**Title: Determining the Volume Required for Back Titration of Nickel(II) Ions Using Zinc(II) Solution****Introduction:**In this experiment, a solution containing copper(II) ions (Cu²⁺) and nickel(II) ions (Ni²⁺) undergoes a series of titrations to determine the volume of zinc(II) sulfate (Zn²⁺) required for back titration of Ni²⁺.**Procedure Overview:**1. A 1.000 mL aliquot of a solution containing Cu²⁺ and Ni²⁺ is reacted with 25.00 mL of 0.03703 M EDTA.2. The resulting solution is back titrated with 0.02138 M Zn²⁺ solution at pH 5, requiring 22.13 mL to reach the xylidene orange end point.3. A separate 2.000 mL aliquot of the original Cu²⁺ and Ni²⁺ solution is passed through an ion-exchange column that retains Ni²⁺.4. The Cu²⁺ that passes through the column is again treated with 25.00 mL of 0.03703 M EDTA. This time, the solution requires 18.53 mL of 0.02138 M Zn²⁺ for back titration.5. The Ni²⁺ retained by the column is then treated with 25.00 mL of 0.03703 M EDTA.**Question:**How many milliliters of 0.02138 M Zn²⁺ are needed for the back titration of the Ni²⁺ solution?**Answer Entry:**- Volume: ______ mL**Key Concepts:**- This titration involves the use of EDTA, which forms complexes with metal ions.- The back titration method is used to determine excess EDTA, indicating the amount of metal ions initially present.- Ion-exchange columns help in separating specific ions for individual analysis.This setup provides a comprehensive understanding of titration methods and ion exchange roles in analytical chemistry.

Given,Concentration of EDTA = 0.03703 M

A 1.000 mL aliquot of a solution containing Cu²+ and Ni²+ is treated with 25.00 mL of a 0.03703 M EDTA solution. The solution is then back titrated with 0.02138 M Zn²+ solution at a pH of 5. A volume of 22.13 mL of the Zn²+ solution was needed to reach the xylenol orange end point. A 2.000 mL aliquot of the Cu²+ and Ni²+ solution is fed through an ion-exchange column that retains Ni²+. The Cu²+ that passed through the column is treated with 25.00 mL of 0.03703 M EDTA. This solution required 18.53 mL of 0.02138 M Zn²+ for back titration. The Ni²+ extracted from the column was treated witn 25.00 mL of 0.03703 M EDTA. How many milliliters of 0.02138 M Zn²+ is required for the back titration of the Ni²+ solution? volume: mL

A 1.000 mL aliquot of a solution containing Cu²+ and Ni²+ is treated with 25.00 mL of a 0.03703 M EDTA solution. The solution is then back titrated with 0.02138 M Zn²+ solution at a pH of 5. A volume of 22.13 mL of the Zn²+ solution was needed to reach the xylenol orange end point. A 2.000 mL aliquot of the Cu²+ and Ni²+ solution is fed through an ion-exchange column that retains Ni²+. The Cu²+ that passed through the column is treated with 25.00 mL of 0.03703 M EDTA. This solution required 18.53 mL of 0.02138 M Zn²+ for back titration. The Ni²+ extracted from the column was treated witn 25.00 mL of 0.03703 M EDTA. How many milliliters of 0.02138 M Zn²+ is required for the back titration of the Ni²+ solution? volume: mL

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

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Question

**Title: Determining the Volume Required for Back Titration of Nickel(II) Ions Using Zinc(II) Solution**

**Introduction:**
In this experiment, a solution containing copper(II) ions (Cu²⁺) and nickel(II) ions (Ni²⁺) undergoes a series of titrations to determine the volume of zinc(II) sulfate (Zn²⁺) required for back titration of Ni²⁺.

**Procedure Overview:**
1. A 1.000 mL aliquot of a solution containing Cu²⁺ and Ni²⁺ is reacted with 25.00 mL of 0.03703 M EDTA.
2. The resulting solution is back titrated with 0.02138 M Zn²⁺ solution at pH 5, requiring 22.13 mL to reach the xylidene orange end point.
3. A separate 2.000 mL aliquot of the original Cu²⁺ and Ni²⁺ solution is passed through an ion-exchange column that retains Ni²⁺.
4. The Cu²⁺ that passes through the column is again treated with 25.00 mL of 0.03703 M EDTA. This time, the solution requires 18.53 mL of 0.02138 M Zn²⁺ for back titration.
5. The Ni²⁺ retained by the column is then treated with 25.00 mL of 0.03703 M EDTA.

**Question:**
How many milliliters of 0.02138 M Zn²⁺ are needed for the back titration of the Ni²⁺ solution?

**Answer Entry:**
- Volume: ______ mL

**Key Concepts:**
- This titration involves the use of EDTA, which forms complexes with metal ions.
- The back titration method is used to determine excess EDTA, indicating the amount of metal ions initially present.
- Ion-exchange columns help in separating specific ions for individual analysis.

This setup provides a comprehensive understanding of titration methods and ion exchange roles in analytical chemistry.

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