How do you calculate the moles of triiodide that is consumed by a thiosulfate titrant in a Vitamin C titration?
IO3– + 8 I– + 6 H+ -> 3 I3– + 3 H2O
I3– + 2 S2O32– -> 3 I– + S4O62–
Moles of I3- = 0.0013
Endpoint = 11.05 ml
Please let me know if you need more info.
Thank you for providing the additional information.
1 mol I3^- is consumed by 2 mols S2O3^2- so moles S2O3^2-/2 = mols I3^-
If that 0.0013 mols I3^- is the amount of I3^- formed from the addition of IO3^-, then 1/2 mols S2O3^2- will give you the excess I3^- formed. Hope this helps.
Well, it seems you've got a reaction party going on there! IO3– and I–, getting together with some H+ cocktails to form I3– and H2O. And then I3– gets cozy with S2O32– to produce even more I– and S4O62–. Quite the chemistry cocktail, I must say!
Now, to calculate the moles of triiodide consumed, we need to use our trusty stoichiometry skills. The balanced equation tells us that 1 molecule of I3– reacts with 2 molecules of S2O32–. But we need to convert that to moles because, well, moles are cool.
Since you mentioned that the moles of I3– is 0.0013, we can use that to determine the moles of triiodide consumed. So, for every 1 molecule of I3–, we need 2 molecules of S2O32–. And since 1 mole of any substance contains Avogadro's number of molecules (approximately 6.022 x 10^23), we can use our stoichiometry skills to calculate the moles of triiodide consumed. Let's do it!
0.0013 moles I3– x (2 moles S2O32– / 1 mole I3–) = 0.0026 moles of S2O32– consumed
So, the moles of triiodide consumed by the thiosulfate titrant in your Vitamin C titration is 0.0026.
Hope that helps! And remember, chemistry jokes are always a mole-ment of levity in serious calculation times.
To calculate the moles of triiodide (I3-) that is consumed by the thiosulfate titrant in a Vitamin C titration, you can follow these steps:
1. Determine the number of moles of triiodide (I3-) present in the given volume of solution:
Moles of I3- = concentration x volume
Given that the volume is 11.05 mL and the moles of I3- is 0.0013, you need to rearrange the equation to solve for the concentration:
Concentration of I3- = moles of I3- / volume
2. Use stoichiometry to calculate the moles of thiosulfate (S2O32-) required to react with the moles of triiodide (I3-):
From the balanced equation:
1 mole of I3- reacts with 2 moles of S2O32-
So moles of S2O32- = 2 x moles of I3-
3. Calculate the moles of triiodide consumed by the thiosulfate titrant:
Moles of triiodide consumed = moles of I3- initially present - moles of I3- remaining after titration
4. Substitute the known quantities into the equations to calculate the moles of triiodide consumed by the thiosulfate titrant.
To calculate the moles of triiodide (I3-) consumed by a thiosulfate titrant in a Vitamin C titration, you need to use the balanced chemical equation and the volume of thiosulfate titrant used.
Step 1: Determine the balanced chemical equation
The balanced chemical equation shows the mole ratio between the substances involved in the reaction. In this case, the balanced chemical equation is:
I3- + 2 S2O32- -> 3 I- + S4O62-
This equation shows that 1 mole of I3- reacts with 2 moles of S2O32- to produce 3 moles of I-.
Step 2: Determine the moles of thiosulfate titrant used
You mentioned that the endpoint was reached at 11.05 ml. In titrations, it's common to use the concentration (molarity) of the titrant to calculate the number of moles used. But since you haven't provided the concentration, we'll have to work with the volume instead.
Step 3: Calculate the moles of I3- consumed
To calculate the moles of I3- consumed, you need to use the stoichiometry (mole ratio) between I3- and S2O32- from the balanced chemical equation.
Using the balanced equation, we know that 1 mole of I3- reacts with 2 moles of S2O32-. Therefore, if we know the moles of S2O32-, we can determine the moles of I3-.
Since 1 mole of I3- is equivalent to 2 moles of S2O32-, we can use the following relationship:
1 mole I3- : 2 moles S2O32-
moles of I3- = (moles of S2O32-)/2
Given that you have mentioned the moles of I3- to be 0.0013, we can calculate the moles of S2O32- used:
moles of S2O32- = 2 * moles of I3-
moles of S2O32- = 2 * 0.0013
moles of S2O32- = 0.0026
Therefore, the moles of triiodide (I3-) consumed by a thiosulfate titrant in this Vitamin C titration is 0.0026 moles.