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Review 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 = You have already submitted this answer. Enter a new answer. No credit lost. Try again. Submit Previous Answers Request Answer Part C 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) pH =

Review 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 = You have already submitted this answer. Enter a new answer. No credit lost. Try again. Submit Previous Answers Request Answer Part C 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) pH =

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...
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I need help for number 5 part b and c
I Review | Constants | Periodic Table When a solution contains a weak acid and its conjugate base or a weak base and its conjugate acid, it will be a buffer solution. Buffers resist change in pH following the addition of acid or base. A butfer solution prepared from a weak acid (HA) and its. conjugate base (A) is represented as Part A What is the pH of a buffer prepared by adding 0.809 mol of the weak acid HA to 0.305 mol of NaA in 2.00L of solution? The dissociation constant K. of HA is 5.66 x 107 HA(aq) - H*(aq) + A (aq) The buffer will follow Le Châtelier's principle. If acid is added, the reaction shifts to consume the added H, forming more HA. When base is added, the base will react with H, reducing its concentration. The reaction then shifts to replace Ht through the dissociation of HA into H and A":In both instances, H Express the pH numerically to three decimal places. > View Available Hint(s) pH = 5.823 tends to remain constant. Submit The pH of a buffer is calculated by using the Henderson- Hasselbalch equation: Previous Answers A] v Correct pH = pK, + log HA 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)
Transcribed Image Text:I Review | Constants | Periodic Table When a solution contains a weak acid and its conjugate base or a weak base and its conjugate acid, it will be a buffer solution. Buffers resist change in pH following the addition of acid or base. A butfer solution prepared from a weak acid (HA) and its. conjugate base (A) is represented as Part A What is the pH of a buffer prepared by adding 0.809 mol of the weak acid HA to 0.305 mol of NaA in 2.00L of solution? The dissociation constant K. of HA is 5.66 x 107 HA(aq) - H*(aq) + A (aq) The buffer will follow Le Châtelier's principle. If acid is added, the reaction shifts to consume the added H, forming more HA. When base is added, the base will react with H, reducing its concentration. The reaction then shifts to replace Ht through the dissociation of HA into H and A":In both instances, H Express the pH numerically to three decimal places. > View Available Hint(s) pH = 5.823 tends to remain constant. Submit The pH of a buffer is calculated by using the Henderson- Hasselbalch equation: Previous Answers A] v Correct pH = pK, + log HA 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)
I Review Constant 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) ΑΣΦ pH = You have already submitted this answer. Enter a new answer. No credit lost. Try again. Submit Previous Answers Request Answer Part C 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) VO AEO ? pH = 國
Transcribed Image Text:I Review Constant 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) ΑΣΦ pH = You have already submitted this answer. Enter a new answer. No credit lost. Try again. Submit Previous Answers Request Answer Part C 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) VO AEO ? pH = 國
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