1. Calculate the molarity of Ag+ in an aqueous solution of AgaPO4 at a pH of 6.00 if the equilibria are the following: (hint, try using mass balance approach) Ag3PO4(s) 3 Ag* + PO, PO, + H20 = HPO,²- + OH HPO,2- + H2O =H2PO4¯+OH 3- Ksp = 2.8 x 10-18 %3D Kp1 = 2.3 x 10-2 %3D Kb2 = 1.6 x 10-7 %3D H2PO4 + H20=H3PO4 + OH° Kb3 = 1.4 x 10-12 %3D

1. Calculate the molarity of Ag+ in an aqueous solution of AgaPO4 at a pH of 6.00 if the equilibria are the following: (hint, try using mass balance approach) Ag3PO4(s) 3 Ag* + PO, PO, + H20 = HPO,²- + OH HPO,2- + H2O =H2PO4¯+OH 3- Ksp = 2.8 x 10-18 %3D Kp1 = 2.3 x 10-2 %3D Kb2 = 1.6 x 10-7 %3D H2PO4 + H20=H3PO4 + OH° Kb3 = 1.4 x 10-12 %3D

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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Precipitation Titration

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Question

1. Calculate the molarity of Ag+ in an aqueous solution of AgaPO4 at a pH of 6.00 if the
equilibria are the following: (hint, try using mass balance approach)
Ag3PO4(s) 3 Ag+ +PO,-
PO, +H20 HPO,2- +OH
HPO,2- + H20 H2PO4 + OH¯
Ksp = 2.8 x 10-18
Kp1 = 2.3 x 10-2
Kb2 = 1.6 x 10-7
%3D
H2PO4 + H20 H3PO4 + OH
Kp3 = 1.4 x 10-12
%3D

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