A cyanide solution with a volume of 12.99 ml was treated with 30.00 mL. of Ni solution (containing excess Ni) to convert the cyanide into tetracyanonickelate(): 4 CN+ Ni?+ Ni(CN) The excess Ni+ was then titrated with 11.96 ml. of 0.01357 M ethylenediaminetetraacetic acid (EDTA): Nit + EDTA Ni(EDTA)- Ni(CN) does not react with EDTA. If 39.40 ml. of EDTA were required to react with 30.65 ml. of the original Nit solution, calculate the molarity of CN in the 12.99 mL cyanide sample. 0.12055 (CN|= Incorrect

A cyanide solution with a volume of 12.99 ml was treated with 30.00 mL. of Ni solution (containing excess Ni) to convert the cyanide into tetracyanonickelate(): 4 CN+ Ni?+ Ni(CN) The excess Ni+ was then titrated with 11.96 ml. of 0.01357 M ethylenediaminetetraacetic acid (EDTA): Nit + EDTA Ni(EDTA)- Ni(CN) does not react with EDTA. If 39.40 ml. of EDTA were required to react with 30.65 ml. of the original Nit solution, calculate the molarity of CN in the 12.99 mL cyanide sample. 0.12055 (CN|= Incorrect

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 1.000 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 Znt 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 NP 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
Determinethe concentration of an EDTA solution given that a 20.00 mLsample of 0.02491M Zn2+was titrated with37.84mL of EDTA
3. Calculate the pZn of solutions prepared by adding 15.0, 25.0, and 35.0 mL of 0.100M EDTA to 50.0 mL of 0.00500M Zn²+ in 0.100M NH3 and 0.175M NH4Cl buffered to a pH of 9.0.
The concentration of sulfate in a solution containing a mixture of sulfuric acid is to be determined. A 25.0 mL portion of the sample is treated with 10.00 mL of 0.0500 M BaCl₂. The resulting precipitate is filtered off and the supernatant solution containing the Ba²⁺ is then titrated with 0.0354 M EDTA which gives an end point at 7.45 mL. (a) Identify the type of EDTA titration method used. (b) Calculate the molar concentration of sulfate in the sample
Kk.468.
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.
0.4545 g CaCO3 was dissolved in HCl and the resulting solution was diluted to 0.25 L. Twenty-five mL aliquot of this solution required 35.2 mL of EDTA upon performing titrimetric analysis. Determine the molarity of EDTA
A 340.00 mL solution of 0.00175 M AB2 is added to a 140.00 mL solution of 0.00235 M CD4. What is pQsp for AD2?
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.
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?