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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

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
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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.
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