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CHEM 113- Unit 3

QuestionAnswer
percent dissociation [HA]dissociated/[HA]initial x 100
% dissociation is higher for more dilute initial acid concentrations
polyprotic acid >1 ionizable proton
what Ka value (of a polyprotic acid) controls pH? Ka1
anions of weak acids are weak bases
cations of weak bases are weak acids
small, highly charged metal cations make H3O+
strong acids (6) HCl, HBr, HI, HNO3, HClO4, H2SO4
lewis base donates an electron pair
lewis acid accepts an electron pair
what is formed in lewis acid/base rxns adducts
arrhenius acid H+
arrhenius base OH-
bronsted-lowry acid donates H+
bronsted-lowry base accepts H+
buffers contain a weak acid and its conjugate base (or vice versa) and are resistant to changes in pH
ratio to be a buffer 1:10
buffers have the highest capacity when concentrations of acid and base are equal
the more concentrated a buffer is... the higher its capacity (more base/acid can be added and still work)
useable range of a buffer +-1 unit of the pKa
buffer range the pH range over which the buffer acts effectively
indicators weak acids with distinct color changes between protonated and deprotonated forms
equivalence point when moles of acid=moles of base
equivalence point of strong acids/bases always 7
when does pKa=pH half way through buffer region [HA] and [A-] cancel
pH of weak base/strong acid <7
pH of weak acid/strong base >7
polyprotic acids (in titrations) have as many buffer region/equivalence points as ionizable protons
Created by: melaniebeale
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