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7 Cards in this Set
- Front
- Back
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arrhenius
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acid = increase H+ concentration
base = increases OH- concentration |
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Bronsted-Lowry
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acid = donates H+ ion
base = accepts H+ ion |
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Lewis
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acid = accepts electron pair
base = donates electron pair |
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acid/base ionization constant
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Ka = [H3O+][A-]/[HA}
Kb = [HA][OH-]/[A-] KbKa = Kw pKa + pKb = 14 |
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polyprotic acid
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donates more than one hydrogen ion
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buffers
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-maintain nearly constant pH with smal additions of acid/base
-approx equal amts of acid and conj base |
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Henderson Hasselbalch
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tells why a buffer can maintian constant pH (approx equal to pKa) with small additions of acid/base
[H3O+] = Ka[HA]/[A-] (as long as [H3O+] << [HA][A-]) **can't use when there is only pure HA or A-, aka @ beginning of titration and @ equiv pt |
