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11 Cards in this Set
- Front
- Back
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acid
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produces H+
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base
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produces OH-
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Bronsted-Lowry Acid and Base
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Acid = donates protons
Base = accepts protons |
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Lewis Acid and Base
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acid = electron-pair acceptor
base = electron-pair donor |
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pH
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ph =
-log[H+] = log(1/[H+]) |
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pOH
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pOH =
-log[OH-] = log(1/[OH-]) |
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Water Dissociation Constant (Kw)
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Kw =
[H+][OH-] = 10^(-14) gives pH + pOH = 14 |
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Percent Ionization
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PI =
(ionized acid concentration at equilibrium) / (initial concentration of acid) x 100% |
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Acid Dissociation Constant (Ka)
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Ka =
[H3O+][A-] / [HA] |
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Base Dissociation Constant
(Kb) |
Kb =
[B+][OH-] / [BOH] |
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Henderson-Hasselbalch Equation
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pH = pKa + log([conjugate base] / [weak acid])
pOH = pKb + log([conjugate acid] / [weak base]) |
