net ionic equations of all neutralizations between strong acid and strong base
H+ (aq) + OH- (aq) → H-OH (l)
monoprotic
one acid hydrogen, acid that dissolves to put one proton in solution, CH3COOH (the OH group dissociates, not the CH3C)
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10.2, 16/5/25
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net ionic equations of all neutralizations between strong acid and strong base
H+ (aq) + OH- (aq) → H-OH (l)
monoprotic
one acid hydrogen, acid that dissolves to put one proton in solution, CH3COOH (the OH group dissociates, not the CH3C)
diprotic
two acid hydrogens, H2SO4
triprotic
three acid hydrogens, H3PO4
polyprotic
anything with more than one acid hydrogen
analyte
what is being analyzed
titrant
what we neutralize analyte with
determining concentration of analyte
acid/base of unknown concentration is neutralized with base/acid of known concentration
measure volume of titrant required to determine concentration of analyte
equivalence point
point where analyte and titrant added is in stoich ratio
determination of concentration depends of titration stopping here
end point
end of a titration
signalled using acid/base indicators
in a well designed titration procedure…
end point must closely correspond to equivalence point
At equivalence
Number of moles of acid (n subscript a) = number of moles of base (n subscript b)