Testbank, Question 7 Two buffer solutions of the same pH are prepared. After adding 15 millimoles of acid to 250 mL of one solution, the pH changes by 0.02 pH unit. Adding 15 millimoles of acid to 250 mL of the second solution results in a 0.05 pH unit change. Which statement most accurately describes the differences between the two buffer solutions? O The second solution has a lower concentration of coniugate base that the firet colution

Testbank, Question 7 Two buffer solutions of the same pH are prepared. After adding 15 millimoles of acid to 250 mL of one solution, the pH changes by 0.02 pH unit. Adding 15 millimoles of acid to 250 mL of the second solution results in a 0.05 pH unit change. Which statement most accurately describes the differences between the two buffer solutions? O The second solution has a lower concentration of coniugate base that the firet colution

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...

See similar textbooks

Similar questions

How does a buffer resist change in pH upon addition of a strong base? Question 4 options: The strong base reacts with the weak base in the buffer to form a weak acid, which produces few H+ ions in solution and therefore only a little change in pH. The strong base reacts with the strong acid in the buffer to form a salt which produces few H+ ions in solution and therefore only a little change in pH. The strong base reacts with the weak acid in the buffer to form a weak base, which produces few H+ ions in solution and therefore only a little change in pH. For the acid/base titration of HNO3 and KOH, choose a suitable indicator from the list below. Beside each indicator, the pH range of colour change at its endpoint is provided. Question 5 options: methyl orange (3.1 - 4.4) bromothylmol blue (6.0 - 7.7) thymolphthalein (8.3 - 10.5)
define the buffer capacity. a) buffer capacity is the amount of acid that can be added until all of the acid is used up b) buffer capacity is the amount of base that can be added until all of the base is used up c) buffer capacity is the amount of acid that can be added until all of the base is used up d) buffer capacity is the amount of acid ir base that can be added to a buffer without destroying its effectiveness e) buffer capacity is the amount of base that can be added until all of the acid is used up
For 530.0 mL of a buffer solution that is 0.145 M in HC2H3O2 and 0.130 M in NaC2H3O2, calculate the initial pH and the final pH after adding 0.020 mol of HCl.
How does a buffer solution prevent larger change in pH? What does it mean when a solution has exceeded the buffer capacity?
A 50.0-ml sample of 0.20 M hydrochloric acid (HCI) is titrated with 0.5 M LIOH. Determine the pH of the solution after the following volumes of LIOH titrant are added. Express your answers to two decimal places. a) pH after 10 mL of LIOH added: b) pH after 20 mL of LIOH added: c) pH after 30 mL of LIOH added: Check
What is the pH of a buffer solution that is 0.508 M in hydrofluoric acid and is 0.604 M is potassium fluoride? The K₂ of hydrofluoric acid is 6.4 x 10-4. (Two decimal places) Type your answer...
Which of the following solutions, when mixed in equal volumes, will create a reasonably effective buffer solution? Select one or more: 0.100 M NaCl and 0.100 M HCl 0.100 M HCl and 0.200 M NO2- 0.100 M NaOH and 0.200 M CH3COOH 0.200 M NaOH and 0.100 M HCOOH 0.100 M HCOOH and 0.100 M HCOO- 0.100 M HCl and 0.100 M NaOH
80.0 mL of 0.30 M NaOH and 80.0 mL of 0.30 M HCl are mixed together what is the pH level
It was assumed: a) Before any acetic acid was added, essentially all the indicator was in the In- form. b) After the HCl was added, essentially all the indicator was in the HIn form. Justify these assumptions using the measured pH of these solutions and your experimental value for pKHIn to determine: 1) The fraction fo the indicator in the HIn form in solution B before any of solution A was added 2) The fraction of the indicator in the In- form after the HCl was added.
What is the pH of a buffer solution that is 0.33 M propionic acid and 0.55 M sodium propionate?
Please don't provide hand written solution.....