Homework Help is Here – Start Your Trial Now!
Science
Chemistry
A weak acid is added to a solution of strong acid (HCl) of unknown concentration. The concentration of the weak acid is 1.17 M. The Ka is 5.80 × 10-2. Given that the degree of ionization of the acid is 0.0166, what was concentration of the initial strong acid solution? (0.001) Correct Answer:3.417

A weak acid is added to a solution of strong acid (HCl) of unknown concentration. The concentration of the weak acid is 1.17 M. The Ka is 5.80 × 10-2. Given that the degree of ionization of the acid is 0.0166, what was concentration of the initial strong acid solution? (0.001) Correct Answer:3.417

Introduction to General, Organic and Biochemistry
Introduction to General, Organic and Biochemistry
11th Edition
ISBN:9781285869759
Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres
Publisher:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres
Chapter8: Acids And Bases
Section: Chapter Questions
Problem 8.98P: 8-98 When a solution prepared by dissolving 4.00 g of an unknown monoprotic acid in 1.00 L of water...
See similar textbooks
icon
Related questions
Question
A weak acid is added to a solution of strong acid (HCl) of unknown concentration. The concentration of the weak acid is 1.17 M. The Ka is 5.80 × 10-2. Given that the degree of ionization of the acid is 0.0166, what was concentration of the initial strong acid solution? (0.001) Correct Answer:3.417
3 A weak acid is added to a solution of strong acid (HCI) of unknown concentration. The concentration of the weak acid is 1.17 M. The K, is 5.80 x 10². Given that the degree of ionization of the acid is 0.0166, what was concentration of the initial strong acid solution? (0.001) X 0.034 Correct Answer: 3.417 Feedback Based on answering incorrectly Consider all the information given and carefully read what is being asked for. The variable being solved for isn't always the change. Here you are asked what was the initial HCI concentration. HCI is a strong acid so you should assume it fully dissociates. Consider what degree of ionization tells you about a system at equilibrium and how it is calculated. This can be used to complete more of the ICE table. Is the ionization an initial condition, does it represent change, is it calculated at equilibrium? Lastly, consider how this would look in front of you at the bench. You might envision a beaker of acid. For simplicity assume 1 L. You add a known quantity of moles to the beaker giving a solution of known molarity of weak acid. This would be an initial value since you understand and can record the moles added, but do not know the changes towards equilibrium until you measure the degree of ionization. Therefore the given molarity is an initial concentration of the weak acid.
Transcribed Image Text:3 A weak acid is added to a solution of strong acid (HCI) of unknown concentration. The concentration of the weak acid is 1.17 M. The K, is 5.80 x 10². Given that the degree of ionization of the acid is 0.0166, what was concentration of the initial strong acid solution? (0.001) X 0.034 Correct Answer: 3.417 Feedback Based on answering incorrectly Consider all the information given and carefully read what is being asked for. The variable being solved for isn't always the change. Here you are asked what was the initial HCI concentration. HCI is a strong acid so you should assume it fully dissociates. Consider what degree of ionization tells you about a system at equilibrium and how it is calculated. This can be used to complete more of the ICE table. Is the ionization an initial condition, does it represent change, is it calculated at equilibrium? Lastly, consider how this would look in front of you at the bench. You might envision a beaker of acid. For simplicity assume 1 L. You add a known quantity of moles to the beaker giving a solution of known molarity of weak acid. This would be an initial value since you understand and can record the moles added, but do not know the changes towards equilibrium until you measure the degree of ionization. Therefore the given molarity is an initial concentration of the weak acid.
Expert Solution
trending now

Trending now

This is a popular solution!

steps

Step by step

Solved in 3 steps with 3 images

SEE SOLUTIONCheck out a sample Q&A here
Blurred answer
Knowledge Booster
Acid-Base 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
Introduction to General, Organic and Biochemistry
Introduction to General, Organic and Biochemistry
Chemistry
ISBN:
9781285869759
Author:
Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres
Publisher:
Cengage Learning
General Chemistry - Standalone book (MindTap Cour…
General Chemistry - Standalone book (MindTap Cour…
Chemistry
ISBN:
9781305580343
Author:
Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:
Cengage Learning
Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
SEE MORE TEXTBOOKS