(b) the volume of added base required to reach the equivalence point? That is, the percent dissociation is small enough that initial concentrations can be used in place of equilibrium concentrations.Įxamples 1, 2, 3, & 4 are the titration of a weak acid with a strong base.Įxamples 5, 6, 7, & 8 are the titration of a weak base with a strong acid.Įxample 9 is the titration of the salt of a weak base (making the salt an acid) with a strong base.Įxample 10 is the titration of the salt of a weak acid (making the salt a base) with a strong acid.Īll ten of the above examples are multi-part problems.Įxamples 11 and 12 are single-part problems that have interesting twists concerning how volumes are determined.Įxample #1: Consider the titration of a 24.0 mL sample of 0.105 M CH 3COOH with 0.130 M NaOH.
Unless the original acid and base are both strong, these salts produce an equivalence point solution that is NOT neutral (i.e., pH ≠ 7).įinally, in all the equilibrium calculations below we assume that the 5% rule applies. This ratio may or may not be 1:1.įurthermore, any acid-base reaction produces salts of the original acid and the original base. This means molar amounts of acid and base are present in a ratio (determined by the ratio of the coefficients of the balanced chemical reaction) such that the acid and base have completely reacted with each other. The equivalence point in acid-base titration is the point where stoichiometrically equivalent amounts of acid and base have been brought together. Go to 15 weak acid/base titration problems
Weak acids/bases titrated with strong acids/bases ChemTeam: Weak acids/bases titrated with strong acids/bases
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