Question

Use Le Châtelier's Principle to predict how this equilibrium system will respond to the changes you will make: Fe3+(aq) + SCN-(aq) ⇌ FeSCN2+(aq) How will adding silver nitrate (AgNO3) initially change the Fe3+, SCN-, and FeSCN2+ concentrations? How will the equilibrium system respond to this change? (Hint: The nitrates, NO3-, of all metal ions are soluble in water. Silver thiocyanate, AgSCN, is not very soluble in water.) (a) The SCN- concentration increases and the other concentrations decrease. The reaction shifts right (products) to reach equilibrium. (b) There is no effect on the concentrations. The system remains at equilibrium. (c) The SCN- and FeSCN2+ concentrations decrease while the Fe3+ concentration increases. The equilibrium shifts to the left (reactant side). (d) The SCN- and Fe3+ concentrations increase and the FeSCN2+ concentration decreases. The reaction shifts right (product side).

          Use Le Châtelier's Principle to predict how this equilibrium system will respond to the changes you will make:

Fe3+(aq) + SCN-(aq) ⇌ FeSCN2+(aq)

How will adding silver nitrate (AgNO3) initially change the Fe3+, SCN-, and FeSCN2+ concentrations? How will the equilibrium system respond to this change? (Hint: The nitrates, NO3-, of all metal ions are soluble in water. Silver thiocyanate, AgSCN, is not very soluble in water.)

(a) The SCN- concentration increases and the other concentrations decrease. The reaction shifts right (products) to reach equilibrium.
(b) There is no effect on the concentrations. The system remains at equilibrium.
(c) The SCN- and FeSCN2+ concentrations decrease while the Fe3+ concentration increases. The equilibrium shifts to the left (reactant side).
(d) The SCN- and Fe3+ concentrations increase and the FeSCN2+ concentration decreases. The reaction shifts right (product side).

Added by Debra L.

Question

Please give Ace some feedback