I am working on a lab and thedirections say to write the balanced chemical react

Question

I am working on a lab and thedirections say to write the balanced chemical reaction for thegiven net ionic equations.

Example: Iron (III) ions, Fe3+, and thiocyanide ions, SCN-, cancombine to form the iron (III) thiocyanate ion, FeSCN-, and set upequilibrium as shown in this net ionic equation:

Fe3+(aq) + SCN-(aq)<---> FeSCN2+(aq) (i used '<--->'for equilibrium sign)

You will examine the effects of adding different reagents(FeCl3, NH4SCN, and HgCl2) to thisequilibrium system.

Thanks for any help.

Explanation / Answer

  Fe3+(aq) +SCN-(aq) <--->FeSCN2+(aq) FeCl3 contains Fe3+ ions so onadding   FeCl3 to the equilibrium thenthe the concentration of Fe3+ ions increases hencereaction will procced towards products side to maitain theequilibrium.    NH4SCN contains SCN- ionsso on adding  NH4SCN to the equilibriumthen the the concentration of SCN- ions increaseshence reaction will procced towards products side to maitainthe equilibrium. Addition of HgCl2  does noteffect the equilibrium because it is not having common ion with anyone of the reactants. FeCl3 contains Fe3+ ions so onadding   FeCl3 to the equilibrium thenthe the concentration of Fe3+ ions increases hencereaction will procced towards products side to maitain theequilibrium.    NH4SCN contains SCN- ionsso on adding  NH4SCN to the equilibriumthen the the concentration of SCN- ions increaseshence reaction will procced towards products side to maitainthe equilibrium. Addition of HgCl2  does noteffect the equilibrium because it is not having common ion with anyone of the reactants.

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