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12.0 mL of a 437.1 mM AgNO3 solution is added to a 20.0 mL sample containing...

12.0 mL of a 437.1 mM AgNO3 solution is added to a 20.0 mL sample containing an unknown chloride ion concentration to precipitate Cl- as AgCl. The AgCl solid is removed and excess Ag+ is titrated with a standard 137.0 mM KSCN solution in the presence of Fe3+. After 2.5 mL of the standard solution have been added, all Ag+ has precipitated as AgSCN and the red complex FeSCN2+ forms. What is the chloride ion concentration in the sample to the nearest 0.1 mM?

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This question is solved by using simple concept of stoichiometry and calculation of molarity.

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