C-vitamin titration (Equivalence Point)

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SUMMARY

The discussion revolves around a titration experiment involving C-vitamin (ascorbic acid) using Potassium Iodate (KIO3) as the titrant. The user conducted three trials, with the first two involving juice and the third using pure C-vitamin. Due to lost data, the user seeks guidance on estimating the volume at which the endpoint is reached, specifically in terms of color change to dark blue or pink. The reaction equations provided indicate the stoichiometry involved, but the exact volume of titrant required remains uncertain without the original data.

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Homework Statement


OK, so I did this experiment a week ago,
I took 75g of juice and added some 1.5gKI, 7.5cm^3HCl and 5cm^3starch and titrated with Potassium Iodate 0.010M(KIO3). I did this titration again
For the third experiment, I just took 0.1g pure C-vitamin dissolved in some water instead of juice and everything the same.
But, unfortunately, I have lost my data and there is no possiblity that I can gain information from anywhere on the equivalent points of these 3 trials.

If you could just give me an idea at what volume the color would be dark blue (shud it be dark blue or pink?)
Just an idea in what range maybe?

e.g. 24cm^3 or something like that
The only thing I remember was that there wasn't a lot of difference between the eq. point in the first and the second trial...

P.S.
The reaction that takes place is:
IO3 + 5I + 6H ---- 3I2 + 3H2O
AND

I2 + c vitamin --- 2I + 'products'PLEASE HELP

REPORT DUE TOMORROW
 
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There is no way anyone can help you. Volume of titrant depends on the sample composition, which is unknown. You may roll the dice as well.

Best approach I can think off is to write your report stating at the very beginning you have lost your data, so you made up some numbers and you did all the calculations using them. This way you at least show good will.
 

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