I recently performed a lab on Chemical Equilibrium. Here is some background on the experiment: -We made...

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Chemistry

I recently performed a lab on Chemical Equilibrium.
Here is some background on the experiment:
-We made a stock solution by combining Fe(NO3)3 and NH4SCN. Thismade a blood red solution. Then, we added different reagents to seethe change of color and the shift of equilibrium.
I'm being asked the following question: Based on the color ofsolutions reported, determine the direction of the reaction's:Fe^3+(aq)+SCN^- --> [FeSCN]^2+(aq) equilibrium shift upon eachaddition of each reagent investigated and write the chemicalreaction involving the reagent that is reponsible for theshift.
We investigated the following additions:
a. 1 M iron (III) nitrate
-Upon adding iron (III) nitrate to the blood red stock solution,it turned a somewhat lighter red.
b. 1 M ammonium thiocyanate
-Upon adding this to the stock solution, it turned from bloodred to a dark red/black
c. 0.1 M tin (II) chloride
-Upon adding this to the stock solution, it turned from bloodred to a cloudy orange color.
Please explain how you determined the shift and equation, Idon't understand how to find either.
Thank you so much for your help!

Answer & Explanation Solved by verified expert

4.1 Ratings (636 Votes)

Fe3aq SCN FeSCN2aqYellow Colorless Deep redaAdditions of Iron III nitrateThe Iron III nitrate is going to dissociate in your solutioninto Fe3 and 3Cl Your elemental iron IIIhas an oxidation number of 3 and so does the Iron atom inFeSCN2 But See Answer

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