Nutrtionest
Determination of Vitamin C Concentration by Titration
(Redox Titration Using Iodate Solution) Introduction
This method determines the vitamin C concentration in a solution by a redox titration with potassium iodate in the presence of potassium iodide. Vitamin C, more properly called ascorbic acid, is an essential antioxidant needed by the human body (see additional notes). When iodate ions (IO3−) are added to an acidic solution containing iodide ions (I−), an oxidation-reduction reaction occurs; - the iodate ions are reduced to form iodine
Burette containing potassium iodate solution
IO3− + 6 H+ + 5 e− → ½ I2 + 3 H2O
- while the iodide ions are oxidised to form iodine.
2 I− → I2 + 2 e−
Combining these half-equations demonstrates the reaction between iodate and iodide
2 IO3− + 10 I− + 12 H+ → 6 I2 + 6 H2O
It is the iodine formed by this reaction that oxidises the ascorbic acid to dehydroascorbic acid as the iodine is reduced to iodide ions.
ascorbic acid + I2 → 2 I− + dehydroascorbic acid
Due to this reaction the iodine formed is immediately reduced to iodide as long as there is any ascorbic acid present. Once all the ascorbic acid has been oxidised, the excess iodine is free to react with the starch indicator, forming the blue-black starch-iodine complex. This is the endpoint of the titration. The method is suitable for use with Vitamin C tablets, fresh or packaged fruit juices and solid fruits and vegetables. NB: This method is really the same as titrating ascorbic acid directly with iodine solution (see Vitamin C Method using Iodine). However, this method is more reliable as the potassium iodate solution is more stable than iodine as a primary standard.
Conical flask
Vitamin C extract
1
Equipment Needed burette and stand 20 mL pipette 100 mL volumetric flask 250 mL conical flasks
Titration
1. Pipette 20 mL of the sample solution into a 250 mL conical flask and add about 150 mL of distilled water, 5 mL of 0.6 mol L−1 potassium
(Redox Titration Using Iodate Solution) Introduction
This method determines the vitamin C concentration in a solution by a redox titration with potassium iodate in the presence of potassium iodide. Vitamin C, more properly called ascorbic acid, is an essential antioxidant needed by the human body (see additional notes). When iodate ions (IO3−) are added to an acidic solution containing iodide ions (I−), an oxidation-reduction reaction occurs; - the iodate ions are reduced to form iodine
Burette containing potassium iodate solution
IO3− + 6 H+ + 5 e− → ½ I2 + 3 H2O
- while the iodide ions are oxidised to form iodine.
2 I− → I2 + 2 e−
Combining these half-equations demonstrates the reaction between iodate and iodide
2 IO3− + 10 I− + 12 H+ → 6 I2 + 6 H2O
It is the iodine formed by this reaction that oxidises the ascorbic acid to dehydroascorbic acid as the iodine is reduced to iodide ions.
ascorbic acid + I2 → 2 I− + dehydroascorbic acid
Due to this reaction the iodine formed is immediately reduced to iodide as long as there is any ascorbic acid present. Once all the ascorbic acid has been oxidised, the excess iodine is free to react with the starch indicator, forming the blue-black starch-iodine complex. This is the endpoint of the titration. The method is suitable for use with Vitamin C tablets, fresh or packaged fruit juices and solid fruits and vegetables. NB: This method is really the same as titrating ascorbic acid directly with iodine solution (see Vitamin C Method using Iodine). However, this method is more reliable as the potassium iodate solution is more stable than iodine as a primary standard.
Conical flask
Vitamin C extract
1
Equipment Needed burette and stand 20 mL pipette 100 mL volumetric flask 250 mL conical flasks
Titration
1. Pipette 20 mL of the sample solution into a 250 mL conical flask and add about 150 mL of distilled water, 5 mL of 0.6 mol L−1 potassium