A buffer was prepared by adding 7.50 moles K2HPO4 and 9.60 mol KH2PO4 to a 1.0 L solution. Ka2 = 6.2 x 108 а. Determine the pH for the buffer. b. Determine the chemical equation when HBr is added to this buffer. Spectator ions should be left out of the equation. C. Determine the pH of the buffer after 125.00 mL of 9.90 M HBr was added. Use an ICE box to show the initial, change and equilibrium quantity of moles for each substance.

A buffer was prepared by adding 7.50 moles K2HPO4 and 9.60 mol KH2PO4 to a 1.0 L solution. Ka2 = 6.2 x 108 а. Determine the pH for the buffer. b. Determine the chemical equation when HBr is added to this buffer. Spectator ions should be left out of the equation. C. Determine the pH of the buffer after 125.00 mL of 9.90 M HBr was added. Use an ICE box to show the initial, change and equilibrium quantity of moles for each substance.

Chemistry & Chemical Reactivity

10th Edition

ISBN:9781337399074

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter17: Principles Of Chemical Reactivity: Other Aspects Of Aqueous Equilibria

Section: Chapter Questions

Problem 108IL: A buffer solution with it pH of 12.00 consists of Na3PO4 and Na2HPO4. The volume of solution is...

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