2. For each of the following acid-base reactions, (i) draw the expected products; (ii) predict if the reaction will go in the forward or the reverse direction. Completely fill in the circle in front of your answer choice. (Hint: use the approximate pka values given in the textbook.) a. H3N-H + The reaction will go in: the forward direction (equilibrium lies to the right). O the reverse direction (equilibrium lies to the left). b. OH The reaction will go in: + H-CI the forward direction (equilibrium lies to the right). O the reverse direction (equilibrium lies to the left).
2. For each of the following acid-base reactions, (i) draw the expected products; (ii) predict if the reaction will go in the forward or the reverse direction. Completely fill in the circle in front of your answer choice. (Hint: use the approximate pka values given in the textbook.) a. H3N-H + The reaction will go in: the forward direction (equilibrium lies to the right). O the reverse direction (equilibrium lies to the left). b. OH The reaction will go in: + H-CI the forward direction (equilibrium lies to the right). O the reverse direction (equilibrium lies to the left).
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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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
![**Educational Content on Acid-Base Reactions**
**Question 2: Acid-Base Reactions**
For each of the following acid-base reactions:
(i) Draw the expected products.
(ii) Predict if the reaction will proceed in the forward or the reverse direction. Completely fill in the circle in front of your answer choice. (Hint: use the approximate \( pK_a \) values given in the textbook.)
**a.**
\[ \text{H}_3\text{N-H}^+ + \text{O=C-O}^- \leftrightarrow \]
- **The reaction will go in:**
- ☐ The forward direction (equilibrium lies to the right).
- ☐ The reverse direction (equilibrium lies to the left).
**b.**
\[ \text{OH-C(O)H} + \text{H-Cl} \leftrightarrow \]
- **The reaction will go in:**
- ☐ The forward direction (equilibrium lies to the right).
- ☐ The reverse direction (equilibrium lies to the left).
**Diagrams/Equations Explanation:**
- **a.** Involves a protonated amine (ammonium ion) reacting with a carboxylate ion. The arrows indicate a reversible reaction, meaning it can proceed in both directions depending on the conditions.
- **b.** Involves a carboxylic acid reacting with hydrochloric acid (HCl). Again, the reversible arrows indicate that the reaction can shift to either the reactants or products based on equilibrium principles.
The decision of direction is influenced by comparing the \( pK_a \) values of the acids on either side of the reaction. Lower \( pK_a \) means a stronger acid. The equilibrium favors the formation of the weaker acid-base pair.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F0fcb0af8-b750-4635-b3ee-2f0c31e9ebdb%2F230c7c40-b813-46c2-9d09-55ea57c5d763%2Fssh3wpu_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Educational Content on Acid-Base Reactions**
**Question 2: Acid-Base Reactions**
For each of the following acid-base reactions:
(i) Draw the expected products.
(ii) Predict if the reaction will proceed in the forward or the reverse direction. Completely fill in the circle in front of your answer choice. (Hint: use the approximate \( pK_a \) values given in the textbook.)
**a.**
\[ \text{H}_3\text{N-H}^+ + \text{O=C-O}^- \leftrightarrow \]
- **The reaction will go in:**
- ☐ The forward direction (equilibrium lies to the right).
- ☐ The reverse direction (equilibrium lies to the left).
**b.**
\[ \text{OH-C(O)H} + \text{H-Cl} \leftrightarrow \]
- **The reaction will go in:**
- ☐ The forward direction (equilibrium lies to the right).
- ☐ The reverse direction (equilibrium lies to the left).
**Diagrams/Equations Explanation:**
- **a.** Involves a protonated amine (ammonium ion) reacting with a carboxylate ion. The arrows indicate a reversible reaction, meaning it can proceed in both directions depending on the conditions.
- **b.** Involves a carboxylic acid reacting with hydrochloric acid (HCl). Again, the reversible arrows indicate that the reaction can shift to either the reactants or products based on equilibrium principles.
The decision of direction is influenced by comparing the \( pK_a \) values of the acids on either side of the reaction. Lower \( pK_a \) means a stronger acid. The equilibrium favors the formation of the weaker acid-base pair.
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