На0 () + НОАс (aq) +ъ Нҙо* (аq) + OAc" (аg) the Dissociation Constant Ka of HOAC: Ka = [HOAC]/([H3O*][OAC¯]) Ka = [H3O*][OAc"]/([HOAC][H2O]) Ka = [H3O*][OAc]/[HOAC] Ka = [HOAC][H2O]/([H3O*][OAC¯]) %3D
На0 () + НОАс (aq) +ъ Нҙо* (аq) + OAc" (аg) the Dissociation Constant Ka of HOAC: Ka = [HOAC]/([H3O*][OAC¯]) Ka = [H3O*][OAc"]/([HOAC][H2O]) Ka = [H3O*][OAc]/[HOAC] Ka = [HOAC][H2O]/([H3O*][OAC¯]) %3D
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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![### Dissociation Constant for Acetic Acid (HOAc)
When acetic acid (HOAc) dissociates in water, it follows the reaction:
\[ \text{H}_2\text{O} (\ell) + \text{HOAc} (\text{aq}) \leftrightarrow \text{H}_3\text{O}^+ (\text{aq}) + \text{OAc}^- (\text{aq}) \]
We aim to find the dissociation constant, \(K_a\), for this reaction. The possible expressions for \(K_a\) are as follows:
1. \( K_a = \frac{[\text{HOAc}]}{[\text{H}_3\text{O}^+][\text{OAc}^-]} \)
2. \( K_a = \frac{[\text{H}_3\text{O}^+][\text{OAc}^-]}{[\text{HOAc}][\text{H}_2\text{O}]} \)
3. \( K_a = \frac{[\text{H}_3\text{O}^+][\text{OAc}^-]}{[\text{HOAc}]} \)
4. \( K_a = \frac{[\text{HOAc}][\text{H}_2\text{O}]}{[\text{H}_3\text{O}^+][\text{OAc}^-]} \)
**Explanation:**
- The dissociation constant, \(K_a\), for acetic acid is calculated based on the concentrations of the reactants and products at equilibrium.
- One correct \(K_a\) expression formula for this reaction should consider the ratio of the product of the concentrations of hydronium ion, \(\text{H}_3\text{O}^+\), and acetate ion, \(\text{OAc}^-\), to the concentration of acetic acid, \(\text{HOAc}\).
**Graph/Diagram Analysis (if any):**
- As there is no graph or diagram in the provided information, no specific analysis is provided here. For a complete understanding, consider representing equilibrium concentrations graphically with time if visual aids are required.
For further explanation, students can refer to the topic of acidic dissociation constants in their Chemistry textbooks or online resources.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fcffe6fb8-a8b1-4738-951c-b41ccaeecf4e%2F3b7e7ce8-1746-4f4b-8fed-a806b225a011%2F1hfapqe_processed.png&w=3840&q=75)
Transcribed Image Text:### Dissociation Constant for Acetic Acid (HOAc)
When acetic acid (HOAc) dissociates in water, it follows the reaction:
\[ \text{H}_2\text{O} (\ell) + \text{HOAc} (\text{aq}) \leftrightarrow \text{H}_3\text{O}^+ (\text{aq}) + \text{OAc}^- (\text{aq}) \]
We aim to find the dissociation constant, \(K_a\), for this reaction. The possible expressions for \(K_a\) are as follows:
1. \( K_a = \frac{[\text{HOAc}]}{[\text{H}_3\text{O}^+][\text{OAc}^-]} \)
2. \( K_a = \frac{[\text{H}_3\text{O}^+][\text{OAc}^-]}{[\text{HOAc}][\text{H}_2\text{O}]} \)
3. \( K_a = \frac{[\text{H}_3\text{O}^+][\text{OAc}^-]}{[\text{HOAc}]} \)
4. \( K_a = \frac{[\text{HOAc}][\text{H}_2\text{O}]}{[\text{H}_3\text{O}^+][\text{OAc}^-]} \)
**Explanation:**
- The dissociation constant, \(K_a\), for acetic acid is calculated based on the concentrations of the reactants and products at equilibrium.
- One correct \(K_a\) expression formula for this reaction should consider the ratio of the product of the concentrations of hydronium ion, \(\text{H}_3\text{O}^+\), and acetate ion, \(\text{OAc}^-\), to the concentration of acetic acid, \(\text{HOAc}\).
**Graph/Diagram Analysis (if any):**
- As there is no graph or diagram in the provided information, no specific analysis is provided here. For a complete understanding, consider representing equilibrium concentrations graphically with time if visual aids are required.
For further explanation, students can refer to the topic of acidic dissociation constants in their Chemistry textbooks or online resources.
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