Question

Q: Estimate the half-life from the following graph S Time (min) Exp. #17: Chemical Equilibrium: Consider the following Equilibrium: Fe."(aq) +3SCN(aq) Fe(SCN),(aq) Q: What happens to the equilibrium when a few mL of NaOH(aq) are added to the test tube where this equilibrium is occurring?

ignore the graph. just need help on experiment 17

Answer 1

Actually we are adding the base to the equilibrium mixture , so we need to check whether there is any acid in the reaction mixture in ordered to study the effect on equilibrium.

Fe(OH)₃ is insoluble in water, then adding NaOH to the equilibrium system should cause the reaction to take place: adding NaOH precipitates Fe³⁺ as Fe(OH)₃ from the equilibrium system. If Fe³⁺ is removed from the equilibrium system, then the system will no longer be in equilibrium and will have to react in the direction that restores some Fe³⁺

here in this case Fe3+ ion in the reaction mixture forming (Fe(OH)3) after it reacting with base NAOH ,which implies that the amount of reactant in the reaction mixture decreases on adding base .hence the reaction shift towards reactant side(backward direction) according to the le chatliers principle to restore the amount of fe3+.