123. A 0.552-g sample of ascorbic acid (vitamin C) was dissolved in water to a total volume of 20.0 mL and titrated with 0.1103 M KOH. The equivalence point occurred at 28.42 mL. The pH of the solution at 10.0 mL of added base was 3.72. From this data, determine the molar mass and K, for vitamin C.

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Calculate the weight percent of ascorbic acid in a tablet of Vitamin C from the following data: A 100 mg sample of a crushed Vitamin C tablet was dissolved in 40 mL of H2SO4 and 20 mL of water. Two grams of KI and 30. mL of 0.0126 M KIO3 solution was added, and the mixture titrated to a starch endpoint. The titration required 26 mL of 0.0490 M thiosulfate solution.

Vitamin C, ascorbic acid (C₆H₆O₆)(molar mass 176.1 g/mol), is a reducing agent. One way to determine the ascorbic acid content of a sample is to mix the acid with excess iodine and then titrate the iodine that did not react with the ascorbic acid with sodium thiosulfate.

Suppose 50.00 mL of 0.0520M I₂ was added to the sample containing ascorbic acid. After the ascorbic acid/I₂reaction was complete, the I₂not used in the reaction required 20.30 mL of 0.196 M Na₂S₂O₃ for titration to the equivalence point. What is the mass of ascorbic acid in the unknown sample?

greyox416

Vitamin C is a water-soluble vitamin, so your body doesn't store it. You have to get the required amount from your diet (citrus fruits are a great source!), or you could take a daily vitamin C supplement pill. Vitamin C is ascorbic acid, so to determine how much vitamin C (acid) has been placed in each pill, you could do an acid-base titration.

One vitamin C pill was dissolved in water and titrated to an endpoint by 16.00 mL of a 0.447 M solution of NaOH. How many grams of ascorbic acid were there in the pill? (MW of ascorbic acid is 176.1 /mol).