**Problem: Net Charge Determination at Different pH Levels on a Given Molecule****9. Given the pKa's indicated, determine the net charge on the molecule shown below when it is in aqueous solution at pH 2.3, 7.6, and 14.**The molecule's structure includes the following ionizable groups:- Carboxylic acid group (pKa = 5)- Phenolic hydroxyl group (pKa = 10)- Amino group (pKa = 11)[Image of the molecule with indicated pKa values]**Net Charge Calculation Table:**| pH | 2.3 | 7.6 | 14 ||----|-----|-----|----|| Net Charge | ___ | ___ | ___ |**Graph and Diagram Explanation:**The molecule features three ionizable groups, each with its own pKa value:- A carboxylic acid group with a pKa of 5.- A phenolic hydroxyl group with a pKa of 10.- An amino group with a pKa of 11.**Determining Charges at Different pH Values:**- **pH 2.3:** At pH 2.3, the environment is acidic. - The carboxylic acid group (pKa = 5) remains protonated and neutral. - The phenolic group (pKa = 10) remains protonated and neutral. - The amino group (pKa = 11) remains protonated and positively charged (+1). Net Charge at pH 2.3: +1- **pH 7.6:** At pH 7.6, the environment is near neutral. - The carboxylic acid group (pKa = 5) will deprotonate and have a negative charge (-1). - The phenolic group (pKa = 10) remains protonated and neutral. - The amino group (pKa = 11) remains protonated and positively charged (+1). Net Charge at pH 7.6: 0- **pH 14:** At pH 14, the environment is highly basic. - The carboxylic acid group (pKa = 5) remains deprotonated and negatively charged (-1).

Answered: Image /qna-images/answer/95e08687-af75-4706-bb2b-632b7bbe240d.jpg

9. Given the pka's indicated, determine the net charge on the molecule shown below when it is in aqueous solution at pH 2.3, 7.6 and 14. pka = 5 O pH 2.3 7.6 14 H NH₂ H net pK₂ = 11 charge H pka: = 10

9. Given the pka's indicated, determine the net charge on the molecule shown below when it is in aqueous solution at pH 2.3, 7.6 and 14. pka = 5 O pH 2.3 7.6 14 H NH₂ H net pK₂ = 11 charge H pka: = 10

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

(Q17) What is the pH of a solution that is 0.596 M in sodium formate (NaCHO2)? The Ka of formic acid is 1.8 x 10-4.
Chemistry H,N. CH, H,N. HO, но Phenylalanine (1) Tyrosine (2) H,C HN CH, H,C `CH, H,C но Triethylamine (4) N-acetyl-OMe-Tyrosine (3) All four compounds are dissolved in ethyl acetate. If you started by extracting the solution with 1 M HCI, which of the following compounds would end up in the aqueous layer? 4 12 Instead, you decide to start by extracting the ethyl acetate solution with 5% NaHCO3 (sodium bicarbonate). What will remain in the organic layer? 1 2 4
Benzoic acid(C6H5-COOH) is a weak acid(pKa=4.2) and naphthalene is neutral, neither acidic or basic. Prepare a flowchart for the separation and recovery of benzoic acid and naphthalene.
5. The titration curve below is two amino acids. Identify the amino acids based on the titration curve. pH 12 10 8 6 4 2 1 2 3 4 NaOH equivalence 5
Calculate the Ka for the weak acid knowing the pKa value is 13.07
Which will change the value of Ksp for BaCrO4? O removing Ba²+ions to the solution increasing the temperature of the solution O increasing the pH of the solution O removing CrO4²-ions form the solution
Which of the following acid/conjugate base pairs has a pKa value of 9.44? A. Ammonium/ammonia B. carboxylic acid/carboxylate C. imidazolium/imidazole
Given: Concentration, Volume, Temperature (20C) Calculated: Molarity, Concentration of OH- and Ca2+ What is the information needed to know if Ksp will increase or decrease with temperature? What is the effect on Ksp when temperature is increased?
What is the pKa of Sylvianic Acid if it is 2.3% dissociated at pH = 10.26?
b. You have 100 mLs of a 2 M histidine solution at pH 6.0, how many mls of a 5 M KOH solution must be added to bring the pH to exactly 7.0? Report your answer to 1 decimal point - assume no change in volume