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1. A student mixes 5.00 mL 2.00 x 10-3 M Fe(NO3) in 1 M HNO3 with...

1. A student mixes 5.00 mL 2.00 x 10-3 M Fe(NO3) in 1 M HNO3 with 3.00 mL 2.00 x 10-3 M KSCN and 2.00 mL of water. She finds that in the equilibrium mixture the concentration of FeSCN2+ is 7.0 x 10-5 M. Find Kc for the reaction Fe3+ (aq0 + SCN- (aq0 ------Fe(SCN)2+ (aq).

Step 1 Find the number of moles Fe3+ and SCN- initially present.

Step 2. How many moles of FeSCN2+ are in the mixture at equilibrium? What is the volume of the equilibrium mixture?

How many moles of Fe3+ and SCN- are used up in making the FeSCN2+?

How many moles of Fe3+ and SCN- remain in the solution at equilibrium?

What are the concentrations of Fe3+, SCN-, and FeSCN2+ at equilibrium?

Fe3+= M; (SCN-)= M; (FeSCN2+)=

what is the value of Kc for the reaction?

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