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bomba923
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I have two aqueous solutions---Fe(III)(NO3)3 and KSCN (no precipitate in either, both are fully dissociated into ions). I react five drops of the ferric nitrate solution with one drop of KSCN (assume that we end up with excess Fe[3+])
The net ionic reaction Fe[3+] + SCN[-] (equilibrium arrows!) FeSCN[2-] forms a blood-red complex ion FeSCN[2-].
I add a small amount (10mg) KNO3 and observe a change (more brown or lighter red). Well, the equilibrium shifted;
Why do I notice a significant color change?
The net ionic reaction Fe[3+] + SCN[-] (equilibrium arrows!) FeSCN[2-] forms a blood-red complex ion FeSCN[2-].
I add a small amount (10mg) KNO3 and observe a change (more brown or lighter red). Well, the equilibrium shifted;
Why do I notice a significant color change?