Answered: The amount of Cd2+ in an aqueous sample…

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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Question

The amount of Cd²⁺ in an aqueous sample was measured with a constant current coulometric technique. If a current of 53.6 mA required 178 s to reduce all of the Cd²⁺ to Cd what is the number of milligrams of Cd²⁺ in the solution?

Expert Solution

Step 1: Introduction to the Faraday's first law of electrolysis

From Faraday's First law of electrolysis, the amount of the substance deposited(W) at the given electrode is directly proportional to the quantity of charge(Q) passed through the electrolytic solution.

Mathematically it is given by W = ZQ

$W space equals Z space i t W space equals fraction numerator E q u i v a l e n t space w e i g h t space o f space C d over denominator F end fraction space i t W space equals fraction numerator left parenthesis fraction numerator A t o m i c space w e i g h t space o f space C d over denominator v a l e n c y end fraction right parenthesis over denominator F end fraction space i t$

where Z = electrochemical equivalent = (E/F)

E = equivalent weight of Cd

F = Faraday's constant = 96500 C

But Q = it where i = current in amperes and t =time in seconds

i = current in amperes = $space 53.6 space m A space equals 53.6 cross times 10 to the power of negative 3 end exponent space A$

t = time in seconds = 178 s

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