What is the pH of a buffer prepared by adding 0.809 mol of the weak acid HA to 0.507 mol of NaA in 2.00 L of solution? The dissociation constant K₁ of HA is 5.66 x 10-7. Express the pH numerically to three decimal places. View Available Hint(s) pH 6.044 Submit Previous Answers Correct 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.

What is the pH of a buffer prepared by adding 0.809 mol of the weak acid HA to 0.507 mol of NaA in 2.00 L of solution? The dissociation constant K₁ of HA is 5.66 x 10-7. Express the pH numerically to three decimal places. View Available Hint(s) pH 6.044 Submit Previous Answers Correct 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.

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...

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Concept explainers

Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.

Question

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
Submit
Part C
pH =
ΑΣΦ
What is the pH after 0.195 mol of NaOH is added to the buffer from Part A? Assume no volume change on the addition of the base.
Express the pH numerically to three decimal places.
► View Available Hint(s)
Submit
?
VG ΑΣΦ
?

What is the pH of a buffer prepared by adding 0.809 mol of the weak acid HA to 0.507 mol of NaA in 2.00 L of solution? The dissociation constant K₂ of HA is
5.66 × 10-7.
Express the pH numerically to three decimal places.
► View Available Hint(s)
pH = 6.044
Submit
Previous Answers
Correct
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.

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Step 2: determine pH for part A (before adding any HCl or NaOH )

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Step 3: determine pH for part B (after adding HCl)

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Step 4: determine pH for part C (after addition of NaOH)

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