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,

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?

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.

0.22012

To find the mole to mole ratio to convert Fe to TI, we need to look at the balanced equation for the reaction between Fe and Cr2O7.

The balanced equation is: Cr2O7 + 6 Fe + 14 H -> 6 Fe + 2 Cr + 7 H2O

From the equation, we can see that 6 moles of Fe react with 1 mole of Cr2O7. Now we can set up the mole to mole ratio:

6 mol Fe / 1 mol Cr2O7

Since the Fe solution was titrated with the dichromate solution, which in turn was produced from TI2CrO4, we know that the number of moles of Cr2O7 is equal to the number of moles of TI2CrO4 (which is equal to moles of TI):

6 mol Fe / 1 mol Cr2O7 = x mol TI / 1 mol TI2CrO4

Now we can solve for x (moles of TI):

x = (6 mol Fe / 1 mol Cr2O7) * (1 mol TI2CrO4 / 1 mol TI)

x = 6 mol Fe

Therefore, the mole to mole ratio to convert Fe to TI is 1:1.

Now we need to find the mass of TI in the sample solution. To do this, we can use the equation:

moles of TI = concentration of TI * volume of TI solution

The concentration of TI is not given in the question, so we cannot calculate the exact mass of TI. Additional information or calculations will be required to determine the concentration of TI in the solution.

To find the mass of TI in the sample solution, you can follow these steps:

1. Determine the moles of Fe in the solution:
- The given concentration of Fe solution is 0.1004 M.
- The volume of Fe solution used is 40.60 mL or 0.04060 L.
- Multiply the concentration by the volume to obtain the moles of Fe:
Moles of Fe = 0.1004 M x 0.04060 L = 0.00407624 mol

2. Use the mole-to-mole ratio to convert from Fe to TI:
- From the balanced equation 2TI2CrO4(s) -> 2H -> 4TI + Cr2O4 + H2, we can see that 2 moles of TI2CrO4 produce 4 moles of TI.
- Therefore, for every mole of TI2CrO4, we have 2 moles of TI.
- This means that the mole-to-mole ratio between Fe and TI is 1:2.

3. Calculate the moles of TI:
- Multiply the moles of Fe by the mole-to-mole ratio to obtain the moles of TI:
Moles of TI = 0.00407624 mol Fe x (2 mol TI / 1 mol Fe) = 0.00815248 mol TI

4. Convert moles of TI to mass:
- To calculate the mass of TI, we need to know the molar mass of TI. Let's assume it is 47.87 g/mol (using the average atomic mass of TI).
- Multiply the moles of TI by the molar mass to obtain the mass of TI:
Mass of TI = 0.00815248 mol TI x 47.87 g/mol = 0.3896 g (rounded to four decimal places)

Therefore, the mass of TI in the sample solution is approximately 0.3896 grams.