Question: a 25.00 mL. aliquot of a solution containing TI(aq) was treated with K2CrO4. the TI2CrO4 was filtered, washed free of excess precipitation reagent, and dissolved in dilute sulfuric acid. the dichromate ion produced was titrated with 40.60 mL. of .1004 m Fe solution. What was the mass of TI in the sample solution. the reactions are : 2TI+CrO4 -> Ti2CrO4,

Question

2TI2CrO4(s) -> 2H -> 4TI+ Cr2O4 + H2),
Cr2O7 + 6 Fe+ 14 H -> 6 Fe +2 Cr + 7 H2O.

How do i go about getting the mass of TI in the sample. You can get the moles of Fe in the solutin by taking .1004 M * .04060 L= .oo407624 mol. What would the mole to mole ratio be to convert to TI?

Answer 1

moles Cr2O7^-2 = (1/6)*moles Fe. Right?
And moles Tl = 4*moles Cr2O7^-2.
So moles Fe*(2/3) = moles Tl?
Check my thinking.

Answer 2

0.22012