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Ammonia, NH3, is a base and will readily accept a proton in accordance with the following reaction: NH3(aq) + H2O <-> NH4+ + OH- ∆G0NH3(ag) = -26.6 kJ/mol ∆G0H2O = -237.1 kJ/mol ∆G0NH4+ = -79.3 kJ/mol ∆G0OH- = -157.2 kJ/mol For NH3 dissolving in water and forming NH4- and OH-, at pH 9.0, [NH3] = 10-5 mol/L, [NH4-] = 10-5 mol/L. Is the reaction at equilibrium? If not, in which direction is the reaction going?

Ammonia, NH3, is a base and will readily accept a proton in accordance with the following reaction: NH3(aq) + H2O <-> NH4+ + OH- ∆G0NH3(ag) = -26.6 kJ/mol ∆G0H2O = -237.1 kJ/mol ∆G0NH4+ = -79.3 kJ/mol ∆G0OH- = -157.2 kJ/mol For NH3 dissolving in water and forming NH4- and OH-, at pH 9.0, [NH3] = 10-5 mol/L, [NH4-] = 10-5 mol/L. Is the reaction at equilibrium? If not, in which direction is the reaction going?

Chemistry
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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Ammonia, NH3, is a base and will readily accept a proton in accordance with the following reaction:

NH3(aq) + H2O <-> NH4+ + OH-

∆G0NH3(ag) = -26.6 kJ/mol

∆G0H2O = -237.1 kJ/mol

∆G0NH4+ = -79.3 kJ/mol

∆G0OH- = -157.2 kJ/mol

For NH3 dissolving in water and forming NH4- and OH-, at pH 9.0, [NH3] = 10-5 mol/L, [NH4-] = 10-5 mol/L. Is the reaction at equilibrium? If not, in which direction is the reaction going?

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