(2)When ammonium sulfate dissolves, both the anion and cation have acid-base reaction:(NH4)2SO4(s)< 2NH4* + SO4²-NH4* + NH3(aq) + H*SO42- + H2O → HSO4 + OH-Ksp = 276Ka = 5.70 ×10-10Кь 3 9.80 х 10-13(a)(b)(c)(Show your Calculation)Write a charge balance for this system.Write a mass balance for this system.Find the concentration of NH3(aq) if the pH is fixed at 9.25.

Questions are 1. Charge balance 2. Mass balance 3. NH3 concentration calculation

When ammonium sulfate dissolves, both the anion and cation have acid-base reaction: (NH4)2SO4(s)→ 2NH4* + SO4²- NH4* + NH3(aq) + H* SO,2- + H2O → HSO4 + OH- Ksp = 276 Ka = 5.70 ×10-10 Kb = 9.80 × 10-13 (а) (b) (c) (Show your Calculation) Write a charge balance for this system. Write a mass balance for this system. Find the concentration of NH3(aq) if the pH is fixed at 9.25.

When ammonium sulfate dissolves, both the anion and cation have acid-base reaction: (NH4)2SO4(s)→ 2NH4* + SO4²- NH4* + NH3(aq) + H* SO,2- + H2O → HSO4 + OH- Ksp = 276 Ka = 5.70 ×10-10 Kb = 9.80 × 10-13 (а) (b) (c) (Show your Calculation) Write a charge balance for this system. Write a mass balance for this system. Find the concentration of NH3(aq) if the pH is fixed at 9.25.

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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