Following equilibrium is set up when `SCN^(-)` ion is added to `Fe^(3+)` in aqueous solution :
`underset("Pale yellow")(Fe^(3+))" "+" "underset("Colour less")(SCN^(-))" "hArr" "underset("Deep red")([Fe(SCN)]^(2+))`
When silver nitrate is added to the solution, AgSCN gets precipitate. What will happen to the equilibrium?

Explanation

Equilibrium gets displaced to the left because with removal `SCN^(-)` ions from the equilibrium mixture, more of the deep red complex (product) will decompose into the reagets. Thus, the colour of the solution will slowly change from deep red to pale yellow.