Which of the following explains why alpha-amino acids, the building blocks of proteins, are nearly 1000 times more acidic thanaliphatic carboxylic acids?H3N.R.An a-amino acidAn aliphatic acidpK, 5pKa = 2O Inductive effects of the aliphatic group destabilize the conjugate base.O Inductive effects of the amino group help stabilize the conjugate base.O Inductive effects of the aliphatic groups help stbilize the conjugate base.O Inductive effects of the amino group destabilize the conjugate base.

Strong acids are those in which the conjugate base of this acid is stable. As amino are stronger…

Answered: Which of the following explains why…

Organic Chemistry

9th Edition

ISBN:9781305080485

Author:John E. McMurry

Publisher:John E. McMurry

Chapter20: Carboxylic Acids And Nitriles

Section20.4: Substituent Effects On Acidity

Problem 7P: Dicarboxylic acids have two dissociation constants, one for the initial dissociation into a...

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Similar questions

Calculate the pKa of each acid and indicate which is the stronger acid. C6O2H8, Ka = 1.7 x 10–5 C2O4H2, Ka = 5.9 x 10–2
Calculate the pKa of a acid at 25°C if its conjugate base has a pKb = 1.19
A weak acid has a pKa of 7.6. What is the proportion of A- to HA if pH is 9.08? Round to one decimal place. Thank You!
3. Rank the following acids in order from strongest to weakest.HA (pKa = 2.55) H2Z (pKa1 = 4.35) H3X (pKa1 = 3.17) HY (pKa = 5.72) 4. Rank each base in order from strongest to weakest.B (pKb = 4.12) Y– (pKa = 5.72 for conjugate acid) A– (pKa = 2.55 for conjugate acid)E (pKb = 8.12)
Using their Ka values, what is the pKb1 of 0.10 M chloroacetic acid 0.20 M carbonic acid 0.40 M citric acid
Dimethylamine (CH3)2NH is a weak base with a pKa of 11.0 Calculate the pH of a solution of dimethylamine at 0.10 mol.L-1. Calculate the pH of a solution of dimethylamine at 1.0 x 10-2 mol.L-1
A naturally occurring amino acid such as alanine has a group that is a carboxylic acid and a group that is a protonated amine. a. If the pKa value of a carboxylic acid such as acetic acid is about 5 (see Table 2.1), then why is the pKa value of the carboxylic acid group of alanine so much lower? b. Draw the structure of alanine in a solution at pH = 0. c. Draw the structure of alanine in a solution at physiological pH (pH 7.4). d. Draw the structure of alanine in a solution at pH = 12. e. Is there a pH at which alanine is uncharged (that is, neither group has a charge)? f. At what pH does alanine have no net charge (that is, the amount of negative charge is the same as the amount of positive charge)?
Given that the Ka value for acetic acid is 1.8 × 10−5 and the Ka value for hypochlorousacid is 3.5 × 10−8, which is the stronger base, OCl− or C2H3O2−?
What percent of acetic acid is present in the acidic form at pH 5.0, assuming a pKa of 4.8?
Dicarboxylic acids have two pKa's.- For maleic acid (cis-2-butenedioic acid) these are pKa1 = 2.0, and pKa2 = 6.3- For fumaric acid (trans-2-butenedioic acid) these are pKa1 = 3.0, and pKa2 = 4.5 Which factor best explains why the cis-isomer has a smaller pKa1 and a larger pKa2 than the trans-isomer? a. Intramolecular hydrogen bonding b. Intramolecular steric hindrance c. Selective solvation in water d. Intramolecular dipole repulsion
15.What would be the pH of a 0.25 M solutionof phenylamine (C6H5NH2) at room temperature? The Kb of phenylamine is 4 × 10^−10. 1. 132. 10.5 3. 94. 15. 5
1.95 grams of ethanolamine were dissolved in water, and the pH of the solution was adjusted with HCl until 62% of the molecules were in their protonated (conjugate acid) state. The pKa of ethanolaminium (the conjugate acid of ethanolamine) is 9.5. What is the pH of the final solution? Round your answer to one decimal place (e.g., 2.3) using standard rounding conventions for the last digit.

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