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A 0.7498-g sample of a chlorocarbon compound was analyzed by burning it in oxygen and collecting…
A 0.7498-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 48.85 mL of a 0.2298 M AgNO3 solution. This precipitated the chloride (Cl–) out as AgCl and left an excess of AgNO3. The excess AgNO3 was titrated with 0.1165 M KSCN and required 20.82 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