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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 Ayailable Hint/s)

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 Ayailable Hint/s)

Chemistry
Chemistry
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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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I need help w all parts of number 5
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 = Submit Previous Answers X Incorrect; Try Again; 5 attempts remaining 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 adition of the base. Express the pH numerically to three decimal places. > View Available Hint(s) pH = P Pearson
Transcribed Image Text: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 = Submit Previous Answers X Incorrect; Try Again; 5 attempts remaining 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 adition of the base. Express the pH numerically to three decimal places. > View Available Hint(s) pH = P Pearson
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 buffer 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 2.00 L of solution? The dissociation constant K of HA is 5.66 x 10-7 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 H† through the dissociation of HA into H+ and A¯. In both instances, H tends to remain constant. Express the pH numerically to three decimal places. • View Available Hint(s) The pH of a buffer is calculated by using the Henderson-Hasselbalch equation: pH = [A] pH = pKa + logHA] Submit Previous Answers 國
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 buffer 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 2.00 L of solution? The dissociation constant K of HA is 5.66 x 10-7 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 H† through the dissociation of HA into H+ and A¯. In both instances, H tends to remain constant. Express the pH numerically to three decimal places. • View Available Hint(s) The pH of a buffer is calculated by using the Henderson-Hasselbalch equation: pH = [A] pH = pKa + logHA] Submit Previous Answers 國
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