f) The reason why acetic acid is more acidic than ethanol. Draw the conjugate bases for each compound and identify the key factor that stabilizes one conjugate base and not the other. ethanol acetic acid pK, = 16 pK, = 5 h) Provide a base that will completely deprotonate propyne (K > 10³) and the conjugate acid of your base. Provide the pKa of propyne and the pKa of the conjugate acid of your base and calculate the equilibrium constant. H3C-=H + + H3C =: Li conjugate acid of your base your base pKa = %3D pKa = K=

f) The reason why acetic acid is more acidic than ethanol. Draw the conjugate bases for each compound and identify the key factor that stabilizes one conjugate base and not the other. ethanol acetic acid pK, = 16 pK, = 5 h) Provide a base that will completely deprotonate propyne (K > 10³) and the conjugate acid of your base. Provide the pKa of propyne and the pKa of the conjugate acid of your base and calculate the equilibrium constant. H3C-=H + + H3C =: Li conjugate acid of your base your base pKa = %3D pKa = K=

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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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.
draw the major organic product of the Bronsted acid-base reaction. Include all lone pairs and charges as appropriate. Ignore any counterions.
Most carboxylic acids have pka's around 4-5. Keeping in mind what makes and carboxylic acid acidic, which of the following compounds would also have a pKa of ~5? OH OH OH ပုံတင် OH
Draw both resonance structures of the anion formed by the reaction of the most acidic C-H bond of the compound below with base. Include all valence lone pairs in your answer. For structures having different hydrogens of comparable acidity, assume that the reaction occurs at the less-substituted carbon. Draw one structure per sketcher. Add additional sketchers using the drop-down menu in the bottom right corner. Separate resonance structures using the ↔ symbol.
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. ata CH3 CH3 -CH3 CH3 CH,- в D ethoxide ethanol dimethylsulfone anion dimethylsulfone a) The weaker base is b) Its conjugate acid is c) The species that predominate at equilibrium are (two letters, e.g. AC)
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3. 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. OH .NO2 OH HO
HW7 #10
Draw the structure of 2-naphthol and highlight the acidic proton.
Indicate which is more acidic: 4-nitrophenol or 4-chlorophenol. Explain the reason.
Phenol (hydroxybenzene) behaves as a weak acid. a) Write out the equilibrium equation for its partial dissociation in water. b) Write out the expression for the acid dissociation constant, Ka. d) Draw the conjugate base of phenol and show how it is stabilised by resonance. e) Compare and explain the acidity of phenol (p = 9.9) with that of: cyclohexanol (pk = 16.0) 3-fluorophenol (pK₁ = 9.3) 4-acetylphenol (pK, = 8.1)