Answered: What mass of silver nitrate must be…

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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The traditional method of analysis for the amount of chloride ion present in a sample is to dissolve the sample in water and then slowly to add a solution of silver nitrate. Silver chloride is very insoluble in water, and by adding silver nitrate, it is possible effectively to remove all chloride ion from the sample.

Ag⁺(aq) + Cl^-(aq) → AgCl(s)

Suppose a 1.515 g sample is known to contain 27.5% chloride ion by mass. What mass of silver nitrate must be used to completely precipitate the chloride ion from the sample?

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