Please answer the the ones in RED. This experiment will also study the reaction
ID: 870326 • Letter: P
Question
Please answer the the ones in RED.
This experiment will also study the reaction of typical amino acids with H+ and OH- ions. Like other weak acids and bases, amino acids show buffering regions. They have 2 or 2 buffering regions, usually well separated, that represent the transition between protonated and deprotonated forms of one of the ionizable groups. Henderson Hasselbalch relationship explains the derivation of pH as a measure of acidity using pKa, the negative log of the acid dissociation constant as follow Amino acids are also characterized by an isoelectric point, pl, which is the pH at which the amino acid has no net electrical charge. A neutral multiple positive and a negative electrical charge, is called zwitterion, though multiple positive and negative charges can be present. Zwitterions are distinct from dipoles, at different locations within that molecule. For a simple amino acid with only an alpha-carboxyl and alpha-amino group. However, for an amino acid with an ionizable side chain.pl is the average of only two of the three pKa values, the two that involve a neutral species in the ionizable equation. This experiment amino acid is glutamic acid. The theoretical pKa's of glutamic acidExplanation / Answer
Second sheet:
You must explain why those equilibriums happen in that exact order, in other words, you need to explain why a group is more acidic than other.
Carboxylic acids are always more acidic, glutamic acid has two of them, the one near the NH3+ is the more acidic because the inductive effect of NH3+ stabilizes the negative charge in the -COO-, second more acidic is the other carboxylic acid.
Carboxylic acid is more acidic than NH3+ because it can stabilize the generated negative charge by resonance in the oxygens.
Third sheet:
You are explaining H+ dissociation (like you are adding base) and your graphic shows an experiment of HCl addition.
If in you experiment you added HCl then you must explain the equilibriums backwards, protonation of NH2, protonation of COO- far from NH2 and protonation of the stronger carboxylic acid.
Add captions to figure, captions are one or two line explanation of the graphic, i.e: pH of solution vs added HCl (x concentration) .
Fourth sheet
The Henderson-Hasselbach equation is just a form of the equation of acid-base equilibrium constant. Is not relevant to note that the system follows that relationship.
You must correct the