I did a lab last week about chemical equilibrium, and I need to explain why the stock solution of .01M Fe(NO3)3 and KSCN (which is already a rust red color) turns a darker red when 5 drops of .1M Fe(NO3)3 is added to one well (1mL stock), and why it turns even a deeper red when 5 drops of 0.1M KSCN is added to another well of the same stock (1mL). I'm thinking that it shifts everything to the right, but I can't exactly explain it? One well was the stock + 0.1M Fe(NO3) (darker red than stock), and the other well was stock + 0.1M KSCN.(even darker than when 0.1 Fe(NO3)3 was added to the other well). Why? I also need a net ionic equation to explain it... but as far as I know, it's the same reaction as the stock? Oh, everything is aqueous, btw.

Any help would be great!
Thanks!

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