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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What is the mass of pure dry CaCO3 (MW: 100.0869 g/mol) standard used in the standardization of EDTA solution? Assume that 1.875 M EDTA solution was computed based on the titration of CaCO3 standard. The volume of titrant needed to reach the endpoint was 30.00 mL. Ca2+ + Y4- → CaY2- 5.630 g 0.6158 g 0.1500 g 6.158 g
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A 50.00-mL of 0.0500 M Sn²+ was titrated against 0.100 M T1³+ in acidic medium. d. Calculate the potential at the equivalence point. e. Calculate the potential when 30.00 mL of titrant is added.
The concentration of a solution of EDTA was determined by standardizing against a solution of Ca2+ prepared from the primary standard CaCO3. A 0.4071-g sample of CaCO3 was transferred to a 500-mL volumetric flask, dissolved using a minimum of 6 M HCl, and diluted to volume. A 50.00-mL portion of this solution was transferred into a 250-mL Erlenmeyer flask and the pH adjusted by adding 5 mL of a pH 10 NH3–NH4Cl buffer containing a small amount of Mg2+–EDTA. After adding calmagite as a visual indicator, the solution was titrated with the EDTA, requiring 42.63 mL to reach the end point. Report the molar concentration of the titrant.
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