CGIER 41 - Buffer system and Henderson-Hasselbalch equation Flashcards
henderson-hasselbalch equation
pH = pKa + log(Conjugate base/weak acid) pH = pKa + log [Ionised or deprotonated acid]/[unionised]
CH3COOH(Acetatic acid) + H2O
CH3COO-(Acetate ion) + H3O+
when does the best buffering occur
when [acid] = [conjugate base] equal amounts
can with stand changes upon addition of acids and bases to equal extent
useful buffer range
pKa +/-1
find an acid that will give good buffering of pH 4
look at list of weak acids
find their pKa and find which one is the closest to 4
closer to 4 greater chance one will have equal amounts of weak acid and conjugate base
the greater the amounts of conjugate acid base pair…..
the more resistant they are to change in pH
How does concentration influence buffering capacity and what does that mean
greater concentration - greater buffering capacity
if a solution of different concentration and pH was added it wouldn’t make a vast difference in the solutions pH