: 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

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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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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