Calculate the pZn2+ for solutions prepared by adding 0.00, 5.00, 10.00, 15.00, 20.00, 25.00 and 30.00 mL of 0.0100 M EDTA to 25.00 mL of 0.00250 M Zn2+. Assume that both the Zn2+ and EDTA are 0.0100 M in NH3 to provide a constant pH of 9.0 Zn(NH3)n 2+: pKfn, = 2.21, 2.29, 2.36, 2.03 ZnY2- : Kf = 3.0 x 1016 EDTA: Ka1 = 1.02 x 10-2 , Ka2 = 2.14 x 10-3 , Ka3 = 6.92 x 10-7 , Ka4 = 5.50 x 10-11
Calculate the pZn2+ for solutions prepared by adding 0.00, 5.00, 10.00, 15.00, 20.00, 25.00 and 30.00 mL of 0.0100 M EDTA to 25.00 mL of 0.00250 M Zn2+. Assume that both the Zn2+ and EDTA are 0.0100 M in NH3 to provide a constant pH of 9.0 Zn(NH3)n 2+: pKfn, = 2.21, 2.29, 2.36, 2.03 ZnY2- : Kf = 3.0 x 1016 EDTA: Ka1 = 1.02 x 10-2 , Ka2 = 2.14 x 10-3 , Ka3 = 6.92 x 10-7 , Ka4 = 5.50 x 10-11
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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Calculate the pZn2+ for solutions prepared by adding 0.00, 5.00, 10.00, 15.00, 20.00, 25.00
and 30.00 mL of 0.0100 M EDTA to 25.00 mL of 0.00250 M Zn2+. Assume that both the Zn2+
and EDTA are 0.0100 M in NH3 to provide a constant pH of 9.0
Zn(NH3)n
2+: pKfn, = 2.21, 2.29, 2.36, 2.03
ZnY2-
: Kf = 3.0 x 1016
EDTA: Ka1 = 1.02 x 10-2
, Ka2 = 2.14 x 10-3
, Ka3 = 6.92 x 10-7
, Ka4 = 5.50 x 10-11
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