A 25.00 mL sample containing an unknown amount of Al³+; + and Pb2+required 15.54 mL of 0.05734 M EDTA to reach the end point. A 50.00 mL sample of the unknown was then treated with F¯ to mask the Al³+. To the 50.00 mL sample, 25.00 mL of 0.05734 M EDTA was added. The excess EDTA was then titrated with 0.02256 M Mn² +. A total of 25.7 mL was required to reach the methylthymol blue end point. Determine pAl³+ and pPb2+ in the unknown sample. PA1³ +: pPb²+ =

A 25.00 mL sample containing an unknown amount of Al³+; + and Pb2+required 15.54 mL of 0.05734 M EDTA to reach the end point. A 50.00 mL sample of the unknown was then treated with F¯ to mask the Al³+. To the 50.00 mL sample, 25.00 mL of 0.05734 M EDTA was added. The excess EDTA was then titrated with 0.02256 M Mn² +. A total of 25.7 mL was required to reach the methylthymol blue end point. Determine pAl³+ and pPb2+ in the unknown sample. PA1³ +: pPb²+ =

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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A 50.00 ml aliquot of a solution containing Ca2+ and Mg2+ was buffered at pH 10 and titrated with 0.0418 M EDTA. The endpoint volume was 44.36 ml. A second aliquot of the same mixture was made strongly basic by the addition of NaOH – this causes the Mg2+ to precipitate as Mg(OH)2. The solution was then titrated with the 0.0418 M EDTA and the endpoint volume was found to be 30.02 ml. Calculate the molar concentration of Mg.
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