2) Consider the reaction B: + H3O+ BH + H₂O. For the following named bases: 1) draw the structure of the base, 2) draw the structure of the conjugate acid, 3) give the name of the conjugate acid, and 4) give the approximate pKa value of the acid in multiples of 5. 1-butynide anion Phenyl anion base conjugate acid base njugate acid pka_ pKa Ethoxide anion Acetic acid pKa pKa Ş Ethyl acetoacetate enolate anion pKa Di-isopropylamide anion pKa Triethylamine pKa Diethyl ether pka

2) Consider the reaction B: + H3O+ BH + H₂O. For the following named bases: 1) draw the structure of the base, 2) draw the structure of the conjugate acid, 3) give the name of the conjugate acid, and 4) give the approximate pKa value of the acid in multiples of 5. 1-butynide anion Phenyl anion base conjugate acid base njugate acid pka_ pKa Ethoxide anion Acetic acid pKa pKa Ş Ethyl acetoacetate enolate anion pKa Di-isopropylamide anion pKa Triethylamine pKa Diethyl ether pka

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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Most of the pKa values given in this text were determined in water. How would the pKa values of carboxylic acids, alcohols, ammonium ions (RN+H3) , phenol, and an anilinium ion (C6H5N+H3) + change if they were determined in a solvent less polar than water
Calculate Ka values from the following pKa’s:(a) Acetone, pKa 5 19.3 (b) Formic acid, pKa 5 3.75
Given the Ka values, estimate the pKa value of each of the following acids without using a calculator (that is, is it between 3 and 4, between 9 and 10, and so on?):
3. The pKa,1 and pKa,2 of ortho and para isomers of phthalic acid (diprotic acid) are shown below: Provide an explanation on the differences of their pKa values.
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?
Consider the following compounds that vary from nearly nonacidic to strongly acidic. Draw the conjugate bases of these compounds, and explain why the acidity increases so dramatically with substitution by nitro groups.CH4 CH3NO2 CH2(NO2)2 CH(NO2)3 pKa ≅ 50 pKa = 10.2 pKa = 3.6 pKa = 0.17
Acetic acid (CH3COOH, abbrev HA) is a very common weak acid with pKa = 4.75 (at 25oC and low ionic strength) A] Write down the dissociation equation of the weak acid HA in aqueous solution, derive the respective formulae for the dissociation constant Ka and pKa. B] Calculate pH of the diluted solution of acetic acid with concentration, c = 0.05 mol/dm3 C] What is the approximate pH of the aqueous acetate buffer solution composed of dissolved mixture of acetic acid (HA) and sodium acetate (NaA) in the same respective concentrations? What is the working pH range of acetate buffers? D] How can you prepare exactly 1 dm3 of acetate buffer solution with required pH 5.0 and the total concentration [HA + NaA], c = 0.01 mol/dm3 if the stock solution of acetic acid (HA) with concentration, cHA = 0.1 mol/dm3, anhydrous sodium acetate (NaA, MT = 82.03 g/mol) and purified water are available? E] Acetate buffer solution may be also prepared by the partial neutralization of HA with NaOH: 20 cm3 of…
Explain the reactions involved in separation separation of benzoic acid from mixture contain 3 components 1.Benzoic acid (acidic nature pKa=4.17) 2.Naphthalene (neutral compound) 3.paraNitroaniline(basic compound pKa=12.99
Calculate (to the nearest 0.1%) the proportion of a dose of ebastine (pKa of conjugate acid = 10.3) that will be ionised at pH 7.7. You do not need to include "%" in your answer.
At what pH will 25% of a compound with a pKa of 5.3 be in its basic form?
In each of the following reactions, one of the reagents contains two reactive groups (either acidic or basic). You have to decide which group will be affected under mentioned conditions. To answer this problem correctly I suggest that you use the following strategy: (i) Write the products of the reaction: conjugate acid and conjugate base. Use curved arrows to track the flow of electrons; (ii) Using Table 3.1 of the textbook estimate and write pKa values for all acidic groups you have in the reaction equation including conjugate acid; (iii) If you wrote the correct reaction the estimated pKa values should confirm that the reaction transformation changes stronger acid to weaker acid and stronger base to weaker.