Answer provided: 0.08432M Ag^+1Please show your complete solution and write yourclearly and readable. Thank you.answer The silver ion in a 25.00-mL sample was converted to dicyanoargentate (l) ion by the addition of anexcess solution containing Ni(CN), ²:Ni(CN), + 2 Ag' → 2Ag(CN)2" Ni2The liberated nickel ion was titrated with 43.77-mL of 0.02408M EDTA.concentration of the silver solution.Molar Masses: Ni = 58.69 AgCalculate the molar- 107.9

Answered: Image /qna-images/answer/e2003cd7-ce7a-4429-b26f-7a4f724237d5.jpg

fön in a 25.00-mL sample was converted to dicyanoargentate (l) ion by the addition of a xcess solution containing Ni(CN), ²: Ni(CN), 2 Ag" → 2Ag(CN);" Ni2 The liberated nickel ion was titrated with 43.77-mL of 0.02408M EDTA. Calculate the mola oncentration of the silver solution. Molar Masses: Ni - 58.69 Ag 107.9

fön in a 25.00-mL sample was converted to dicyanoargentate (l) ion by the addition of a xcess solution containing Ni(CN), ²: Ni(CN), 2 Ag" → 2Ag(CN);" Ni2 The liberated nickel ion was titrated with 43.77-mL of 0.02408M EDTA. Calculate the mola oncentration of the silver solution. Molar Masses: Ni - 58.69 Ag 107.9

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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Concept explainers

Potentiometric Titrations

Potentiometric titration is one of the important titration methods and is mainly carried out to characterize acid solutions. It follows a method similar to that of the normal titration technique, but the main difference is that there is no indicator used in the potentiometric titrations. Instead of using an indicator, electrodes are employed for monitoring the whole titration process. A scientist named Robert Behrend did the potentiometric titration for the first time, and it was done using the mercurous solution and potassium chloride.

Question

Answer provided: 0.08432M Ag^+1
Please show your complete solution and write your
clearly and readable. Thank you.
answer

The silver ion in a 25.00-mL sample was converted to dicyanoargentate (l) ion by the addition of an
excess solution containing Ni(CN), ²:
Ni(CN), + 2 Ag' → 2Ag(CN)2" Ni2
The liberated nickel ion was titrated with 43.77-mL of 0.02408M EDTA.
concentration of the silver solution.
Molar Masses: Ni = 58.69 Ag
Calculate the molar
- 107.9

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