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AnnyKZ [126]
3 years ago
13

Why amino acids are soluble in pH=3 or pH=10 solutions more than it dissolves in pH=7 solutions?

Chemistry
1 answer:
Ray Of Light [21]3 years ago
8 0

Answer:

Solubility is Affected by pH

The pH of an aqueous solution can affect the solubility of the solute. By changing the pH of the solution, you can change the charge state of the solute.

At pH extremes, the amino acid molecules mostly carry a net charge, thus increasing their solubility in polar solvent. At very low or very high pH, the amino acid molecules have increased charge, thus form more salt bonds with water solvent molecules.

An isoelectric point is the pH at which an amino acid exists as its zwitterion. A zwitterion is the dipolar ionic form of an amino acid. ... If the pH is lower (in acidic conditions) than the isoelectric point then the amino acid acts as a base and accepts a proton at the amino group. This gives it a positive change.

An amino acid is usually more soluble in aqueous solvent at pH extremes than it is at a pH near the isolelectric point of the amino acid. (Note that this does not mean that the amino acid is insoluble at a pH near its pI.)

Which of the following statements correctly explains this phenomenon?

(Select all that apply.)

The neutral charge of an amino acid molecule at its isoelectric point will make the molecule hydrophobic.

At pH extremes, the amino acid molecules mostly carry a net charge, thus increasing their solubility in polar solvent.

At very low or very high pH, the amino acid molecules have increased charge, thus form more salt bonds with water solvent molecules.

At pH values far from the isoelectric point, individual amino acid molecules have greater kinetic energy, thus more readily stay in solution.

<h2>Please mark me as brainliest</h2>

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You use 50.00 mL of a 12.0 M solution of HCl solution to make a 500.00 mL solution. What is the concentration of the new solutio
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Answer: 1.0 M molecular sucrose (C₁₂H₂₂O₁₁).


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2) Colligative properties are those physical properties of solutions that depends on the number of solute particles dissolved into the solution.


3) The relation between the number of solute particles and the depresson of the freezing point is proportional: the greater the number of solute particles the greater the freezing point depression.


4) You need to find the solution with the highest freezing point, this is the solution in which the freezing point decreased the least.


5) Then, that is the solution with least number of solute particles.


6) Since all the given solutions have the same molarity (1.0 M), you only have to deal with the possible ionization of the different solutes.


7) NaCl, CaBr₂, AlBr₃, and KCl are ionic compounds, so each unit of them will ionize into two, three, four, and two ions, respectively, while sucrose, being a covalent compound does not dissociate.


Then, 1.0 M solution of sucrose will have less solute particles than the others, and will exhitibit the lowest freezing point depression, meaning that it will have the highest freezing point of the given solutions.



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