Question 2, part c: please see attachedPart a answer:if an initial concentration before equilibrium of c2h4o2 is 0.080 M, what are the equilibrium conc of the three species in the equilibrium:[H3O+]=[C2H3O2-]=1.20x10^-3MPart b answer: a solution in which this reaction takes place is analyzed and found to have [C2H4O2]=0.073M and [C2H3O2-]=0.251M and pH 2.131. Is the system and equilibrium? Calculate QQc=2543.0 x 10^-5Kc=1.81 x 10^-5not at equilibrium ### Equilibrium Concentration Analysis**Question:****c)** If part b) is not at equilibrium, then what will the concentrations of the three species be when the system reaches equilibrium? The following reaction reaches equilibrium and has \( K_c = 1.81 \times 10^{-5} \) at 25°C.\[ \text{C}_2\text{H}_4\text{O}_2(\text{aq}) + \text{H}_2\text{O}(\text{l}) \rightleftharpoons \text{H}_3\text{O}^+(\text{aq}) + \text{C}_2\text{H}_3\text{O}_2^-(\text{aq}) \] This equilibrium equation represents the dissociation of acetic acid (\(\text{C}_2\text{H}_4\text{O}_2\)) in water (\(\text{H}_2\text{O}\)), forming hydronium ions (\(\text{H}_3\text{O}^+\)) and acetate ions (\(\text{C}_2\text{H}_3\text{O}_2^-\)).

Reaction :-C2 H4 O2(aq) + H2O(l) ⇌ H3O(aq)P + C2 H3 O2(aq)-Kc = 1.81 x 10-5Kc = H3O+C2 H3 O2-C2 H4…

Answered: if an initial concentration before…

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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Question 2, part c: please see attached

Part a answer:

if an initial concentration before equilibrium of c2h4o2 is 0.080 M, what are the equilibrium conc of the three species in the equilibrium:

[H3O+]=[C2H3O2-]=1.20x10^-3M

Part b answer: a solution in which this reaction takes place is analyzed and found to have [C2H4O2]=0.073M and [C2H3O2-]=0.251M and pH 2.131. Is the system and equilibrium? Calculate Q

Qc=2543.0 x 10^-5

Kc=1.81 x 10^-5

not at equilibrium

The following reaction reaches equilibrium and has \( K_c = 1.81 \times 10^{-5} \) at 25°C.

\[ \text{C}_2\text{H}_4\text{O}_2(\text{aq}) + \text{H}_2\text{O}(\text{l}) \rightleftharpoons \text{H}_3\text{O}^+(\text{aq}) + \text{C}_2\text{H}_3\text{O}_2^-(\text{aq}) \]

This equilibrium equation represents the dissociation of acetic acid (\(\text{C}_2\text{H}_4\text{O}_2\)) in water (\(\text{H}_2\text{O}\)), forming hydronium ions (\(\text{H}_3\text{O}^+\)) and acetate ions (\(\text{C}_2\text{H}_3\text{O}_2^-\)).

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