4. A sample of orange juice was titrated with the standardized iodine solution f

Question

4. A sample of orange juice was titrated with the standardized iodine solution from the previous problem. A 100 mL sample of juice took 10.57 mL of I2 to reach the starch end point. a. Write the reaction of vitamin C with iodine. b. What is the stoichiometric ratio of vitamin C to iodine in the reaction? c. What is the concentration of the vitamin C in units of mg Vit C/100 mL juice? mg Vit C 100 mL d. How much of the juice does one need to drink to meet the RDA standard amount of vitamin C for one day? mL juice

Explanation / Answer

Desity of iodine = 3.96 gm / mL

So mass of iodine used = 3.96 * 10.57 = 41.86 gm

molar mass of iodine = 126.9 gm/mol

therefore mol of iodine used = 41.86 / 126.9 = 0.33 mol

Since stoichiometric ratio of vitamin C to iodine is 1:1.

So,mole of vitamin C in 100 ml = 0.33 mol

molar mass of vitamin C = 12*6 + 1*8 + 16*6 = 72 + 8 + 96 = 176 gm/mol

concentration of Vitamin C = 176 * 0.33 * 1000 mg Vit C / 100 mL

= 58080 mg Vit C / 100 mL

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