Homework Help is Here – Start Your Trial Now!
Science
Chemistry
Lab Report #2-2-4: 0.1 M Na2CO3 solution, using the given pH data, calculate value of (Ka or Kb) 1.0 x 10-5 O 1.0 x 10-6 1.0 x 10-4 O 1.0 x 10-3

Lab Report #2-2-4: 0.1 M Na2CO3 solution, using the given pH data, calculate value of (Ka or Kb) 1.0 x 10-5 O 1.0 x 10-6 1.0 x 10-4 O 1.0 x 10-3

Chemistry
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...
See similar textbooks
icon
Related questions
Question
### Lab Report #2-2-4: **Topic:** Calculating the Value of (Ka or Kb) for a 0.1 M Na₂CO₃ Solution Using Given pH Data ### Objective: Using the pH data provided for a 0.1 M sodium carbonate (Na₂CO₃) solution, determine the value of the acid dissociation constant (Ka) or base dissociation constant (Kb). ### Multiple Choice Options: - □ \(1.0 \times 10^{-5}\) - □ \(1.0 \times 10^{-6}\) - □ \(1.0 \times 10^{-4}\) - □ \(1.0 \times 10^{-3}\)
Transcribed Image Text:### Lab Report #2-2-4: **Topic:** Calculating the Value of (Ka or Kb) for a 0.1 M Na₂CO₃ Solution Using Given pH Data ### Objective: Using the pH data provided for a 0.1 M sodium carbonate (Na₂CO₃) solution, determine the value of the acid dissociation constant (Ka) or base dissociation constant (Kb). ### Multiple Choice Options: - □ \(1.0 \times 10^{-5}\) - □ \(1.0 \times 10^{-6}\) - □ \(1.0 \times 10^{-4}\) - □ \(1.0 \times 10^{-3}\)
### Solutions and Their pH Values The table below provides the pH values of various solutions. pH is a measure of how acidic or basic a solution is, with a scale ranging from 0 to 14. A pH value of 7 is considered neutral, values below 7 are acidic, and values above 7 are basic (alkaline). | **Solutions** | **pH values** | |---------------------|---------------| | H₂O (unboiled) | 3.5 | | H₂O (boiled) | 7.0 | | NaCl | 7.0 | | NaC₂H₃O₂ | 9.1 | | NH₄Cl | 4.5 | | NaHCO₃ | 9.5 | | Na₃PO₄ | 11.9 | | Na₂CO₃ | 11.0 | **Explanation of the pH Values of the Solutions:** 1. **H₂O (unboiled):** The unboiled water has a pH of 3.5, indicating it is slightly acidic. This could be due to the dissolved carbon dioxide forming carbonic acid. 2. **H₂O (boiled):** Boiled water has a neutral pH of 7.0. Boiling water removes dissolved gases such as CO₂, which can lower the pH of water. 3. **NaCl:** Sodium chloride solution has a pH of 7.0, showing it is completely neutral. NaCl is a neutral salt formed from a strong acid (HCl) and a strong base (NaOH). 4. **NaC₂H₃O₂:** Sodium acetate solution is slightly basic with a pH of 9.1. This is because sodium acetate is derived from a weak acid (acetic acid) and a strong base (sodium hydroxide). 5. **NH₄Cl:** Ammonium chloride solution has a pH of 4.5, making it acidic. This is due to the hydrolysis of NH₄⁺ ions producing H⁺ ions. 6. **NaHCO₃:** Sodium bicarbonate solution has a basic pH of 9.5. It forms a weakly basic solution as it partially dissociates to
Transcribed Image Text:### Solutions and Their pH Values The table below provides the pH values of various solutions. pH is a measure of how acidic or basic a solution is, with a scale ranging from 0 to 14. A pH value of 7 is considered neutral, values below 7 are acidic, and values above 7 are basic (alkaline). | **Solutions** | **pH values** | |---------------------|---------------| | H₂O (unboiled) | 3.5 | | H₂O (boiled) | 7.0 | | NaCl | 7.0 | | NaC₂H₃O₂ | 9.1 | | NH₄Cl | 4.5 | | NaHCO₃ | 9.5 | | Na₃PO₄ | 11.9 | | Na₂CO₃ | 11.0 | **Explanation of the pH Values of the Solutions:** 1. **H₂O (unboiled):** The unboiled water has a pH of 3.5, indicating it is slightly acidic. This could be due to the dissolved carbon dioxide forming carbonic acid. 2. **H₂O (boiled):** Boiled water has a neutral pH of 7.0. Boiling water removes dissolved gases such as CO₂, which can lower the pH of water. 3. **NaCl:** Sodium chloride solution has a pH of 7.0, showing it is completely neutral. NaCl is a neutral salt formed from a strong acid (HCl) and a strong base (NaOH). 4. **NaC₂H₃O₂:** Sodium acetate solution is slightly basic with a pH of 9.1. This is because sodium acetate is derived from a weak acid (acetic acid) and a strong base (sodium hydroxide). 5. **NH₄Cl:** Ammonium chloride solution has a pH of 4.5, making it acidic. This is due to the hydrolysis of NH₄⁺ ions producing H⁺ ions. 6. **NaHCO₃:** Sodium bicarbonate solution has a basic pH of 9.5. It forms a weakly basic solution as it partially dissociates to
Expert Solution
trending now

Trending now

This is a popular solution!

steps

Step by step

Solved in 3 steps with 2 images

SEE SOLUTIONCheck out a sample Q&A here
Blurred answer
Knowledge Booster
Complexometric Titrations
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
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
SEE MORE TEXTBOOKS