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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Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.
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Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.
Bronsted Lowry Base In Inorganic Chemistry
Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.
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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)
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