Please answer all parts to QUESTION 4 ONLY, posted with other questions as first attempt was rejected for lack of information. This is all that is provided. Please answer QUESTION 4 part A and B thoroughly and with explanations. 1. A weak acid HA, has a pK of 5.0. If 1.0 mol of this acid and 0.1 mol of NaOH were dissolved in one liter ofwater, what would the final pH be? (hint: First write the acid base reaction that occurs and use an ice table tofind the concentration of the acid and conjugate base at the end of the reaction.)2. Making a buffer solution. Suppose you add 100 mL of a solution containing 5M of acetic acid to 400 mL of0.5 M NaOH. Write the acid base reaction that is taking place and use an ICE table to show how the number ofmoles of each species changes. What is the final pH of the buffer solution? (The pK of acetic acid is 4.7.)3. a) A weak acid has a pKa of 5.5. A buffer (1L) is prepared by adding NaOH to a 1M solution of the weakacid until the pH=6.0. Calculate the number of moles of HA and A- in the buffer solution.b) 150 ml of 1.0 M HCl is added to the buffer in part a. What reaction is taking place and what will the resultingpH be?4. Ionic Forms of Aspartic Acid. Aspartic acid is a triprotic acid that can undergo three dissociation reactions(a) Given the structure of protonated aspartic acid below, draw the chemical structures of the other three formsthat predominate in aqueous solution as the pH increases. Think about this in terms of a titration, adding OH.What acid base reactions occur? Note that the pKa of the carboxylic acid group (-COOH) nearest the -NH, is2.1, The other -COOH has a pKa of 3.9, and the pKa of the amino group, - NH₂*, is 9.7.HOOHΟ ΘΝΗ3aspartic acidb) Draw the titration curve. What form of aspartic acid would be present at the highest concentration insolutions with the following pHs: 1.0, 4.5, 5.7, 2,0. Explain your answers in terms of the pKa values.

Answered: 4. Ionic Forms of Aspartic Acid.…

Aquaculture Science

3rd Edition

ISBN:9781133558347

Author:Parker

Publisher:Parker

Chapter11: Health Of Aquatic Animals

Section: Chapter Questions

Problem 3KA

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Please answer all parts to QUESTION 4 ONLY, posted with other questions as first attempt was rejected for lack of information. This is all that is provided. Please answer QUESTION 4 part A and B thoroughly and with explanations.

1. A weak acid HA, has a pK of 5.0. If 1.0 mol of this acid and 0.1 mol of NaOH were dissolved in one liter of
water, what would the final pH be? (hint: First write the acid base reaction that occurs and use an ice table to
find the concentration of the acid and conjugate base at the end of the reaction.)
2. Making a buffer solution. Suppose you add 100 mL of a solution containing 5M of acetic acid to 400 mL of
0.5 M NaOH. Write the acid base reaction that is taking place and use an ICE table to show how the number of
moles of each species changes. What is the final pH of the buffer solution? (The pK of acetic acid is 4.7.)
3. a) A weak acid has a pKa of 5.5. A buffer (1L) is prepared by adding NaOH to a 1M solution of the weak
acid until the pH=6.0. Calculate the number of moles of HA and A- in the buffer solution.
b) 150 ml of 1.0 M HCl is added to the buffer in part a. What reaction is taking place and what will the resulting
pH be?
4. Ionic Forms of Aspartic Acid. Aspartic acid is a triprotic acid that can undergo three dissociation reactions
(a) Given the structure of protonated aspartic acid below, draw the chemical structures of the other three forms
that predominate in aqueous solution as the pH increases. Think about this in terms of a titration, adding OH.
What acid base reactions occur? Note that the pKa of the carboxylic acid group (-COOH) nearest the -NH, is
2.1, The other -COOH has a pKa of 3.9, and the pKa of the amino group, - NH₂*, is 9.7.
HO
OH
Ο ΘΝΗ3
aspartic acid
b) Draw the titration curve. What form of aspartic acid would be present at the highest concentration in
solutions with the following pHs: 1.0, 4.5, 5.7, 2,0. Explain your answers in terms of the pKa values.

Expert Solution

Step 1: Ionic forms of Aspartic acid

Aspartic acid is a triprotic acid, It can give 3 protons from 3 ionizable groups

from the carboxylic group near to NH₃⁺
From the amino group
From the side chain carboxyl group

with pKa values 2.1,9.7 and 3.9 respectively. Remember of pKa values are the pH at which half of the group deprotonate. For example pKa for side chain is 3.9 which indicates half of the side chain carboxylic acid deprotonates and becomes negatively charged. When the pH increases further then deronated form also increases. When the amino group loses protons loses the positive charge but carboxylic group has negative charge while deprotonate.

The 3 predominant ionic forms as pH increases