Asked by GeeGee
23.55 ml of the NaOH were added to partially neutralize a new 25.00 ml sample of the acid. The pH of the mixture was measured as 5.33. Calculate Ka for the acid, HA, using the partial neutralization method
Answers
Answered by
DrBob222
I don't think you have typed the entire question. What's missing is the volume of titrant needed to completely titrate (to the end equivalence point) the acid.
Ka = (H^+) x (A^-)/(HA)
You obtain (H^+ from pH in the problem.
fraction A^- = 23.55/V
fraction HA = 1- fraction A^-
where V = volume to reach the equivalence point.
Ka = (H^+) x (A^-)/(HA)
You obtain (H^+ from pH in the problem.
fraction A^- = 23.55/V
fraction HA = 1- fraction A^-
where V = volume to reach the equivalence point.
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