If the pH of a 0.0850 M solution of HB1O2 is 2.29, then what is the value for the acidity constant, Ka, of HBrO2? HB1O2(aq) + H20(I) H3O*(aq) + Br0, (aq) K¸ = ?
If the pH of a 0.0850 M solution of HB1O2 is 2.29, then what is the value for the acidity constant, Ka, of HBrO2? HB1O2(aq) + H20(I) H3O*(aq) + Br0, (aq) K¸ = ?
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
![**Problem Statement:**
If the pH of a 0.0850 M solution of HBrO₂ is 2.29, then what is the value for the acidity constant, Kₐ, of HBrO₂?
**Chemical Equation:**
\[ \text{HBrO}_2(\text{aq}) + \text{H}_2\text{O}(\text{l}) \rightleftharpoons \text{H}_3\text{O}^+(\text{aq}) + \text{BrO}_2^−(\text{aq}) \]
\[ K_a = ? \]
**Calculation Pathway:**
To find the \( K_a \), use the equation for the equilibrium constant for acids:
\[ K_a = \frac{[\text{H}_3\text{O}^+][\text{BrO}_2^-]}{[\text{HBrO}_2]} \]
**Provided Values:**
- Initial concentration of HBrO₂: 0.0850 M
- pH: 2.29
**Steps for Calculation:**
1. **Calculate the Hydronium Ion Concentration (\([\text{H}_3\text{O}^+]\)):**
From the pH value:
\[ [\text{H}_3\text{O}^+] = 10^{-\text{pH}} = 10^{-2.29} \]
2. **Determine Changes in Concentrations:**
- Initial concentration of HBrO₂: 0.0850 M
- Change in concentration of HBrO₂ and formation of \(\text{H}_3\text{O}^+\) = \(x\)
3. **Expression for Kₐ:**
Substitute the concentrations into the equilibrium expression to solve for \( K_a \).
4. **Conclusion and Analysis:**
Complete the calculation and then answer the following:
*Given the information above, is the bromite ion, \(\text{BrO}_2^-\), a strong base, a weak base, or not basic in water?*
Use the result of the \( K_a \) value to determine the basicity of \(\text{BrO}_2^-\).](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F092bd7db-9bdb-4d81-a056-eb65c4616336%2F684b6020-db09-4a66-b1a8-46d1d4ed3bb7%2Fhl5jzd_processed.png&w=3840&q=75)
Transcribed Image Text:**Problem Statement:**
If the pH of a 0.0850 M solution of HBrO₂ is 2.29, then what is the value for the acidity constant, Kₐ, of HBrO₂?
**Chemical Equation:**
\[ \text{HBrO}_2(\text{aq}) + \text{H}_2\text{O}(\text{l}) \rightleftharpoons \text{H}_3\text{O}^+(\text{aq}) + \text{BrO}_2^−(\text{aq}) \]
\[ K_a = ? \]
**Calculation Pathway:**
To find the \( K_a \), use the equation for the equilibrium constant for acids:
\[ K_a = \frac{[\text{H}_3\text{O}^+][\text{BrO}_2^-]}{[\text{HBrO}_2]} \]
**Provided Values:**
- Initial concentration of HBrO₂: 0.0850 M
- pH: 2.29
**Steps for Calculation:**
1. **Calculate the Hydronium Ion Concentration (\([\text{H}_3\text{O}^+]\)):**
From the pH value:
\[ [\text{H}_3\text{O}^+] = 10^{-\text{pH}} = 10^{-2.29} \]
2. **Determine Changes in Concentrations:**
- Initial concentration of HBrO₂: 0.0850 M
- Change in concentration of HBrO₂ and formation of \(\text{H}_3\text{O}^+\) = \(x\)
3. **Expression for Kₐ:**
Substitute the concentrations into the equilibrium expression to solve for \( K_a \).
4. **Conclusion and Analysis:**
Complete the calculation and then answer the following:
*Given the information above, is the bromite ion, \(\text{BrO}_2^-\), a strong base, a weak base, or not basic in water?*
Use the result of the \( K_a \) value to determine the basicity of \(\text{BrO}_2^-\).
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
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