D.20) when a carboxylic acid is placed in water, it reacts with water and an equilibrium is established. The reaction of a carboxylic acids and water is shown below. O || R-C-OH + H₂O carboxylic acid (acid form) O R-C-O + H₂O+ carboxylate ion (base form) In many biochemical applications, it is of interest to understand whether the acid form or the base form of a species is predominant. We use the implications of the Henderson-Hasselbalch Equation to predict the predominant species at any particular pH. The pK, of acetic acid is about 4.74. Is the acid form or base form of acetic acid predominant at physiological pH (~7.4)? PH (7.4 pka 4.74 PH [A-] PH>pka [A-]> [HA] PH=pka [HA] = [A] Base form of acetic acidis predominant.
D.20) when a carboxylic acid is placed in water, it reacts with water and an equilibrium is established. The reaction of a carboxylic acids and water is shown below. O || R-C-OH + H₂O carboxylic acid (acid form) O R-C-O + H₂O+ carboxylate ion (base form) In many biochemical applications, it is of interest to understand whether the acid form or the base form of a species is predominant. We use the implications of the Henderson-Hasselbalch Equation to predict the predominant species at any particular pH. The pK, of acetic acid is about 4.74. Is the acid form or base form of acetic acid predominant at physiological pH (~7.4)? PH (7.4 pka 4.74 PH [A-] PH>pka [A-]> [HA] PH=pka [HA] = [A] Base form of acetic acidis predominant.
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![9.20) when a carboxylic acid is placed in water, it reacts with water and an equilibrium is established. The general form of the
reaction of a carboxylic acids and water is shown below.
O
O
11
||
R-C-OH + H₂O R-C-O + H₂O+
carboxylic acid
(acid form)
carboxylate ion
(base form)
In many biochemical applications, it is of interest to understand whether the acid form or the base form of a species is
predominant. We use the implications of the Henderson-Hasselbalch Equation to predict the predominant species at any
particular pH.
The pK, of acetic acid is about 4.74. Is the acid form or base form of acetic acid predominant at physiological pH (~7.4)?
PH (~7.4)>pka 4.74
pH<pka [HA] > [A-]
PH>pka [A-]> HA]
PH=pka HA] =[A]
Base form of acetic acidis predominant](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fab7421aa-d1f8-448e-9827-892b5c53a390%2Fe99104e5-5db2-4cd1-be6e-c3d31625f2ec%2Fgjyomz_processed.jpeg&w=3840&q=75)
Transcribed Image Text:9.20) when a carboxylic acid is placed in water, it reacts with water and an equilibrium is established. The general form of the
reaction of a carboxylic acids and water is shown below.
O
O
11
||
R-C-OH + H₂O R-C-O + H₂O+
carboxylic acid
(acid form)
carboxylate ion
(base form)
In many biochemical applications, it is of interest to understand whether the acid form or the base form of a species is
predominant. We use the implications of the Henderson-Hasselbalch Equation to predict the predominant species at any
particular pH.
The pK, of acetic acid is about 4.74. Is the acid form or base form of acetic acid predominant at physiological pH (~7.4)?
PH (~7.4)>pka 4.74
pH<pka [HA] > [A-]
PH>pka [A-]> HA]
PH=pka HA] =[A]
Base form of acetic acidis predominant
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