**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

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

A mixture of sodium chloride (NaCl) and sucrose (C₁2H22011) of combined mass 10.2 g is dissolved in enough wat The osmotic pressure of the solution is 6.19 atm at 23.0 °C. Calculate the mass percent of NaCl in the mixture. Rour Note: Reference the Fundamental constants table for additional information.
The calcium content of a milk sample was to be determined by EDTA titration. A sample weighing 0.206 g was mixed with an aqueous buffer at pH 11.5. A few drops of EBT indicator were added and the solution required 24.25 mL of 1.538 x 10-2 M EDTA to reach the endpoint. Calculate the weight percent of calcium (FW =40) in the milk.
50 mL of a solution of 0.0200 M Zn2+ will be titrated with 0.0100 M EDTA in 0.0100 M NH3 at pH 6.0. Ethylenediaminetetraacetic acid (EDTA) can be considered as a tetraprotic acid (H4Y). The stepwise acid dissociation constants are: K1 = 1.02 x 10-2, K2= 2.14 x 10-3, K3 = 6.92 x 10-7 and K4 = 5.50 x 10-11. The alplia value of the un-deprotonated species in a solution buffered to a certain pH is given by the following equation: a0 = [H+]4/([H+]4 + K1[H+]3 + K1K2[H+]2 + K1 K2K3[H+] + K1 K2K3K4) Calculate the alpha value of the fully deprotonated species (Y4- ) in a solution buffered to a pH of 6.0.
A solution containing 60 mL of a 0.025 mol / L metal ion (Mn +) buffer buffered to pH 7.0 was titrated with a 0.05 mol / L EDTA solution. Data: Conditional formation constant (Kf)=10^15. Determine: i) The concentration of the free metal when ½ of the equivalence volume is added. ii) the concentration of free metal in the equivalence volume. iii) the concentration of free metal with an excess of 2 mL of EDTA? (Data - EDTA constants: K1=0.01; K2=2.19.10^-3; K3=6.92.10^-7; K4=5.75.10^-11)
Calculate the resulting pH of the buffer solution when 18 mL of 398 mM HCl is added to 1 L of a 50 mM MOPS buffer at pH = 7.2. The pKa for the MOPS compound is 7.2. Assume negligible volume change upon the addition of the acid.
Calculate PCa of the solution that results when 50.0 mL of 0.0050 M Ca2+ is titrated with 25.00 mL of 0.0100 M EDTA in a solution buffered to a conastant pH of 10.00.
A 50.00 mL aliquot of city drinking water was treated with a small amount of ammonia –- ammonium chloride buffer to bring the pH to 10. After the addition of EBT indicator the solution required 10.00 mL of 8.000 x 10-3 M EDTA for titration. Calculate the hardness in terms of parts per million calcium carbonate (100.0869 g/mol). O 80 160 ppm 320
50 mL of a sample known to contain Mg+2 was taken and titrated with 0.075 M EDTA standard solution by adding pH 10 buffer and EBT indicator. Since the EDTA consumption is 10.5 mL, which of the following is the amount of magnesium in the sample in ppm? (Mg:24 B/mol)
An unknown solution containing 25.00 mL of Ni2+ in dilute HCl is treated with a known excess of 25.00 mL of 0.05382 M EDTA solution. The solution turns yellow when a few drops of indicator are added. The excess unreacted EDTA back titrated with 0.02299 M Zn2+, which requires 17.00 mL to reach the red end point. What is the molarity of Ni2+ in the unknown solution?
A 1.00 mL aliquot of a solution containing Cu and Ni is treated with 25.00 ml. of a 0.03468 M EDTA solution. The solution is then back titrated with 0.02308 M Zn+ solution at a pH of 5. A volume of 20.28 ml. of the Zn solution was needed to reach the xylenol orange end point. A 2.000 mL aliquot of the Cu* and Ni* solution is fed through an ion- exchange column that retains Ni?*. The Cu?+ that passed through the column is treated with 25.00 mL of 0.03468 M EDTA. This solution required 23.18 mL of 0.02308 M Zn* for back titration. The Ni extracted from the column was treated witn 25.00 mL of 0.03468 M EDTA. How many milliliters of 0.02308 M Zn+ is required for the back titration of the Ni solution? volume: ml.
The water hardness of tap water has been determined to be 120 (= 120 mg CaCO3 per 1 L of water). After the tap water has run through the ion exchange column, titration of a 20.00 mL sample used only 0.70 mL of 0.0100 M EDTA, to reach the endpoint. Calculate the effectiveness of the ion exchange column: what is the % of the calcium, removed by the ion exchange column? Provide your answer in % and without decimal. ( Please type answer note write by hend)
A titration of 50.00 mL of 0.1100 M Fe3+ with 0.07750 M Sn2+ is carried out. The analytical reaction is 2Fe3+ + Sn2+ ⇋ 2Fe2+ + Sn4+ and Fe3+ + e− ⇋ Fe2+ E° = +0.732 V Sn4+ + 2e− ⇋ Sn2+ E° = +0.139 V What is the volume of Sn2+ is added at the equivalence point?