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Given the reaction:
Fe3+(yellow) + SCN-(colorless) <--> [FeSCN]2+(dark red)
If Fe3+ is added to the solution:
Group of answer choices

A. No changes in color occur

B. The solution turns darker red

C. The solution becomes colorless

D. The solution becomes more yellow

Respuesta :

Fe3+(yellow) + SCN-(colorless) <--> [FeSCN]2+(dark red)

If Fe3+ is added to the solution the solution turns darker red

While precipitating out Fe3+ (as Fe(OH)3) or SCN- (as AgSCN) will push the equilibrium to the left, consuming the complex and reducing color intensity, the addition of Fe3+ or SCN- will push the equilibrium to the right, creating more complex and intensifying the color.

The pace of reaction rises as Fe3+ levels rise. The concentration of SCN reduces as the rate rises.

The FeSCN2+ complex, which is created when iron(III) and thiocyanate ions react, displays an extremely strong blood red color (or orange in diluted solution), making it simple to detect and quantify using spectrophotometry.

To learn more about Fe3+ and SCN reaction please visit -
https://brainly.com/question/14575042
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