: How would you prepare a liter of "carbonate buffer" at a pH of 10.10?H2CO3 > H* + HCO3Ka = 4.2 x 10HCO3 +> H* + co3 2Ka = 4.8 x 10-1113 buffer is preferred to prepare at mole ratio of 0.40 to 1.0, dissolve in enough water to make up a1-L solution2nobuffer is preferred to prepare at mole ratio of 0.60 to 1.0, dissolve in enough water to make up a1-L solution13 buffer preferred to prepare at mole ratio of 0.60 to 1.0, dissolve in enough water to make up a 1-L solution2nd buffer is preferred to prepare at mole ratio of 0.40 to 1.0, dissolve in enough water to make upa 1-L solution

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: How would you prepare a liter of "carbonate buffer" at a pH of 10.10? H2CO3 > H* + HCO3 Ka = 4.2 x 10-7 HCO3 > H* + co3 2 Ka = 4.8 x 10-11

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter14: Equilibria In Acid-base Solutions

Section: Chapter Questions

Problem 75QAP: A diprotic acid, H2B(MM=126g/moL), is determined to be a hydrate, H2B xH2O. A 10.00-g sample of this...

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Question

: How would you prepare a liter of "carbonate buffer" at a pH of 10.10?
H2CO3 > H* + HCO3
Ka = 4.2 x 10
HCO3 +> H* + co3 2
Ka = 4.8 x 10-11
13 buffer is preferred to prepare at mole ratio of 0.40 to 1.0, dissolve in enough water to make up a
1-L solution
2nobuffer is preferred to prepare at mole ratio of 0.60 to 1.0, dissolve in enough water to make up a
1-L solution
13 buffer preferred to prepare at mole ratio of 0.60 to 1.0, dissolve in enough water to make up a 1-
L solution
2nd buffer is preferred to prepare at mole ratio of 0.40 to 1.0, dissolve in enough water to make up
a 1-L solution

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