3. A solution contains the blood-red hexathiocyanatoferrate(III) complex ion, Fe
ID: 549853 • Letter: 3
Question
3. A solution contains the blood-red hexathiocyanatoferrate(III) complex ion, Fe(SCN) in equilibrium with the iron(III) ion, Fe3, and six thiocyanate ions, SCN-. If the solution is diluted with water, will the color deepen, fade, or stay the same? Why? In addition to predicting whether the solution will deepen, fade, or stay the same, give TWO reasons for that prediction. One of those reasons will involve Le Chatelier's Principle, and one will not. (At least, that will be the case if you make the right prediction!)Explanation / Answer
Equilibrium:
Fe(SCN)63- (aq) <-----> Fe3+ (aq) + 6 CN-(aq)
The color is due to Fe(SCN)63- complex. So, the increase in concentration of complex deepen the color and decrease in the concentration of complex fades the color.
When solution is diluted with water, the concentrations of all species in the solution decreases as well complex concentration also. Thereofe, the solution color faded.
Ionization is in aqueous meadium, here we treat water also one of the reactant.
According to Le Chatelier's principle, as increasing the concnetraion of reactant shift the equilibrium towards product side. So, increasing water (reactant), the equilibrium shift towards products. So, the concentraion of complex (one of the reactant) decreases. Hence, the soluiton color fades.
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