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16 Cards in this Set
- Front
- Back
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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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Bronsted-Lowry acid
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H+/proton donor
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Bronsted-Lowry base
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H+/proton acceptor
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Arrhenius acid
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produces H+/H3O+ in water
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Arrhenius base
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produces OH- in water
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strong acid
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-fully dissociates in water
-proton donating power of strong acid is greater than proton donating power of H3O+ -HI, HClO4, HBr, HCl, HClO3, H2SO4, HNO3 |
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weak acid
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-does not fully dissociate in water (equilibrium)
-proton donating power of weak acid is less than proton donating power of H3O+ -reactions that favor weak acid tend to proceed in reverse |
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conjugate see-saw
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-the stronger the acid, the weak the base and vice versa
-the bigger Ka, the smaller Kb and vice versa |
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strong base
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-proton-accepting power of strong base is greater than proton-accepting power of OH-
-O(2-), H-, NH2 (-), CH3 (-), NaOH, KOH |
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weak base
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-proton-accepting power of weak base is less than proton-accepting power of OH-
-NH3, OAc-, F- |
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Ka
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[H3O+][A-]/[HA]
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Kb
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[OH-][B+]/[BOH]
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Kw
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Kw = KaKb = 1.0 x 10-14
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pH, pOH
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pH = -log [H3O+]
pOH = -log [OH-] pH + pOH = 14 |
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auto-ionization of water
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2H2O (l) <-> H3O+ (aq) + OH- (aq)
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