Calculate the pH at the equivalence point when 12.35 mL of a 0.100 M Codeine solution (Kb = 1.6X10-6) is titrated with 0.100 M hydrochloric acid.
Codeine is weak base.
pKb = - log Kb = - log (1.6 * 10^-6) = 5.796
one mole codeine react with one mole HCl.
thus
volume of HCl at equivalence point = 12.35 mL * 0.100 M / 0.100 M = 12.35 ml
total volume of solution = 12.35 + 12.35 = 24.70 ml
thus
concentration salt = 12.35 mL * 0.100 M / 24.70 = 0.05 M
salt hydrolysis occurs.
pH = 1/2 * [pKw - pkb - log C]
or
pH = 0.5 * [14 - 5.796 - log (0.05)]
or
pH = 4.75
pH at the equivalence point = 4.75
Calculate the pH at the equivalence point when 12.35 mL of a 0.100 M Codeine solution...
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