Iron (II) ion (Fe^3+) reacts with thiocynante ion (SCN) to form a red complex io
ID: 1052565 • Letter: I
Question
Iron (II) ion (Fe^3+) reacts with thiocynante ion (SCN) to form a red complex ion with the formula (FeSCN)^2+. The net ionic equation describing this reaction is given in Equation 10. Fe^3+ (aq. It. yellow) + SCN^- (aq, colorless) (FeSCN)^2+ (aq, red) A student studying this equilibrium begins with an equilibrium mixture that is light pink. What change will the student observe when a solution containing Fe^2+ ion is added to this mixture? Briefly explain how your answer to (1) is consistent with lessthanorequalto Chitelier's principle. Silver ion (Ag^+) reacts with SCN6- ion to form silver thiocyanate (AgSCN) What change will student observe when a solution containing Ag^+ ion is added to the mixture? Briefly explain how your answer to (3) is consistent with lessthanorequalto Chateliei's principle.Explanation / Answer
What change will the student observe when s solution containing fe3+ ion is added to the mixture
Fe(III) ions can form the blood red color with CNS- ions,
It happens due to the formation of Fe(CNS)3& Fe(CNS)6 complex with three K/Na+
This complex is visible as red color
the dilution effect has the effect on the color intensity,
briefly explain how your answer is consistent with lechatelier principle
Fe3+(aq, it. yellow) + SCN- (aq, colourless) <-----> [ FeSCN]2+ (aq,red)
For the reaction Fe3+ + SCN – FeSCN2+,
the equilibrium constant expression is [FeSCN2+ ] K = [Fe3+ ] · [SCN – ] where
, for example, [Fe3+ ] is the molar concentration (mol
Fe3+ / L solution) present in an equilibrium mixture.
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