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=
Organic Chemistry: A Guided Inquiry
2nd Edition
ISBN:9780618974122
Author:Andrei Straumanis
Publisher:Andrei Straumanis
Chapter20: Acidity And Pka Of Phenols
Section: Chapter Questions
Problem 20CTQ
Related questions
Question
![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
pk =
pKa =
K=](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F4fb404b9-8e1c-41d2-a59e-964abbbd4b28%2F9ea35dd1-2846-4e86-ae8f-27f512efb515%2F578yqva_processed.png&w=3840&q=75)
Transcribed Image Text: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
pk =
pKa =
K=
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