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!
