(3) At room temperature, 80.0 ml of 0.125 M AgNO 3 (aq) and 20.0 ml of 0.500 M F

Question

(3) At room temperature, 80.0 ml of 0.125 M AgNO3(aq) and 20.0 ml of 0.500 M Fe(NO3)2(aq) are mixed together, generating the following equilibrium system

Ag+(aq) + Fe2+(aq) -> Ag(s) + Fe3+(aq).

At equilibrium, the concentration of Fe3+ is 0.00505 M.

(a) (4 pts) Calculate the initial concentrations of Ag+(aq) and Fe2+(aq) immediately upon mixture of the two solutions (you may disregard any changes in volume due to mixing).

(b) (4 pts) What is the value of the equilibrium constant Kc at room temperature for this system? (c) (6 pts) Dilute the resulting solution with water to 200.0 ml. What chemical reaction, if any, will

take place? Calculate the equilibrium concentrations of each reagent in this diluted solution.

Explanation / Answer

initial concentration of Ag+=80*.125/(80+20)=0.1M;

initial concentration of Fe2+=20*0.05/(80+20)=0.1M;

Kc=[Fe3+]/[Ag+]/[Fe2+]=0.00505/(0.1-0.00505)^2=0.56;

since dilution doesnt change concentration no reaction will occur;

final concentration:[Fe3+]=0.00505 M ;[Ag+]=[Fe2+]=1-0.00505=0.09495 M

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