**Bronsted-Lowry Acid Behavior of Phenol**To illustrate the behavior of phenol (a weak acid), C₆H₅OH, as a Bronsted-Lowry acid in water, we need to write a net ionic equation. **Diagram Explanation:**The diagram consists of a chemical equation setup with labels indicating the roles of the reactants and products:1. **Reactants:** - **BL acid:** An empty box indicating where the formula for the Bronsted-Lowry acid (C₆H₅OH) should be placed. - Plus sign (+) followed by: - **BL base:** H₂O (water) acts as the Bronsted-Lowry base in this reaction.2. **Arrow (→):** Indicates the direction of the reaction.3. **Products:** - **BL base:** An empty box indicating where the formula for the conjugate base (C₆H₅O⁻) should be placed. - Plus sign (+) followed by: - **BL acid:** An empty box indicating where the formula for the conjugate acid (H₃O⁺) should be placed.**Overall Reaction Notes:**- The phenol (C₆H₅OH) donates a proton (H⁺) to water (H₂O), transforming into its conjugate base (C₆H₅O⁻), while water becomes its conjugate acid (H₃O⁺).- This exemplifies the Bronsted-Lowry acid-base theory, where an acid donates a proton, and a base accepts a proton.

(a) Bronsted Lowry Acid : In this, BL Acid will give its proton to form conjugate base . (b)…

Answered: Write a net ionic equation to show that…

Write a net ionic equation to show that phenol (a weak acid), C6H5OH, behaves as a Bronsted-Lowry acid in water. BL acid BL base BL base BL acid + H2O +

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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Concept explainers

Ionic Equilibrium

Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.

Arrhenius Acid

Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.

Bronsted Lowry Base In Inorganic Chemistry

Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.

Question

**Bronsted-Lowry Acid Behavior of Phenol**

To illustrate the behavior of phenol (a weak acid), C₆H₅OH, as a Bronsted-Lowry acid in water, we need to write a net ionic equation.

**Diagram Explanation:**

The diagram consists of a chemical equation setup with labels indicating the roles of the reactants and products:

1. **Reactants:**
- **BL acid:** An empty box indicating where the formula for the Bronsted-Lowry acid (C₆H₅OH) should be placed.
- Plus sign (+) followed by:
- **BL base:** H₂O (water) acts as the Bronsted-Lowry base in this reaction.

2. **Arrow (→):** Indicates the direction of the reaction.

3. **Products:**
- **BL base:** An empty box indicating where the formula for the conjugate base (C₆H₅O⁻) should be placed.
- Plus sign (+) followed by:
- **BL acid:** An empty box indicating where the formula for the conjugate acid (H₃O⁺) should be placed.

**Overall Reaction Notes:**
- The phenol (C₆H₅OH) donates a proton (H⁺) to water (H₂O), transforming into its conjugate base (C₆H₅O⁻), while water becomes its conjugate acid (H₃O⁺).
- This exemplifies the Bronsted-Lowry acid-base theory, where an acid donates a proton, and a base accepts a proton.

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