Anthocyanin is a naturally occurring compound that acts as a pigment in many fruits and vegetables. At low pH values (<3), it exists as the cation shown below and exhibits a bright red color. At higher pH values (~7), it exhibits a purple-ish color. As the pH is raised from pH 3 to pH 7, one of the hydroxyl groups can be deprotonated (the H* that is removed has been circled for you) to produce the corresponding resonance stabilized neutral compound. Draw the two most stable resonance structures for this anthocyanin at pH 7. Make sure to explicitly show all non-bonding lone pairs and formal charges where appropriate. Include curved arrows to show how you got from the first resonance structure to the other. first resonance strucure here OH НО. -[sugar] H OH Structure of anthocyanidine at pH 3 H+ second resonance structure here
Ionic Equilibrium
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.
Arrhenius Acid
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.
![Connections to biology
Anthocyanin is a naturally occurring compound that acts as a pigment in many fruits and vegetables. At low
pH values (<3), it exists as the cation shown below and exhibits a bright red color. At higher pH values (~7), it
exhibits a purple-ish color. As the pH is raised from pH 3 to pH 7, one of the hydroxyl groups can be
deprotonated (the H* that is removed has been circled for you) to produce the corresponding resonance
stabilized neutral compound. Draw the two most stable resonance structures for this anthocyanin at pH 7.
Make sure to explicitly show all non-bonding lone pairs and formal charges where appropriate. Include curved
arrows to show how you got from the first resonance structure to the other.
first resonance strucure here
OH
HO.
-[sugar]
H
OH
Structure of anthocyanidine at pH 3
H+
second resonance structure here](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F5b650808-0e30-4865-a4ae-51537c7fc6b8%2F885399fe-8d51-4b06-9920-6ba46c49de8f%2Fqi9o2d_processed.png&w=3840&q=75)
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