Answer questions a-c about the Bronsted acid-base reaction below using the identifying letters A-D below eachstructure. The pKa's for the acids of interest are: ethanol (pK,=16.0), and benzoic acid (pK,=4.2).HOCH3ноCH3ADbenzoic acidethoxidebenzoateethanola) The stronger base isb) Its conjugate acid isc) The species that predominate at equilibrium are (two letters, e.g. ac)Submit AnswerRetry Entire Group5 more group attempts remainingPreviousNextEmail InstructorSave and Exitfo

We are given the pKa values of benzoic acid = 4.2 and ethanol = 16.

Answered: Answer questions a-c about the Bronsted…

Organic Chemistry

9th Edition

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Publisher:John E. McMurry

Chapter20: Carboxylic Acids And Nitriles

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Answer questions a-c about the Bronsted acid-base reaction below using the identifying letters A-D below each structure.A table of pKa values for various organic and inorganic acids can be found in the references section.for parts 1 and 2 a) The weaker acid is b) Its conjugate base is c) The species that predominate at equilibrium are (two letters, e.g. AC)
Answer questions a-c about the Bronsted acid-base reaction below using the identifying letters A-D below each structure. The pKa's for the acids of interest are: water (pKa = 15.7), and phenol (pKa = 9.9).a) The stronger base is b) Its conjugate acid is c) The species that predominate at equilibrium are (two letters, e.g. ac)
3. The ranking of the acids in terms of increasing acid strength. 4. The ranking of the conjugate bases in terms of increasing base strength. 5.A justification for the rankings based on the factors that influence the relative stability of the different conjugate bases. I need to answer these for C3H5ClO2, ClCH2CO2, and CH3COOH. (Acetic acid, 3-chloropropanic, and chloroacetic acid). Pleaseeee help I will definitely rate
Given that Ka for acetic acid is 1.8 * 10-5 and that for hypochlorous acid is 3.0 * 10-8, which is the stronger acid?
Aniline C6H5NH2 has a base dissociation constant (Kb) of 4.3 × 10-10. What is the conjugate acid of aniline and what is its acid dissociation constant (Ka)? (SHOW CALCULATION)
The Ka of acetic acid (CH3CO2H) is 1.8x10-5 and the Kb of methylamine (CH3NH2) is 4.4x10-4. Complete the following equilibrium reaction (acid-base reaction) equation and predict the side of the equilibrium that is favored. Explain. Show all your work.
What is the approximate pKa value of acetic acid? Is it protonated or not at pH -10? At pH 7? Please explain your answer.
According to the Evan's pKa table, phenol has a pKa of 9.95. p-Nitro and m-nitrophenol have pKas of 7.14 and 8.35 respectively. Using resonance structures, explain the observed trends in the acidity of these molecules.
Treatment of indene with NaNH2 forms its conjugate base in a Brønsted– Lowry acid–base reaction. Draw all reasonable resonance structures for indene's conjugate base, and explain why the pKa of indene is lower than the pKa of most hydrocarbons.
Write equations for the following acid-base reactions. Label the conjugate acids and bases, and show any inductive stabilization. Predict whether the equilibrium favors the reactants or products. Try to do this without using a table of pKa values, (a) CH3CH2OH + CH3NH- (b) F3CCOONa + Br3C¬COOH(c) CH3OH + H2SO4 (d) NaOH + H2S(e) CH3NH3+ + CH3O- (f) BrCH2CH2OH + F3C¬CH2O-(g) NaOCH2CH3 + Cl2CHCH2OH (h) H2Se + NaNH2(i) CH3CHFCOOH + FCH2CH2COO- (j) CF3CH2O- + FCH2CH2OH
Identify the acid and conjugate base in each reaction. Calculate the pKA for each acid. List them in order from the strongest to weakest acid. The acid-ionization constants, KA, at 25°C are provided for each. C6H5OH + H2O Û H3O+ + C6H5O-, KA = 1.2589254 x 10-10 CH3CO2H + H2O Û H3O+ CH3CO2-, KA = 1.5848 x 10-5 CF6CO2H+H2O Û H3O+ + CF6CO2-, KA = 0.6309
Verify that the equilibrium position for the reaction between phenol and hydroxide ion is on the right by comparing the pKa value of the acid on the left with that of the acid on the right. Which acid is stronger? do the same for the reaction of phenol with hydrogen carbonate ion

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