Precipitimetry The chloride in a 4.321-g food sample was precipitated through the addition of 50.00 mL of a standard AgNO3 solution (10.00 mL AgNO3 = 11.22 mL KSCN). The precipitate was coated with nitrobenzene and the mixture was diluted to 250.0 mL. A 50.00 mL aliquot was taken from the diluted solution and required 4.56 mL back titration with a standard KSCN solution (22.33 mL KSCN = 0.9758 g AgNO3). Formula Masses: AgNO3 = 169.87; Cl = 35.45 Calculate the following: 1. Molar concentration of KSCN solution = 2. Molar concentration of AgNO3 solution = 3. % (w/w) chloride in the original sample = M M %

Precipitimetry The chloride in a 4.321-g food sample was precipitated through the addition of 50.00 mL of a standard AgNO3 solution (10.00 mL AgNO3 = 11.22 mL KSCN). The precipitate was coated with nitrobenzene and the mixture was diluted to 250.0 mL. A 50.00 mL aliquot was taken from the diluted solution and required 4.56 mL back titration with a standard KSCN solution (22.33 mL KSCN = 0.9758 g AgNO3). Formula Masses: AgNO3 = 169.87; Cl = 35.45 Calculate the following: 1. Molar concentration of KSCN solution = 2. Molar concentration of AgNO3 solution = 3. % (w/w) chloride in the original sample = M M %

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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