0.753-g sample of a chlorocarbon compound was analyzed by burning it in oxygen and collecting the evolved gases in a solution of NaOH. After neutralizing, the sample was treated with 25.74 mL of a 0.264 M AgNO3 solution. This precipitated the chloride (Cl-) out as AgCl and left an excess of AgNO3. The excess AgNO3 was titrated with 0.1 M KSCN and required 16.47 mL to reach the endpoint in a Volhard titration. Calculate the % w/w Cl– (35.45 g/mol) in the sample. Provide your answer to 2 places after the decimal point and without units. Reactions: Cl– + Ag+ → AgCl(s) Reaction 1 Ag+ + SCN– → AgSCN(s) Reaction 2 HINT: This is an example of a back-titration. Steps to success: First, calculate the TOTAL amount (in moles) of Ag+ added from the volume and molarity of the silver nitrate solution. Second, determine the EXCESS amount of Ag+ from the reaction with thiocyanate (Reaction 2 above). Third, calculate the DIFFERENCE (TOTAL - EXCESS). This DIFFERENCE represents the amount in moles of silver ion which reacted with the chloride ion (Reaction 1 above) in the unknown chlorocarbon compound. Finally, calculate the % w/w Cl– in the 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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0.753-g sample of a chlorocarbon compound was analyzed by burning it in oxygen and collecting the evolved gases in a solution of NaOH. After neutralizing, the sample was treated with 25.74 mL of a 0.264 M AgNO₃ solution. This precipitated the chloride (Cl^-) out as AgCl and left an excess of AgNO₃. The excess AgNO₃ was titrated with 0.1 M KSCN and required 16.47 mL to reach the endpoint in a Volhard titration.

Calculate the % w/w Cl^– (35.45 g/mol) in the sample. Provide your answer to 2 places after the decimal point and without units.

Reactions: Cl^– + Ag⁺ → AgCl(s) Reaction 1

Ag⁺ + SCN^– → AgSCN(s) Reaction 2

HINT: This is an example of a back-titration. Steps to success:

First, calculate the TOTAL amount (in moles) of Ag⁺ added from the volume and molarity of the silver nitrate solution.
Second, determine the EXCESS amount of Ag⁺ from the reaction with thiocyanate (Reaction 2 above).
Third, calculate the DIFFERENCE (TOTAL - EXCESS). This DIFFERENCE represents the amount in moles of silver ion which reacted with the chloride ion (Reaction 1 above) in the unknown chlorocarbon compound.
Finally, calculate the % w/w Cl^–in the sample.

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