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3 months ago
Experimental Design

The potassium dichromate solution is first standardized by titration with a sample of an acidified mol/L solution of the primary standard, iron(II) ammonium sulfate-6-water.  The concentration of Cr2O72-(aq)  was found to be 0.0085 mol/L. The standardized dichromate solution is then titrated against a 20.00 mL sample of the acidified tin(II) chloride solution.

Evidence

 

TITRATION OF TIN (II) SOLUTION

(volume of K2Cr2O7(aq) required to react with 20.00 ml of Sn2+(aq))

Trial

1

2

3

4

Final buret reading(ml)     

11.8

22.9

33.9

45.0

Initial buret reading (ml)     

0.3

11.8

22.9

33.9

  Find the concentration of the Sn2+(aq) in mol/L:  (give your answer to 4 decimal places)

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wrote...
Educator
3 months ago Edited: 3 months ago, bio_man
Could you confirm the final chemical equation?

I'm getting:

Cr2O72- + 6Fe3+ + 3Sn2+ ⇄ 6Fe2+ + 2Cr3+ + 7H2O + 3Sn4+

I'm doubting that it is right correct, please confirm and get back to me as soon as possible. Remember, if this is incorrect, everything else is wrong too, so it's a major stepping stone, and I don't want to mislead you with the wrong answer
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wrote...
3 months ago
Yeah I believe that was my equation as well still waiting to see what I get on that. If you could help me with my granary question that would be great!
Answer accepted by topic starter
wrote...
Educator
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Posts: 24715
3 months ago
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So if that was your equation, the mole value for Sn2+ should be 70.028 mol/L

I find this answer problematic honestly because it feels like too large of a number for molarity, especially for an ion. Could you could check to see if that is in fact the right formula? I have included the rest of the solution in the attachment showing how I got:
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