A 25.0 mL aliquot of 0.0570 M EDTA was added to a 59.0 mL solution containing an unknown concentration of V³+. All of the V³ + present in the solution formed a complex with EDTA, leaving an excess of EDTA in solution. This solution was back- titrated with a 0.0480 M Ga³ + solution until all of the EDTA reacted, requiring 14.0 mL of the Ga³ + solution. What was the original concentration of the V3+ solution? [V³+] = M The end point of the Zn²+-EDTA titration was observed after 15.50 mL of 0.0500 M EDTA solution was dispensed. Determine the number of moles of zinc ion present in the sample. number of moles of zinc ion = mol

A 25.0 mL aliquot of 0.0570 M EDTA was added to a 59.0 mL solution containing an unknown concentration of V³+. All of the V³ + present in the solution formed a complex with EDTA, leaving an excess of EDTA in solution. This solution was back- titrated with a 0.0480 M Ga³ + solution until all of the EDTA reacted, requiring 14.0 mL of the Ga³ + solution. What was the original concentration of the V3+ solution? [V³+] = M The end point of the Zn²+-EDTA titration was observed after 15.50 mL of 0.0500 M EDTA solution was dispensed. Determine the number of moles of zinc ion present in the sample. number of moles of zinc ion = mol

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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