Explain the effect of concentration on equili | vedclass

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Question

(B) The equilibrium reaction is: $Fe^{3+}_{(aq)} + SCN^{-}_{(aq)} \rightleftharpoons [Fe(SCN)]^{2+}_{(aq)}$.Adding $KSCN$ increases the concentration

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$b.$ Equilibrium shifts to the right and the red color intensity increases.

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(B) The equilibrium reaction is: $Fe^{3+}_{(aq)} + SCN^{-}_{(aq)} \rightleftharpoons [Fe(SCN)]^{2+}_{(aq)}$.Adding $KSCN$ increases the concentration of $SCN^{-}$ ions.According to Le Chatelier's principle,the equilibrium shifts in the direction that consumes the added reactant,which is the forward direction (right).This results in an increase in the concentration of the blood-red complex $[Fe(SCN)]^{2+}$,thereby increasing the intensity of the red color.

Explain the effect of concentration on equilibrium when two drops of $0.2 \ M$ potassium thiocyanate $(KSCN)$ are added to $1 \ mL$ of $0.2 \ M$ iron $(III)$ nitrate solution.

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