Acids, Bases, and pH

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Fichas sobre Acids, Bases, and pH, creado por I Shouldn't be awake el 05/05/2018.
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Fichas por I Shouldn't be awake, actualizado hace más de 1 año
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Creado por I Shouldn't be awake hace más de 6 años
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Bronsted-lowry model emphasises Proton transfer
Bronsted-lowry acid Proton donor
Bronsted-lowry base proton acceptor
Conjugate acid-base pairs for HCl and Water HCl + H2O <-> H3O+ + Cl- Acid 1 Base 2 Acid 2 Base 1
Spectator ions are Ions that don't participate in reaction
Express pH to ___ dp 2
pH = [H+(aq)] = pH = -log[H+(aq)] [H+(aq)] = 10^-pH
[H+(aq)] of strong acid [H+(aq)] = [HA(aq)] Totally dissociates
Ka = Ka = [H+(aq)]*[A-(aq)] --------------- [HA(aq)]
Larger the Ka value = Stronger the acid, more it dissociates
pKA = Ka = pKa = -logKa Ka=10^-pKa
Weak acid approximations (2) 1. H+ dissociation from H2O is negligible: [H+(aq)] = [A-(aq)] 2. H+ dissociation from weak acids is tiny so [HA(aq)]start = [HA(aq)]eq
Ka for weak acids Ka = [H+(aq)]^2 / [HA(aq)]
When do approximations fail? When Ka > 10^-2 moldm-3
Kw 1.00*10^-14 mol-2 dm6
Formula for Kw Kw = [H2O] = [OH-(aq)][H+(aq)]
What to keep in mind when dealing with di/tribasic acids/bases? [OH-(aq)] x 2/3 [H+(aq)] x 2/3
% dissociation of acid [H+(aq)] * 100 / [HA(aq)]
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