What volume of a 0.101 M barium hydroxide solution is required to neutralize 25.0 mL of a 0.147 M hydrobromic acid solution? mL barium hydroxide Submit Answer Retry Entire Group 9 more group attempts remaining
What volume of a 0.101 M barium hydroxide solution is required to neutralize 25.0 mL of a 0.147 M hydrobromic acid solution? mL barium hydroxide Submit Answer Retry Entire Group 9 more group attempts remaining
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
100%
![### Chemistry Neutralization Problem
**Problem Statement:**
What volume of a 0.101 M barium hydroxide solution is required to neutralize 25.0 mL of a 0.147 M hydrobromic acid solution?
**Answer Box:**
\[ \_\_\_\_\_\_\_\_ \text{ mL barium hydroxide} \]
**Buttons:**
- **Submit Answer**
- **Retry Entire Group**
**Remaining Attempts:**
- 9 more group attempts remaining.
### Explanation
This problem involves the concept of a neutralization reaction, where an acid reacts with a base to produce water and a salt. The task is to determine the volume of barium hydroxide (a base) needed to completely neutralize a given volume and molarity of hydrobromic acid (an acid).
### Extended Support
1. **Understanding the Reaction:**
- The balanced neutralization reaction between barium hydroxide \((\text{Ba(OH)}_2)\) and hydrobromic acid \((\text{HBr})\) can be represented as:
\[
\text{Ba(OH)}_2 + 2\text{HBr} \rightarrow \text{BaBr}_2 + 2\text{H}_2\text{O}
\]
2. **Reaction Stoichiometry:**
- According to the balanced equation, one mole of barium hydroxide reacts with two moles of hydrobromic acid.
3. **Calculations:**
- Find the moles of hydrobromic acid:
\[
\text{Moles of HBr} = \text{Molarity of HBr} \times \text{Volume of HBr} = 0.147 \text{ M} \times 0.025 \text{ L} = 0.003675 \text{ moles}
\]
- Using the stoichiometry, calculate the moles of barium hydroxide required:
\[
\text{Moles of Ba(OH)}_2 = \frac{\text{Moles of HBr}}{2} = \frac{0.003675}{2} = 0.0018375 \text{ moles}
\]
- Finally, determine the volume of barium hydroxide solution needed:
\[
\text](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fb9bc6dc7-2424-4f69-956a-285f3752d785%2F542911a6-5756-4eae-84cf-9e72524a0341%2F9m3cec_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Chemistry Neutralization Problem
**Problem Statement:**
What volume of a 0.101 M barium hydroxide solution is required to neutralize 25.0 mL of a 0.147 M hydrobromic acid solution?
**Answer Box:**
\[ \_\_\_\_\_\_\_\_ \text{ mL barium hydroxide} \]
**Buttons:**
- **Submit Answer**
- **Retry Entire Group**
**Remaining Attempts:**
- 9 more group attempts remaining.
### Explanation
This problem involves the concept of a neutralization reaction, where an acid reacts with a base to produce water and a salt. The task is to determine the volume of barium hydroxide (a base) needed to completely neutralize a given volume and molarity of hydrobromic acid (an acid).
### Extended Support
1. **Understanding the Reaction:**
- The balanced neutralization reaction between barium hydroxide \((\text{Ba(OH)}_2)\) and hydrobromic acid \((\text{HBr})\) can be represented as:
\[
\text{Ba(OH)}_2 + 2\text{HBr} \rightarrow \text{BaBr}_2 + 2\text{H}_2\text{O}
\]
2. **Reaction Stoichiometry:**
- According to the balanced equation, one mole of barium hydroxide reacts with two moles of hydrobromic acid.
3. **Calculations:**
- Find the moles of hydrobromic acid:
\[
\text{Moles of HBr} = \text{Molarity of HBr} \times \text{Volume of HBr} = 0.147 \text{ M} \times 0.025 \text{ L} = 0.003675 \text{ moles}
\]
- Using the stoichiometry, calculate the moles of barium hydroxide required:
\[
\text{Moles of Ba(OH)}_2 = \frac{\text{Moles of HBr}}{2} = \frac{0.003675}{2} = 0.0018375 \text{ moles}
\]
- Finally, determine the volume of barium hydroxide solution needed:
\[
\text
Expert Solution
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
This is a popular solution!
Trending now
This is a popular solution!
Step by step
Solved in 3 steps with 3 images
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