A 0.10 µM aqueous solution of a metal ion, M2+, is extracted into an organic solvent by 0.43 mM of the ligand L¯. Given that KL = 1.2 x 104, KM = 6.0 × 10*, Ka = 3.0 x 10-5, Bn = 5.0 x 1022, and n = 2, calculate the distribution ratio, D, for the extraction at pH 1.50 and at pH 4.00. DpH=1.50 = DpH=4.00 =

A 0.10 µM aqueous solution of a metal ion, M2+, is extracted into an organic solvent by 0.43 mM of the ligand L¯. Given that KL = 1.2 x 104, KM = 6.0 × 10*, Ka = 3.0 x 10-5, Bn = 5.0 x 1022, and n = 2, calculate the distribution ratio, D, for the extraction at pH 1.50 and at pH 4.00. DpH=1.50 = DpH=4.00 =

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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Question

A 0.10 µM aqueous solution of a metal ion, M²+, is extracted into an organic solvent by 0.43 mM of the ligand L¯. Given that
KĻ = 1.2 × 10ª, KM = 6.0 × 10*, Ka = 3.0 × 10-5, B, = 5.0 × 1022, and n = 2, calculate the distribution ratio, D, for the
extraction at pH 1.50 and at pH 4.00.
DpH=1.50 =
DpH=4.00 =

Calculate the fraction of M2+ that remains in the aqueous phase, q, if 145 mL of 0.10 µM M²+ is extracted once with 10.0 mL
of 0.43 mM L¯ at pH 1.50.
9pH=1.50 =

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