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18 Cards in this Set
- Front
- Back
pH of a buffered solution
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Henderson-Hasselbalch equation
pH = pKa + log[conj. base]/[conj.acid] |
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Neutralization
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mixing of equal mole portions of an acid with a base regardless of their concentrations and strengths. (NOTE: does not mean to make the solution pH = 7)
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Equivalence point for a weak acid and strong base
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The point at which the weak acid is completely converted to its conjugate base. pH will be greater than 7 at the equivalence point.
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Buffer
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solutions that resist drastic changes in pH. Make of roughly equal mole mixture of a weak acid and its weak conjugate base.
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Ka
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[H+] x [conj. base]/[weak acid]
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Acid
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Proton donor, electron-pair acceptor, or a compound that yields H30+
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Base
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Proton acceptor, electron-pair donor, or a compound that yields OH- when added to water.
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Arrhenius acid
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yields H30+ when added to H20
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Arrhenius base
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yields OH- when added to H20
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Bronsted-Lowry acid
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Proton donor
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Bronsted-Lowry base
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Proton acceptor
i.e. KOH in protic solvent |
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Lewis Acid
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Electron pair acceptor
i.e. BF3 in aprotic solvent |
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Lewis Base
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Electron pair donor
i.e. NH3 in aprotic solvent |
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Acid Dissociation, Ka
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[H30+]*[A-]/[HA]
10^(-pKa) |
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pKa
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-logKa
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Van der waals forces
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Weak intermolecular attractive forces
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Snell's Law
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n1sin01 = n2sin02
n air approx. = 1 |
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Faraday
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1 mole of electric charge
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