Iron(III) ion (Fe^3+) reacts with thiocyanate ion (SCN^-) to form a red complex

Question

Iron(III) ion (Fe^3+) reacts with thiocyanate ion (SCN^-) to form a red complex ion with the formula [FeSCN]^2+. The net ionic equation this reaction is given in Equation 10. Fe^3+ (aq, It. yellow) + SCN^- (aq, colorless) reversible [FeSCN]^2+ (aq, red) A student studying this equilibrium mixture that is light pink. What change will the student observe when containing Fe^3+ ion is added to this mixture? Briefly explain how your answer to (1) is consistent with lessthanorequalto Chatelier's principle. Silver ion (Ag^+) reacts with SCN ion to form silver thiocyanate (AgSCN). What change will the student observe when a solution containing Ag^+ ion is added to the mixture? Briefly explain how your answer to (3) is consistent with lessthanorequalto Chatelier's principle.

Explanation / Answer

Q1.

if you add Fe+3 ions, the shift goes toward products, since there is excess of reactants

so the solutoin gets more RED

Q2.

it is consistent, since more reagent will favour more produciton of FeSCN, therefore, the red color must increase

Q3.

if you add Ag+ ions, then you will have AgSCN production

SCN- decreases, so the reagents decrease

the reaction stops productino of FeSCN complex, and the complex starts formid reactants

so the color goes more YELLOW

Q4.

this is consistent, since Q = [products] / [reactants] constant must be kept...

Related Questions

Navigate

• Browse (All)
• Browse I
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.