Homework Help is Here – Start Your Trial Now!
Science
Chemistry
Find the p H of a 0.439 M N a A solution. The salt completely dissociates intoNaus and Anus, N a is the cation of a strong base so it will not affect the p H of the solution. Anus is the anion of the weak acid H A. The Ka of HAis 19E-5. If the 5% rule is valid you may apply it.

Find the p H of a 0.439 M N a A solution. The salt completely dissociates intoNaus and Anus, N a is the cation of a strong base so it will not affect the p H of the solution. Anus is the anion of the weak acid H A. The Ka of HAis 19E-5. If the 5% rule is valid you may apply it.

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
**Determining the pH of a 0.439 M NaA Solution** To find the pH of a 0.439 M NaA solution, consider the following steps. The salt NaA fully dissociates into Na⁺ and A⁻ ions. Given that Na⁺ is the cation from a strong base, it does not influence the pH of the solution. The ion A⁻ is the conjugate base of a weak acid, HA. 1. **Dissociation Context:** - Na⁺ is neutral and doesn't affect pH. - A⁻ is from the weak acid HA. - The acid dissociation constant (Ka) for HA is 1.9E-5. 2. **Using the 5% Rule:** - If applicable, use the 5% rule to simplify calculations involving ion concentrations. By focusing on the properties of A⁻ and its relation to the weak acid HA, a deeper understanding of the solution's behavior and pH can be achieved.
Transcribed Image Text:**Determining the pH of a 0.439 M NaA Solution** To find the pH of a 0.439 M NaA solution, consider the following steps. The salt NaA fully dissociates into Na⁺ and A⁻ ions. Given that Na⁺ is the cation from a strong base, it does not influence the pH of the solution. The ion A⁻ is the conjugate base of a weak acid, HA. 1. **Dissociation Context:** - Na⁺ is neutral and doesn't affect pH. - A⁻ is from the weak acid HA. - The acid dissociation constant (Ka) for HA is 1.9E-5. 2. **Using the 5% Rule:** - If applicable, use the 5% rule to simplify calculations involving ion concentrations. By focusing on the properties of A⁻ and its relation to the weak acid HA, a deeper understanding of the solution's behavior and pH can be achieved.
Expert Solution
Step 1

Pka= -logka

Use formula of PH of salt which is mixture of strong base and weak acid.

PH=9.32

 

steps

Step by step

Solved in 2 steps with 1 images

SEE SOLUTIONCheck out a sample Q&A here
Blurred answer
Knowledge Booster
Redox 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.
Similar questions
  • SEE MORE QUESTIONS
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