Sulfate buffer? Your laboratory is out of materials to make phosphate buffer and you are considerifi, 971g sulfate to make a buffer instead. The pKapKa values for the two hydrogens in H2SO4H,SO4 are –10 -10 and 2. (a) Will this approach work for making a buffer effective near pHPH 7? (b) Around what PHPH might a sulfate-based buffer be useful?

Sulfate buffer? Your laboratory is out of materials to make phosphate buffer and you are considerifi, 971g sulfate to make a buffer instead. The pKapKa values for the two hydrogens in H2SO4H,SO4 are –10 -10 and 2. (a) Will this approach work for making a buffer effective near pHPH 7? (b) Around what PHPH might a sulfate-based buffer be useful?

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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Similar questions

Buffers will resist pH changes following the addition of acid or base within about +/-1 pH unit of the pka of a solution. True False
A buffer containing 0.1 M HCN presents a pH = 10. What would be the new pH if to 1 litre of this solution we add 2g of HCl? Ka = 4.8 × 10-10
What is the pH of a buffer system that is 0.25 M in NH3 and 0.26 M in NHẠC?? Кь NH3 %3D 1.8 х 10:5 NOTE: Even though this system involves the weak base NH3 and its conjugate acid NH4*, it is still possible to use the Henderson-Hasselbalch equation using pKą for the weak acid NH4* and the ratio of [conjugate base]/[conjugate acid]. You do not need to convert the equation and use a pКь value.
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What is the pH after 8.0 mL of 0.10 M HCl is added to 20.0 mL of 0.10 M NH3? (Kb=1.8 x 10-5)
What is the pH of a buffer that is 0.200M HC2H3O2 and 0.100M NaC2H3O2 (Ka =1.8 x 10-5).