What is the pH of a buffer prepared by adding 0.506 mol of the weak acid HA to 0.305 mol of NaA in 2.00 L ofsolution? The dissociation constant Ka of HA is 5.66 × 10-7.Express the pH numerically to three decimal places.• View Available Hint(s)pH := 6.027SubmitPrevious AnswersCorrectImportant: If you use this answer in later parts, use the full unrounded value in your calculations.Since both the acid and base exist in the same volume, we can skip the concentration calculations and usethe number of moles in the Henderson-Hasselbalch equation to calculate the pH. The answer will be thesame.Part BWhat is the pH after 0.150 mol of HCl is added to the buffer from Part A? Assume no volume change on theaddition of the acid.Express the pH numerically to three decimal places.• View Available Hint(s)?pH =

When acid is added the concentration of HA increases and concentration of salt decreases.

What is the pH after 0.150 mol of HCl is added to the buffer from Part A? Assume no volume change on the addition of the acid. Express the pH numerically to three decimal places. • View Available Hint(s) ? pH =

What is the pH after 0.150 mol of HCl is added to the buffer from Part A? Assume no volume change on the addition of the acid. Express the pH numerically to three decimal places. • View Available Hint(s) ? pH =

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter14: Acid- Base Equilibria

Section: Chapter Questions

Problem 118CP: Malonic acid (HO2CCH2CO2H) is a diprotic acid. In the titration of malonic acid w ith NaOH,...

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What is the pH of a buffer prepared by adding 0.506 mol of the weak acid HA to 0.305 mol of NaA in 2.00 L of
solution? The dissociation constant Ka of HA is 5.66 × 10-7.
Express the pH numerically to three decimal places.
• View Available Hint(s)
pH :
= 6.027
Submit
Previous Answers
Correct
Important: If you use this answer in later parts, use the full unrounded value in your calculations.
Since both the acid and base exist in the same volume, we can skip the concentration calculations and use
the number of moles in the Henderson-Hasselbalch equation to calculate the pH. The answer will be the
same.
Part B
What is the pH after 0.150 mol of HCl is added to the buffer from Part A? Assume no volume change on the
addition of the acid.
Express the pH numerically to three decimal places.
• View Available Hint(s)
?
pH =

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