10.2 Neutralization & Acid/base Titrations

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net ionic equations of all neutralizations between strong acid and strong base

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H+ (aq) + OH- (aq) → H-OH (l)

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monoprotic

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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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12 Terms

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net ionic equations of all neutralizations between strong acid and strong base

H+ (aq) + OH- (aq) → H-OH (l)

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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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diprotic

two acid hydrogens, H2SO4

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triprotic

three acid hydrogens, H3PO4

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polyprotic

anything with more than one acid hydrogen

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analyte

what is being analyzed

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titrant

what we neutralize analyte with

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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

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equivalence point

  • point where analyte and titrant added is in stoich ratio

  • determination of concentration depends of titration stopping here

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end point

  • end of a titration

  • signalled using acid/base indicators

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in a well designed titration procedure…

end point must closely correspond to equivalence point

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At equivalence

Number of moles of acid (n subscript a) = number of moles of base (n subscript b)