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Question 2-17 You want to maintain a pH = 7.0 for an enzyme-catalyzed reaction that will...

Question 2-17

You want to maintain a pH = 7.0 for an enzyme-catalyzed reaction that will produce hydrogen ions along with the desired product. At equal concentrations, which weak acid, if any, will serve as the better buffer for the reaction: Acid A, with pKa = 6.5 or Acid B, with pKa = 7.5?

a. Acid A

b. Water is as good as either of the acid available

c. Acid B

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Expert Solution

You want to maintain pH = 7.0 for an enzyme-catalyzed reaction that will produce hydrogen ions along with the desired product. At equal concentrations, which weak acid, if any, will serve as the better buffer for the reaction:

Acid A, with pKa = 6.5 or Acid B, with pKa = 7.5

Acid A with pKa = 6.5 is preferred (Option A) : According to Henderson - Hasselbalch equation :

pH = pKa + log [conjugated base]/[acid]

Effective buffer range is pH = pKa +/- 1

Both the buffers are in this range and also with equal concentration.

The requirement is to maintain a pH = 7.0 for an enzyme-catalyzed reaction that will produce hydrogen ions along with the desired product.

So the acid which is more acidic in nature will be better buffer for this reaction.

An Acid A is a stronger acid and easily dissociates to produce hydrogen ions than the acid B because acid A has lower pKa (6.5) value than the pKa of acid B (7.5)

Lower the pKa then greater the Ka value and greater the acidity.

Hence option A i.e acid A is better option

queen_honey_blossom answered 1 year ago
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