I took 0.100g of ascrobic acid and took 30 ml of water to disolve it. I then fil

ID: 1009794 • Letter: I

Question

I took 0.100g of ascrobic acid and took 30 ml of water to disolve it. I then filled the rest up to 100ml (the fill line on the volumetric flask)

I then took another flask and poured 20ml of that solution in it and added 1.0ml of the starch indicator solution and added it to it.

I then took a burette and put 50ml of 0.015 M iodine solution

After 7.60 ml had been dispenced, it changed to a orange yellow color. The total volume of the flask was 27.62ml.

1. Based on the number of moles of ascorbic acid and iodine reacted during the titration, what is the stoichiometry of the reaction?

A.1 I2 : 1 C6H8O6

B.5 I2 : 1 C6H8O6

C.2 I2 : 1 C6H8O6

D.1 I2 : 2 C6H8O6

C6H8O6 + I2 -------> C6H6O6 + 2H+ + 2 I-

From the balanced eqaution between ascorbic acid and iodine, the number of moles of iodine and ascorbic acid are in the ratio of 1:1.

Answer = A) 1 I2 : 1 C6H8O6