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amphiprotic/ amphoteric
can be both and acid or a base
Arrhenius acid
when dissolved in water, increases the concentration of Hydorgen
Arrhenius base
when dissolved in water, increases the concentrations of hydroxide ions
Bronsted-Lowry acid
proton donor
Bronsted-Lowry base
proton acceptor
Lewis acid
electron pair acceptors
Lewis base
electron pair donors
strong acids
HCl, HBr, HNO3, H2SO4, HClO3, HClO4
strong bases
soluble hydroxide, alkali metals (first column) and heavier alkali earth metals (Ca, Sr, Ba)
percent ionization
[H30+]/[HA] x 100
polyprotic acids
pH depends on the first dissociation
K total
Ka1xKa2xKa3…
Find Kb
KaxKb=1E-14
what makes a cation more acidic
greater charge and smaller size
acid strength
increasing polarity of the H-X bond making it easier to remove the H+ ion and increasing the acid strength
acidity increase
left to right across row and top to bottom of group, increases with number of Oxygens
half equivalence point of weak acid
pH=pKa
Note 
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