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April 20, 2014

April 20, 2014

Posted by **titration** on Tuesday, October 7, 2008 at 5:36pm.

1.) 1.7423g of potassium dichromate were placed in a 250.00 mL volumetric flask and water was added to the mark. Calculate the molarity of the dichromate solution to the appropriate number of significant figures.

0.0237M ?? is this correct

2.) a 1.2523 g sample of a souluble iron(II) salt was dissolved in water and titrated with the dichromate solution prepared in question #1. 37.50mL of the dichromate solution was required to reach the end point.

a.) calculate the mass in grams of iron in the sample.

b.) Calculate the percent of iron in the sample.

- chemistry -
**DrBob222**, Tuesday, October 7, 2008 at 5:49pmThe molarity of the dichromate appears to be correct; however, you have 5 significant figures in both the mass and the volume. You need to carry out the division to 5 s.f.

- chemistry -
**DrBob222**, Tuesday, October 7, 2008 at 5:55pmFor #2:

1. Write the equation for the titration of iron(II) with dichromate and balance it.

2. Calculate the mols of dichromate used. M x L = mols.

3. Convert mols dichromate in step 2 to mols iron(II) using the coefficients in the balanced equation.

4. Convert mols iron to grams iron.

5. Calculate percent iron.

%Fe = [mass iron step 4/mass sample in the problem]*100 = ??

- chemistry -
**titration**, Thursday, October 9, 2008 at 12:25amMy balanced answer is

6Fe + Cr2O7 + 14H ---> 6Fe + 2Cr + 7H2O

for mols of dichromate i got 0.00088834

but what would be my conversion factor for part 3?

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