References Submit Answer Use the References to access important values if needed for this question. Determine the pH change when 0.102 mol KOH is added to 1.00 L of a buffer solution that is 0.372 M in HCIO and 0.373 M in CIO™. pH after addition - pH before addition pH before addition = pH change =
References Submit Answer Use the References to access important values if needed for this question. Determine the pH change when 0.102 mol KOH is added to 1.00 L of a buffer solution that is 0.372 M in HCIO and 0.373 M in CIO™. pH after addition - pH before addition pH before addition = pH change =
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...
Related questions
Question
![**Educational Content: Buffer Solution pH Change Analysis**
---
**Objective:**
Learn how to determine the pH change when a base is added to a buffer solution.
**Problem Statement:**
Determine the pH change when 0.102 mol KOH is added to 1.00 L of a buffer solution that is 0.372 M in HClO and 0.373 M in ClO⁻.
**Procedure:**
1. **Calculate the pH before the addition of KOH.**
- Use the Henderson-Hasselbalch equation:
\[
\text{pH} = \text{pKa} + \log \left(\frac{[\text{Base}]}{[\text{Acid}]}\right)
\]
- Identify pKa for HClO.
- Plug in concentrations: [Base] = 0.373 M, [Acid] = 0.372 M.
2. **Calculate the pH after the addition of KOH.**
- The added KOH reacts fully with the weak acid, HClO.
- Adjust concentrations based on the reaction:
\[
\begin{align*}
\text{New } [\text{Acid}] &= [\text{HClO}] - 0.102 \, \text{mol/L}, \\
\text{New } [\text{Base}] &= [\text{ClO}^{-}] + 0.102 \, \text{mol/L}.
\end{align*}
\]
- Calculate new pH using the Henderson-Hasselbalch equation.
3. **Determine the pH change.**
- Subtract the initial pH from the pH after addition.
**Interactive Elements:**
- Input boxes for calculating initial and final pH.
- A "Submit Answer" button to verify calculations.
**Notes:**
- This lesson applies the Henderson-Hasselbalch equation to assess buffer capacity.
- It is a group attempt with automated saving features, ensuring progress is not lost.
- Engage with the problem consecutively through varied attempts to deepen understanding.
**Technical Features:**
- Autosaved progress at time stamps.
- Encourages collaborative problem-solving skills.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F47386969-f92b-4827-b6d7-02bdac2aa892%2F0203fcd6-2352-40d5-9735-b22e279cf708%2Fbr0cuoa_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Educational Content: Buffer Solution pH Change Analysis**
---
**Objective:**
Learn how to determine the pH change when a base is added to a buffer solution.
**Problem Statement:**
Determine the pH change when 0.102 mol KOH is added to 1.00 L of a buffer solution that is 0.372 M in HClO and 0.373 M in ClO⁻.
**Procedure:**
1. **Calculate the pH before the addition of KOH.**
- Use the Henderson-Hasselbalch equation:
\[
\text{pH} = \text{pKa} + \log \left(\frac{[\text{Base}]}{[\text{Acid}]}\right)
\]
- Identify pKa for HClO.
- Plug in concentrations: [Base] = 0.373 M, [Acid] = 0.372 M.
2. **Calculate the pH after the addition of KOH.**
- The added KOH reacts fully with the weak acid, HClO.
- Adjust concentrations based on the reaction:
\[
\begin{align*}
\text{New } [\text{Acid}] &= [\text{HClO}] - 0.102 \, \text{mol/L}, \\
\text{New } [\text{Base}] &= [\text{ClO}^{-}] + 0.102 \, \text{mol/L}.
\end{align*}
\]
- Calculate new pH using the Henderson-Hasselbalch equation.
3. **Determine the pH change.**
- Subtract the initial pH from the pH after addition.
**Interactive Elements:**
- Input boxes for calculating initial and final pH.
- A "Submit Answer" button to verify calculations.
**Notes:**
- This lesson applies the Henderson-Hasselbalch equation to assess buffer capacity.
- It is a group attempt with automated saving features, ensuring progress is not lost.
- Engage with the problem consecutively through varied attempts to deepen understanding.
**Technical Features:**
- Autosaved progress at time stamps.
- Encourages collaborative problem-solving skills.
Expert Solution
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
Step by step
Solved in 7 steps
Knowledge Booster
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.Recommended textbooks for you
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY