A buffer solution is made that is 0.310 M in H₂CO3 and 0.310 M in KHCO3. If Kal for H₂CO3 is 4.20 × 10-7, what is the pH of the buffer solution? pH = Write the net ionic equation for the reaction that occurs when 0.083 mol HBr is added to 1.00 L of the buffer solution. (Use the lowest possible coefficients. Omit states of matter. Use H3O+ instead of H+) + +
A buffer solution is made that is 0.310 M in H₂CO3 and 0.310 M in KHCO3. If Kal for H₂CO3 is 4.20 × 10-7, what is the pH of the buffer solution? pH = Write the net ionic equation for the reaction that occurs when 0.083 mol HBr is added to 1.00 L of the buffer solution. (Use the lowest possible coefficients. Omit states of matter. Use H3O+ instead of H+) + +
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
Concept explainers
Ionic Equilibrium
Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.
Arrhenius Acid
Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.
Bronsted Lowry Base In Inorganic Chemistry
Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.
Question
Please help
![### Buffer Solution and pH Calculation
A buffer solution is prepared with the following concentrations:
* \(0.310 \, \text{M}\) in \( \text{H}_2\text{CO}_3 \)
* \(0.310 \, \text{M}\) in \( \text{KHCO}_3 \)
Given:
* The ionization constant \(K_{\text{a1}}\) for \( \text{H}_2\text{CO}_3 \) is \( 4.20 \times 10^{-7} \).
**Question:** What is the pH of the buffer solution?
**Calculation of pH:**
To calculate the pH of the buffer solution, use the Henderson-Hasselbalch equation:
\[ \text{pH} = \text{pK}_\text{a} + \log\left(\frac{[\text{A}^-]}{[\text{HA}]}\right) \]
Where:
* \([\text{A}^-]\) is the concentration of the conjugate base (\(\text{HCO}_3^-\)).
* \([\text{HA}]\) is the concentration of the weak acid (\(\text{H}_2\text{CO}_3\)).
* \(\text{pK}_\text{a} = -\log(K_{\text{a}})\).
Given that both concentrations are equal:
\[ \text{pH} = \text{pK}_\text{a} = -\log(4.20 \times 10^{-7}) \]
**Net Ionic Equation:**
Write the net ionic equation for the reaction that occurs when \(0.083 \, \text{mol} \, \text{HBr}\) is added to \(1.00 \, \text{L}\) of the buffer solution.
\[ \text{H}_3\text{O}^+ + \text{HCO}_3^- \rightarrow \text{H}_2\text{CO}_3 + \text{H}_2\text{O} \]
(Use the lowest possible coefficients. Omit states of matter. Use \( \text{H}_3\text{O}^+ \) instead of \( \text{H}^+ \))](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F5baa0102-60f7-4f8d-865b-4da67ad08e15%2F0da74b98-b0a8-47a0-a7b2-16126ea84dd9%2Fmipt3tn_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Buffer Solution and pH Calculation
A buffer solution is prepared with the following concentrations:
* \(0.310 \, \text{M}\) in \( \text{H}_2\text{CO}_3 \)
* \(0.310 \, \text{M}\) in \( \text{KHCO}_3 \)
Given:
* The ionization constant \(K_{\text{a1}}\) for \( \text{H}_2\text{CO}_3 \) is \( 4.20 \times 10^{-7} \).
**Question:** What is the pH of the buffer solution?
**Calculation of pH:**
To calculate the pH of the buffer solution, use the Henderson-Hasselbalch equation:
\[ \text{pH} = \text{pK}_\text{a} + \log\left(\frac{[\text{A}^-]}{[\text{HA}]}\right) \]
Where:
* \([\text{A}^-]\) is the concentration of the conjugate base (\(\text{HCO}_3^-\)).
* \([\text{HA}]\) is the concentration of the weak acid (\(\text{H}_2\text{CO}_3\)).
* \(\text{pK}_\text{a} = -\log(K_{\text{a}})\).
Given that both concentrations are equal:
\[ \text{pH} = \text{pK}_\text{a} = -\log(4.20 \times 10^{-7}) \]
**Net Ionic Equation:**
Write the net ionic equation for the reaction that occurs when \(0.083 \, \text{mol} \, \text{HBr}\) is added to \(1.00 \, \text{L}\) of the buffer solution.
\[ \text{H}_3\text{O}^+ + \text{HCO}_3^- \rightarrow \text{H}_2\text{CO}_3 + \text{H}_2\text{O} \]
(Use the lowest possible coefficients. Omit states of matter. Use \( \text{H}_3\text{O}^+ \) instead of \( \text{H}^+ \))
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 2 steps with 1 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.Similar questions
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