The K₂ of a monoprotic weak acid is 0.00493. What is the percent ionization of a 0.103 M solution of this acid? 21.9 percent ionization: Incorrect %

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...
icon
Related questions
icon
Concept explainers
Question
Use the quadratic the Quadratic equation.
 
**Problem:** The \( K_a \) of a monoprotic weak acid is 0.00493. What is the percent ionization of a 0.103 M solution of this acid?

**Answer Box (Incorrect Submission):**
- **percent ionization:** 21.9 %

**Feedback:**
- **Status:** Incorrect 

When working on this problem, use the percent ionization formula for weak acids, which is:

\[ \text{Percent Ionization} = \left( \frac{[\text{H}^+]}{[\text{HA}]} \right) \times 100\]

Where:
- \( [\text{H}^+] \) is the concentration of hydrogen ions after ionization.
- \( [\text{HA}] \) is the initial concentration of the weak acid solution.
 
Further steps typically involve setting up an equilibrium expression involving \( K_a \) and solving for the concentration of ionized acid.
Transcribed Image Text:**Problem:** The \( K_a \) of a monoprotic weak acid is 0.00493. What is the percent ionization of a 0.103 M solution of this acid? **Answer Box (Incorrect Submission):** - **percent ionization:** 21.9 % **Feedback:** - **Status:** Incorrect When working on this problem, use the percent ionization formula for weak acids, which is: \[ \text{Percent Ionization} = \left( \frac{[\text{H}^+]}{[\text{HA}]} \right) \times 100\] Where: - \( [\text{H}^+] \) is the concentration of hydrogen ions after ionization. - \( [\text{HA}] \) is the initial concentration of the weak acid solution. Further steps typically involve setting up an equilibrium expression involving \( K_a \) and solving for the concentration of ionized acid.
Expert Solution
steps

Step by step

Solved in 3 steps

Blurred answer
Knowledge Booster
Ionic Equilibrium
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.
Similar questions
Recommended textbooks for you
Chemistry
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY