A buffer with pH = 8.96 must be created. 8.90 g of the acid component of the best buffer system will be used, and the volume of the solution will be 1 L. Choose which is the best buffer system, then compute the mass of the salt or base component of the chosen system. Choices: HClO (Ka = 2.9 x 10-8 , 52.46 g/mol)& KClO (90.55 g/mol) NH3 (Ka = 5.65 x 10-10 , 17.031g/mol) &NH4Cl (53.491 gmol) CH3COOH (Ka = 1.77 x 10-5 , 60.052 g/mol) & CH3COOK (98.15 g/mol) HClO2 (Ka = 1.1 x 10-2 , 68.46 g/mol)) & KClO2 (106.55 g/mol)
A buffer with pH = 8.96 must be created. 8.90 g of the acid component of the best buffer system will be used, and the volume of the solution will be 1 L. Choose which is the best buffer system, then compute the mass of the salt or base component of the chosen system. Choices: HClO (Ka = 2.9 x 10-8 , 52.46 g/mol)& KClO (90.55 g/mol) NH3 (Ka = 5.65 x 10-10 , 17.031g/mol) &NH4Cl (53.491 gmol) CH3COOH (Ka = 1.77 x 10-5 , 60.052 g/mol) & CH3COOK (98.15 g/mol) HClO2 (Ka = 1.1 x 10-2 , 68.46 g/mol)) & KClO2 (106.55 g/mol)
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 29QAP: A buffer is made up of 0.300 L each of 0.500 M KH2PO4 and 0.317 M K2HPO4. Assuming that volumes are...
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A buffer with pH = 8.96 must be created. 8.90 g of the acid component of the best buffer system will be used, and the volume of the solution will be 1 L.
Choose which is the best buffer system, then compute the mass of the salt or base component of the chosen system.
Choices:
- HClO (Ka = 2.9 x 10-8 , 52.46 g/mol)& KClO (90.55 g/mol)
- NH3 (Ka = 5.65 x 10-10 , 17.031g/mol) &NH4Cl (53.491 gmol)
- CH3COOH (Ka = 1.77 x 10-5 , 60.052 g/mol) & CH3COOK (98.15 g/mol)
- HClO2 (Ka = 1.1 x 10-2 , 68.46 g/mol)) & KClO2 (106.55 g/mol)
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