Consider the reaction of acetic acid in water, where K, = 1.8x10-5.CH3CO,H(aq) + H,0(1) = CH3CO2 (aq) + H30*(aq)(a) Which two bases are competing for the proton? (Select all that apply.)O HCH,CO,O H20O CH;CO,-O H30+(b) Which is the stronger base?O HCH,CO2O H20O CH;CO,O H30*(c) In light of your answer to part (b), why do we classify the acetate ion (CH,CO,) as a weak base?The acetate ion is a ---Select--- v base than water and produces ---Select--- v solutions in water. When the acetate ion is put into solution as the only major --Select--- v species, the competition is betweenthe acetate ion and the hydroxide ion for the proton. The resulting equilibrium lies far to the left producing a K, value of -Select-- v one. ---Select---v is the strongest base possible in water.Species that are classified as weak bases are stronger bases than water but are weaker bases thanSelect---Use an appropriate reaction to justify your answer. (Include states-of-matter at 25°C and 1 atm in your answer.)chemPadО Help->Greek -

Answered: Consider the reaction of acetic acid in…

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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Consider the reaction of acetic acid in water, where K, = 1.8x10-5.
CH3CO,H(aq) + H,0(1) = CH3CO2 (aq) + H30*(aq)
(a) Which two bases are competing for the proton? (Select all that apply.)
O HCH,CO,
O H20
O CH;CO,-
O H30+
(b) Which is the stronger base?
O HCH,CO2
O H20
O CH;CO,
O H30*
(c) In light of your answer to part (b), why do we classify the acetate ion (CH,CO,) as a weak base?
The acetate ion is a ---Select--- v base than water and produces ---Select--- v solutions in water. When the acetate ion is put into solution as the only major --Select--- v species, the competition is between
the acetate ion and the hydroxide ion for the proton. The resulting equilibrium lies far to the left producing a K, value of -Select-- v one. ---Select---
v is the strongest base possible in water.
Species that are classified as weak bases are stronger bases than water but are weaker bases than
Select---
Use an appropriate reaction to justify your answer. (Include states-of-matter at 25°C and 1 atm in your answer.)
chemPad
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According to Bronsted-Lowry theory of acid and base, an acid is a species that give its proton to other species and base is species that can receive a proton.

Generally acids dissociate in water to form proton or hydronium and its conjugate base. Similarly, base dissociates in water form hydroxide ion and conjugate acid.

Acetic acid is a weak acid meaning that it undergoes only partial dissociation in water to produce hydronium ions (H₃O⁺) and acetate ion (CH₃COO^-). Acetate ion is a conjugate base of the weak acetic acid. Water though amphoteric in nature, that is capable of acting as both acid and base at suitable condition, here acts as base and forms hydronium ion.

In the dissociation of acetic acid, there exists an equilibrium between the acetic acid that remains undissociated and acetate ion that dissociated from the acetic acid. The equilibrium constant of the reaction is the acid dissociation constant (K_a).

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