound with a cation from the base and an anion from the acid
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Neutralization
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Acid + Base -> Salt + Water
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Driving force of strong acid-base reactions
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The elimination of ions from the solution by formation of water
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Oxidizing agent
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Causes oxidation.
Gains electrons. Is reduced. Decreases its ox #. |
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Reducing Agent
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Causes Reduction.
Loses electrons. Is oxidized. Increases its ox #. |
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Oxidation
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Loss of electrons
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Reduction
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Gain of electrons
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Oxidation and Reduction Reactions
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Transfer of electrons from one species to another
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Gas Formation Reactions
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Reactions of salts of weak or volatile acids with strong acids
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Equivalence Point
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The amount of titrant added is stoichiometrically equivalent to the amount of analyte present in the sample
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Activity Series
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Metals higher in the list are stronger reducing agents and can displace (reduce) metals lower in the list from their aqueous solutions
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