A buffer is prepared by dissolving a base, HONH2, and its conjugate acid, HONH3NO3, in some water. Write equations to show how this buffer neutralizes any added acid or base.
A buffer is prepared by dissolving a base, HONH2, and its conjugate acid, HONH3NO3, in some water. Write equations to show how this buffer neutralizes any added acid or base.
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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![### Buffer Preparation and Neutralization Mechanism
**Task:**
A buffer is prepared by dissolving a base, HONH₂, and its conjugate acid, HONH₃NO₃, in some water. Write equations to show how this buffer neutralizes any added acid or base.
**Explanation:**
1. **Introduction to Buffers:**
Buffers are solutions that resist changes in pH upon the addition of small amounts of acids or bases. They typically consist of a weak acid and its conjugate base, or a weak base and its conjugate acid.
2. **Components:**
- **Base:** Hydroxylamine (HONH₂)
- **Conjugate Acid:** Hydroxylammonium nitrate (HONH₃NO₃)
3. **Buffer Solution Preparation:**
When hydroxylamine (HONH₂) dissolves in water, it partially ionizes:
\[
HONH₂ + H₂O ⇌ HONH₃^+ + OH^-
\]
Hydroxylammonium nitrate (HONH₃NO₃) dissociates as follows:
\[
HONH₃NO₃ ⇌ HONH₃^+ + NO₃^-
\]
4. **Neutralization of Added Acid:**
When an acid, such as HCl, is added to the buffer solution, the conjuguate base (HONH₂) will react with the added H⁺ ions:
\[
HONH₂ + H⁺ ⇌ HONH₃^+
\]
This reaction removes the excess H⁺ ions, minimizing the change in pH.
5. **Neutralization of Added Base:**
When a base, such as NaOH, is added, the conjugate acid (HONH₃^+) will react with the added OH⁻ ions:
\[
HONH₃^+ + OH⁻ ⇌ HONH₂ + H₂O
\]
This reaction neutralizes the excess OH⁻ ions, again minimizing the change in pH.
By these mechanisms, the buffer solution prepared using HONH₂ and HONH₃NO₃ successfully maintains a stable pH when either an acid or base is introduced into the system.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F7c13c2cd-7092-4d54-837b-d1e36936f099%2F184736a3-6f2c-4aea-96d2-2a08c53ad2fc%2Fuvgrstl.jpeg&w=3840&q=75)
Transcribed Image Text:### Buffer Preparation and Neutralization Mechanism
**Task:**
A buffer is prepared by dissolving a base, HONH₂, and its conjugate acid, HONH₃NO₃, in some water. Write equations to show how this buffer neutralizes any added acid or base.
**Explanation:**
1. **Introduction to Buffers:**
Buffers are solutions that resist changes in pH upon the addition of small amounts of acids or bases. They typically consist of a weak acid and its conjugate base, or a weak base and its conjugate acid.
2. **Components:**
- **Base:** Hydroxylamine (HONH₂)
- **Conjugate Acid:** Hydroxylammonium nitrate (HONH₃NO₃)
3. **Buffer Solution Preparation:**
When hydroxylamine (HONH₂) dissolves in water, it partially ionizes:
\[
HONH₂ + H₂O ⇌ HONH₃^+ + OH^-
\]
Hydroxylammonium nitrate (HONH₃NO₃) dissociates as follows:
\[
HONH₃NO₃ ⇌ HONH₃^+ + NO₃^-
\]
4. **Neutralization of Added Acid:**
When an acid, such as HCl, is added to the buffer solution, the conjuguate base (HONH₂) will react with the added H⁺ ions:
\[
HONH₂ + H⁺ ⇌ HONH₃^+
\]
This reaction removes the excess H⁺ ions, minimizing the change in pH.
5. **Neutralization of Added Base:**
When a base, such as NaOH, is added, the conjugate acid (HONH₃^+) will react with the added OH⁻ ions:
\[
HONH₃^+ + OH⁻ ⇌ HONH₂ + H₂O
\]
This reaction neutralizes the excess OH⁻ ions, again minimizing the change in pH.
By these mechanisms, the buffer solution prepared using HONH₂ and HONH₃NO₃ successfully maintains a stable pH when either an acid or base is introduced into the system.
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