# Chemistry

Someone help me with my titration molarity calculation please!?

I have titrated 1.000 mL of Ca(IO3)2 with 2.197 ml of 0.022 M thiosulfate.

First I found the moles of thiosulfate present with
0.002197 L x 0.022 M = 4.8388E-5.

The mole ratio of S2O3^-2 and IO3- should be 6:1 (Please tell me if that is correct or not!)

So 4.8388E-5/6 = 8.0648E-6 moles.

I found the Molarity with this equation:
M = 8.0648E-6 moles/.001 L
= .00806 M IO3-

Can anyone please check if this is correct? I want to know before I continue and make a tremendous amount of mistakes if it's wrong.

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1. First I object to saying you titrated Ca(IO3)2 with S2O3^-. You didn't do that; you added I^- to IO3^- and titrated the liberated I2 with S2O3^-
Here are the equations.
Ca(IO3)2 ==> Ca^2+ + 2IO3^-
IO3^- + 5I^- ==> 3I2 (which isn't complete but the redox part is balanced).
I2 + 2S2O3^2- ==> S4O6^2- + 2I^-

So 1Ca(IO3)2 = 2IO3^- = 6I2 = 12S2O3^2-

I think your first calculation is wrong.
0.002197 x 0.022 = 4.833E-5 mols S2O3^2-.

mols IO3^- = 4.833E-5 x (1 mol Ca(IO3)2/12 mols S2O3^2-) = ?
Then M = mols Ca(IO3)2/L Ca(IO3)2 = ?
Check that ratio. Just follow the multipliers fromj one equation to the next and you get 1:12.

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