Students performed a procedure similar to Part III of this experiment (Analyzing

Question

Students performed a procedure similar to Part III of this experiment (Analyzing a Vitamin Supplement for Vitamin C Content) as described in the procedure section. A 1.043g vitamin C tablet is crushed, treated, and diluted to 100.00mL in a volumetric flask with deionized water. Three 5.00mL samples of this solution are titrated with DCP that had a standardized concentration of 9.93x10-4M. The three titrations took an average of 35.52mL of DCP. (MM Ascorbic Acid = 176.124 g/mol)

Calculate the mass (in mg) in the vitamin C tablet. (MM Ascorbic Acid = 176.124 g/mol)

Explanation / Answer

mol of DCP = 35.52 x 9.93x10-4/1000 ; which would be the mole of the ascorbic acid in 5 ml vol.

so, in 100 ml vol , the amount of ascorbic acid would be 35.52 x 9.93x10-4/1000 x 100

so weight would be 35.52 x 9.93x10-4/1000 x 100 x 176.12 g = 0.62 g or 620 mg of ascorbic acid is present in the tablet.

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