NHINHS Ammonium ion + amnoonia 4 Buffer syatem ma. Making a buffen r solution with D-10M & 15.0mL aud olpMR15.0mL e canjigate. base The measure eltf the solution is 9.39. Find the Ka & pka ?
NHINHS Ammonium ion + amnoonia 4 Buffer syatem ma. Making a buffen r solution with D-10M & 15.0mL aud olpMR15.0mL e canjigate. base The measure eltf the solution is 9.39. Find the Ka & pka ?
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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Find the Ka and pKa using Ka = ([H3O+] [A])/[HA]
![**Topic: Buffer Systems – Ammonium and Ammonia**
**Buffer System:**
\[ \text{NH}_4^+ + \text{NH}_3 \]
Ammonium + Ammonia
**Problem Statement:**
You are tasked with making a buffer solution. Use 0.10 M and 15.0 mL of acid and 0.10 M and 15.0 mL of conjugate base. The measured pH of the solution is 9.39.
**Objective:**
Find the \( K_a \) and \( pK_a \).
**Notes:**
- Understanding buffer systems is crucial for maintaining stable pH conditions in chemical and biological processes.
- The \( K_a \) value represents the acid dissociation constant, a measure of the strength of an acid in solution.
- \( pK_a \) is the logarithmic form of \( K_a \) and gives insight into the acidity; calculated as \( pK_a = -\log(K_a) \).
**Steps to Solve:**
1. Use the Henderson-Hasselbalch equation:
\[ \text{pH} = pK_a + \log \left(\frac{[\text{Base}]}{[\text{Acid}]}\right) \]
2. Substitute the given values into the equation to find \( pK_a \) and hence \( K_a \).
Understanding how to determine \( K_a \) and \( pK_a \) is essential for calculating the acid strength and predicting chemical behavior.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F331da123-07a7-406d-84cf-688088cb4b31%2Ff28ea6bb-017b-4197-9cb8-8c6c37b09fb2%2Fp800shi_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Topic: Buffer Systems – Ammonium and Ammonia**
**Buffer System:**
\[ \text{NH}_4^+ + \text{NH}_3 \]
Ammonium + Ammonia
**Problem Statement:**
You are tasked with making a buffer solution. Use 0.10 M and 15.0 mL of acid and 0.10 M and 15.0 mL of conjugate base. The measured pH of the solution is 9.39.
**Objective:**
Find the \( K_a \) and \( pK_a \).
**Notes:**
- Understanding buffer systems is crucial for maintaining stable pH conditions in chemical and biological processes.
- The \( K_a \) value represents the acid dissociation constant, a measure of the strength of an acid in solution.
- \( pK_a \) is the logarithmic form of \( K_a \) and gives insight into the acidity; calculated as \( pK_a = -\log(K_a) \).
**Steps to Solve:**
1. Use the Henderson-Hasselbalch equation:
\[ \text{pH} = pK_a + \log \left(\frac{[\text{Base}]}{[\text{Acid}]}\right) \]
2. Substitute the given values into the equation to find \( pK_a \) and hence \( K_a \).
Understanding how to determine \( K_a \) and \( pK_a \) is essential for calculating the acid strength and predicting chemical behavior.
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