### Acid Dissociation Constants (Kₐ) and Conjugate BasesIn this section, we will explore the acid dissociation constants (Kₐ values) of different acids and determine the formula for the strongest conjugate base. The Kₐ value is a measure of the strength of an acid in solution; lower values indicate weaker acids.1. **Phenol (a weak acid)**, $ \text{C}_6\text{H}_5\text{OH} $: - **Kₐ**: $1.00 \times 10^{-10}$2. **Hydrofluoric Acid (HF)**: - **Kₐ**: $7.20 \times 10^{-4}$3. **Acetylsalicylic Acid (aspirin)**, $ \text{HC}_9\text{H}_7\text{O}_4 $: - **Kₐ**: $3.00 \times 10^{-4}$Given these values, the **strongest conjugate base** is associated with the **weakest acid**, which has the lowest Kₐ value.#### Task**What is the formula for the strongest conjugate base?**\[ \boxed{\hspace{1cm}} \]The provided information presents the Kₐ values for phenol, hydrofluoric acid, and acetylsalicylic acid. Based on this information, students are expected to determine that the strongest conjugate base comes from phenol, as it has the lowest Kₐ value, indicating it is the weakest acid of the three listed.

Weak acids acidic strength can be measured by Ka value When a weak acid HA dissolved in water…

Answered: Ką for phenol (a weak acid), CH5OH, is…

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Chemistry

Ką for phenol (a weak acid), CH5OH, is 1.00×10-10.

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

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Question

### Acid Dissociation Constants (Kₐ) and Conjugate Bases

In this section, we will explore the acid dissociation constants (Kₐ values) of different acids and determine the formula for the strongest conjugate base. The Kₐ value is a measure of the strength of an acid in solution; lower values indicate weaker acids.

1. **Phenol (a weak acid)**, $ \text{C}_6\text{H}_5\text{OH} $:
- **Kₐ**: $1.00 \times 10^{-10}$

2. **Hydrofluoric Acid (HF)**:
- **Kₐ**: $7.20 \times 10^{-4}$

3. **Acetylsalicylic Acid (aspirin)**, $ \text{HC}_9\text{H}_7\text{O}_4 $:
- **Kₐ**: $3.00 \times 10^{-4}$

Given these values, the **strongest conjugate base** is associated with the **weakest acid**, which has the lowest Kₐ value.

#### Task
**What is the formula for the strongest conjugate base?**

\[ \boxed{\hspace{1cm}} \]

The provided information presents the Kₐ values for phenol, hydrofluoric acid, and acetylsalicylic acid. Based on this information, students are expected to determine that the strongest conjugate base comes from phenol, as it has the lowest Kₐ value, indicating it is the weakest acid of the three listed.

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