1.00 L of an aqueous solution containing 0.1026M of compound B and 0.0296M of its conjugate acid HB* was prepared to form a buffer solution with apH of 8.61 (pKą 8.072). Upon addition of a 12.0mL of 1.00M HCI to the solution, the pH changed from 8.61 to 8.41. Had there been no buffer, theaddition of the same amount and concentration of HCl would have lowered the pH to 1.93. Select ALL statements from the choices that are true. (Makesure to check all applicable answers to get a full points.)The added HC will be consumed by B and result to the formation of BH+. This will then cause the slight decrease in pH as predicted by the Henderson-Hasselbalchequation.Based on the Henderson-Hasselbalch equation, the HCl will increase the H+ concentration, thereby increasing the pH by itself because pH = - log [H+].The added HCI will not factor in the calculations for the pH, as the Henderson-Hasselbalch equation only accounts for the concentrations of B and BH+.Check this only if NONE of the other statements are true.

For buffer solution change in pH can be predicted by Henderson–Hasselbalch equation. pH = pKa +…

1.00 L of an aqueous solution containing 0.1026M of compound B and 0.0296M of its conjugate acid HB* was prepared to form a buffer solution with a pH of 8.61 (pK3 8.072). Upon addition of a 12.0mL of 1.00M HCI to the solution, the pH changed from 8.61 to 8.41. Had there been no buffer, the addition of the same amount and concentration of HCI would have lowered the pH to 1.93. Select ALL statements from the choices that are true. (Make sure to check all applicable answers to get a full points.) O The added HCI will be consumed by B and result to the formation of BH+. This will then cause the slight decrease in pH as predicted by the Henderson-Hasselbalch equation. O Based on the Henderson-Hasselbalch equation, the HCl will increase the H+ concentration, thereby increasing the pH by itself because pH = - log [H+]. O The added HCI will not factor in the calculations for the pH, as the Henderson-Hasselbalch equation only accounts for the concentrations of B and BH+. O Check this only if NONE of the other statements are true.

1.00 L of an aqueous solution containing 0.1026M of compound B and 0.0296M of its conjugate acid HB* was prepared to form a buffer solution with a pH of 8.61 (pK3 8.072). Upon addition of a 12.0mL of 1.00M HCI to the solution, the pH changed from 8.61 to 8.41. Had there been no buffer, the addition of the same amount and concentration of HCI would have lowered the pH to 1.93. Select ALL statements from the choices that are true. (Make sure to check all applicable answers to get a full points.) O The added HCI will be consumed by B and result to the formation of BH+. This will then cause the slight decrease in pH as predicted by the Henderson-Hasselbalch equation. O Based on the Henderson-Hasselbalch equation, the HCl will increase the H+ concentration, thereby increasing the pH by itself because pH = - log [H+]. O The added HCI will not factor in the calculations for the pH, as the Henderson-Hasselbalch equation only accounts for the concentrations of B and BH+. O Check this only if NONE of the other statements are true.

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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