Acids, Bases, and pH

Question	Answer
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)]

Resource summary

	Created by I Shouldn't be awake over 6 years ago