Calculation of the number of moles of IO3- used in the titration(i.e. in the Erlenmeyer flask):
KIO3(s) → K+(aq) + IO3-(aq): balanced eqn of dissolving KIO3 in water
1. Calculate the moles of KIO3 used: Molecular weight of KIO3 = 214.0011 g/mol
Amount of KIO3 used in grams = 0.0356g
# of moles = 0.0356g/(214.0011g/mol) (grams cancels out) = 1.6635 × 10^-5 moles
The mole ratio is 1:1:1. So # of moles of KIO3 will be equal to # of moles of IO3-
2. Calculate the Molarity
Amount of dH2O used for dissolving = 100mL = 0.1L
Molarity = (moles of solute) / (volume of solution in Liters) = 1.6635 × 10^-5 moles/0.1L
= 1.6635 × 10^-4 moles/L
I did untill this. But in the question, it says that <Calculate the # of moles of IO3- in the Erlenmeyer flask> And in the Erlenmeyer flask, there was 10mL of KIO3 solution, and other solution of 54ml.
And my question is, do I have to multiply the molarity I gained by calculation by 0.064mL (because (10ml+54ml)/1000 = 0.064L=amount in Erlenmeyer flask) to gain the # of moles of IO3- in the Erlenmeyer flask, Or can I just multiply the molarity by 10mL Or am I doing wrong??