[bigmoe70]

Hi everyone, new to forums here. I'm having trouble with this question:

At a certain temperature K = 1.10×103 for the reaction:

Fe3+(aq) + SCN-(aq)= FeSCN2+(aq)

2.00×10-2 mol of Fe(NO3)3 is added to 5.90×10-1 L of 3.22×10-1 M KSCN.

Neglecting any volume change and assuming that all species remain in solution--:

Calculate the equilibrium concentration of Fe3+ (in mol/L).

Calculate the equilibrium concentration of SCN- (in mol/L).

Calculate the equilibrium concentration of FeSCN2+ (in mol/L).

I'm having trouble figuring out how to calculate the initial concentrations of Fe3+, SCN- and FeSCN2+.

Thanks for your help.

[Borek]

http://en.wikipedia.org/wiki/ICE_table