Please correct answer and don't used hand raiting Acetic acid (pKa 4.76) and trifluoroacetic acid (aka TFA; pKa 0.25) are similarin structure and both have carboxylic acid functional groups that make themacidic. What is the primary rationale for why trifluoroacetic acid has arelatively different acidity than the very similar structure of acetic acid?the overall molecule of acetic acid is bigger than TFAonly the acetic acid has a resonance structure that stabilizes its conjugate baseonly the TFA has a resonance structure that stabilizes its conjugate baseacetic acid has more inductive withdraw that stabilizes its conjugate base thandoes the TFATFA has more inductive withdraw that stabilizes its conjugate base than does theacetic acidTFA has less inductive withdraw that stabilizes its conjugate base than does theacetic acid

Acetic acid (top) and trifluoroacetic acid are both acidic due to their carboxylic group. The only…

Answered: Acetic acid (pKa 4.76) and…

Organic Chemistry

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Chapter20: Carboxylic Acids And Nitriles

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The pka for 2-hydroxybenzoic acid (i.e. salicylic acid, used in pain relief and a precursor for aspirin) is 2.98, while the pKa for 3-hydroxybenzoic acid (found in castoreum, a scent- marking substance secreted by beavers) is 4.08. What does this difference in pK₂ tell us about the relative acidities of these two compounds?, Why is there such a significant difference? OH OH 2-hydroxybenzoic acid (pKa = 2.98) OH OH 3-hydroxybenzoic acid (pKa 4.08)
At pH 3.0, what percentage (in %) of lactic acid is in its deprotonated form? Hint: The pka of lactic acid is 3.86.
4. The pk, of vanillin is about 9, which is much more acidic than a normal alcohol. Draw a reaction showing the deprotonation of vanillin with NaOH, and then draw six resonance structures of the conjugate base. Draw the hybrid structure and clearly indicate how the negative charge is distributed in the compound.
Acetic, formic, hydrofluoric, and acetylsalicylic acids have the following values of pKa (25°C), respectively: 4.74, 3.74, 3.17, 3.49. Order these acids in order acidity (from highest to lowest acidity)
но HO но он The pK, of ascorbic acid (vitamin C) is 4.17, showing that it is slightly more acidic than acetic acid (CH3CO0H, pKa 4.74). (a) Show the fou r different conjugate bases that would be formed by deprotonation of the four different OH groups in ascorbic acid. (b) Compare the stabilities of these four conjugate bases, and predict which OH group of ascorbic acid is the most acidic. (c) Compare the most stable conjugate base of ascorbic acid with the conjugate base of acetic acid, and suggest why these two compounds have similar acidities, even though ascorbic acid lacks the carboxylic acid (COOH) group.
Sulfuric acid (H2SO4) has a pKa value of -10 and it is almost completely ionized in water. Write the ewis structure for the conjugate base of sulfuric acid. Draw all the possible resonance structures for the corresponding conjugate base.
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The Ka1 of ascorbic acid is 7.94 x 10°. Would you expect ascorbic acid dissolved in blood plasma (pH 7.35-7.45) to exist primarily as ascorbic acid or as ascorbate anion? From the choices provided below, indicate whether the carboxylic acid will exist primarily in its protonated form as a Free Acid or in its deprotonated form as a Carboxylate Anion by clicking on the corresponding button. At equilibrium in this pH, the concentration of the preferred form of the acid is approximately times higher than the concentration of its conjugate form. Round to the nearest order of magnitude.
Suppose you have a mixture of these three compounds. Devise a chemical procedure based on their relative acidity or basicity to separate and isolate each in pure form.
The pKa values of the carboxylic acid groups of oxaloacetic acid are 2.22 and 3.98.a. Which carboxyl group is the stronger acid?b. The amount of hydrate present in an aqueous solution of oxaloacetic acid depends on the pH of the solution: 95% at pH 0, 81% at pH 1.3, 35% at pH3.1, 13% at pH 4.7, 6% at pH 6.7, and 6% at pH 12.7. Explain this pH dependence.
The pkb of methylamine, CH3NH2, is 3.36. Calculate the pka of its conjugate acid, CH3NH3*. pka =
(i) Draw the dissociation reaction for a carboxylic acid in water and define the Ka for this reaction. Write the equation that relates pKa to Ka. (ii) A deprotonated carboxylic acid can be drawn in two resonance forms. Draw the two forms and explain what the term “resonance” means. (iii) Draw an energy profile for the above dissociation reaction and describe how the profiles for a strong and a weak acid would differ.

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