The structure of the molecule below shows its structure where all of the ionizable/protonatable groups are labeled with their corresponding pKas and are drawnas being in their fully protonated form.С: рКa - 3.9OHHА: pka ~ 9.0H3NN.OH'N.N.D: pKa - 3.5NHH2NNH,B: pКa - 12.5At physiological pH, which of the groups will be deprotonated?O A, B, C, and DO A and BO A and CO Cand DO B and DO A, C, and DWhat is the total charge of the structure at pH 2?What is the total charge of the structure at pH 10?

The -COOH and -NH3+ group of a peptide is deprotonated at pH greater than the pKa value. The…

Answered: The structure of the molecule below…

EBK A SMALL SCALE APPROACH TO ORGANIC L

4th Edition

ISBN:9781305446021

Author:Lampman

Publisher:Lampman

Chapter30: Resolution Of (6)-a-phenylethylamine And Determination Of Optical Purity

Section: Chapter Questions

Problem 1Q

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Experimental observations show that thiocyanate (SCN- ), the conjugate base of thiocyanic acid (pKa = 1.1 at 25 °C), is quite soluble in neutral water at pH > 2. In the space provided below, explain this experimental observation. That is, why does SCN– readily dissolve in water when the pH > 2?
calculate the percentage of ethylenediamine in the predominant form at pH 6.043, pKb1 of ethylenediamine is 4.072 and pKb2 is 7.152 please answer in percentage
The pKa values of the conjugate acids of 2-aminopyridine (6.71) and 4- aminopyridine (9.11) are as shown. Why are these structures so much more basic than pyridine?
The pKa values of the conjugate acids of 2-aminopyridine (6.71) and 4- aminopyridine (9.11) are as shown. Which nitrogen is the more basic in these structures and why?
Using the information in the first picture, solve the problem in the second. I am not good at drawing molecules when determining which structure to use in relationship of pH and pKA. Please explain your answer. Thank you very much!
A dibasic organic acid has a neutralization equivalent of 45+1. Deduce the structure of this organic acid
explain in great detail why the pKa values are what they are and compare them among the three compounds. The conjugate acids that are protonated are drawn in red for each compound. Which one based on the pKa is most acidic and what does that tell you about how basic their lone pairs are?
Complete the following acid-base reactions and predict the direction of equilibrium (to the right or to the left) for each. Justify your prediction by citing values of pKa for the stronger and weaker acid in each equilibrium. For values of acid ionization constants, consult Table 23.2 (Acid Strengths, pKa, of the Conjugate Acids of Selected Amines) and Appendix 2 (Acid Ionization Constants for the Major Classes of Organic Acids). Where no ionization constants are given, make the best estimate from the information given in the reference tables and sections.
Show which of the nitrogen atoms in purine are basic, and which one is not basic. For the nonbasic nitrogen, explain why its nonbonding electrons are not easily available to become protonated.
Draw the structure of the predominant form (principal species) of 1,3-dihydroxybenzene at pH 9.00 and at pH 11.00. What is the second most prominent species at each pH?
Can any functional groups on Risperidone ionize? If so, which ones? Under what conditions? What are the pKa values of these functional groups? Write the structures in their correct ionization state at physiological pH.
What is the predominant form of cyclohexylamine at pH 9.5? Approximately what fraction is in this form?

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