CGIER 41 - Buffer system and Henderson-Hasselbalch equation Flashcards

1
Q

henderson-hasselbalch equation

A
pH = pKa + log(Conjugate base/weak acid)
pH = pKa + log [Ionised or deprotonated acid]/[unionised]
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2
Q

CH3COOH(Acetatic acid) + H2O

A

CH3COO-(Acetate ion) + H3O+

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3
Q

when does the best buffering occur

A

when [acid] = [conjugate base] equal amounts

can with stand changes upon addition of acids and bases to equal extent

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4
Q

useful buffer range

A

pKa +/-1

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5
Q

find an acid that will give good buffering of pH 4

A

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

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6
Q

the greater the amounts of conjugate acid base pair…..

A

the more resistant they are to change in pH

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7
Q

How does concentration influence buffering capacity and what does that mean

A

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

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