Write a net ionic equation to show that triethylamine, (C2H5)3N, behaves as a Bronsted-Lowry base in water. BL base BL acid BL acid BL base H2O
Write a net ionic equation to show that triethylamine, (C2H5)3N, behaves as a Bronsted-Lowry base in water. BL base BL acid BL acid BL base 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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When a chemical species is transformed into another chemical species it is said to have undergone a chemical reaction. It consists of breaking existing bonds and forming new bonds by changing the position of electrons. These reactions are best explained using a chemical equation.
Question
![**Transcription for Educational Website**
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**Title:** Understanding Triethylamine as a Bronsted-Lowry Base
**Objective:** To write a net ionic equation demonstrating how triethylamine, \((\text{C}_2\text{H}_5)_3\text{N}\), functions as a Bronsted-Lowry base in water.
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**Instruction:**
Fill in the boxes below to complete the net ionic equation for the reaction of triethylamine in water.
**Equation Template:**
\[
\text{BL base} \square + \text{BL acid} \, \text{H}_2\text{O} \rightarrow \text{BL acid} \square + \text{BL base} \square
\]
**Explanation:**
- **BL base (Box 1):** This represents the Bronsted-Lowry base in the reaction, which should be triethylamine, \((\text{C}_2\text{H}_5)_3\text{N}\).
- **BL acid (Box 2):** Water (\(\text{H}_2\text{O}\)) acts as the Bronsted-Lowry acid in this scenario.
- **Resultant BL acid (Box 3):** Following the base's acceptance of a proton, the resultant should be the conjugate acid of triethylamine.
- **Resultant BL base (Box 4):** After donating a proton, the resultant is the conjugate base formed from water.
**Concepts to Explore:**
- Define and explain Bronsted-Lowry acid-base theory.
- Discuss the role of donor and acceptor molecules in acid-base reactions.
- Explore the relationship between acids and their conjugate bases and bases and their conjugate acids.
**Application:**
This exercise helps understand how organic bases like triethylamine behave in aqueous solutions and reinforces the concepts of the Bronsted-Lowry acid-base theory.
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Transcribed Image Text:**Transcription for Educational Website**
---
**Title:** Understanding Triethylamine as a Bronsted-Lowry Base
**Objective:** To write a net ionic equation demonstrating how triethylamine, \((\text{C}_2\text{H}_5)_3\text{N}\), functions as a Bronsted-Lowry base in water.
---
**Instruction:**
Fill in the boxes below to complete the net ionic equation for the reaction of triethylamine in water.
**Equation Template:**
\[
\text{BL base} \square + \text{BL acid} \, \text{H}_2\text{O} \rightarrow \text{BL acid} \square + \text{BL base} \square
\]
**Explanation:**
- **BL base (Box 1):** This represents the Bronsted-Lowry base in the reaction, which should be triethylamine, \((\text{C}_2\text{H}_5)_3\text{N}\).
- **BL acid (Box 2):** Water (\(\text{H}_2\text{O}\)) acts as the Bronsted-Lowry acid in this scenario.
- **Resultant BL acid (Box 3):** Following the base's acceptance of a proton, the resultant should be the conjugate acid of triethylamine.
- **Resultant BL base (Box 4):** After donating a proton, the resultant is the conjugate base formed from water.
**Concepts to Explore:**
- Define and explain Bronsted-Lowry acid-base theory.
- Discuss the role of donor and acceptor molecules in acid-base reactions.
- Explore the relationship between acids and their conjugate bases and bases and their conjugate acids.
**Application:**
This exercise helps understand how organic bases like triethylamine behave in aqueous solutions and reinforces the concepts of the Bronsted-Lowry acid-base theory.
---
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