Question

Consider the following equilibrium: Fe3+ + SCN1-   ↔ FeSCN2+ Fe3+ and SCN1- are essentially colourless and...

Consider the following equilibrium:

Fe3+ + SCN1-   ↔ FeSCN2+

Fe3+ and SCN1- are essentially colourless and FeSCN2+ is blood red in colour.

How would you expect the intensity of colour to change if SCN1- were added? (Choose...IncreaseDecreaseNo change)

How would you expect the reaction to shift if OH1- were added? (Choose...ForwardReverseNo change)

How would you expect the intensity of colour to change if Ag+ were added (Choose....increase,decrease,no change)

Science   Chemistry   
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Answer #1

To discuss this question,let us first be aware of the Formation Constant of Fe and thiocyaanate complex.The Fe and SCN- can form complex in presence of excess Thiocyanate.

So,Intensity of colour would increase if excess SCN-is added.

If OH- is added to the equilibrium, The complex would be formed in some amount which would result decrease in the rate of forward reaction of Fe-Thiocyanate complexation and from Le Chatelier's principle,in fact some would dissociate to give back i.e. the reaction would shift in reverse direction.

has a formation constant in the order of whereas has a formation constant in order.So the colour intensity of the Fe-Thiocyanate would decrease as the equilibrium shifts backwards.

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