I understand how to do ICE tables chemistry but how would apply it or calculate for this table?

Question

Test Tube: Volume of 1.25x10^-4M Fe(NO3)3mL: Volume of 1.0M KSCN mL: Volume of 0.10M HNO3 mL

1 0.50 2.50 2.00

2 1.00 2.50 1.50

3 1.50 2.50 1.00

4 2.00 2.50 0.50

5 2.50 2.50 0.00

How would I find the calculated FeSCN2+ for each test tube?

Heres the net ionic equation again Fe3+SCN-=FeSCN^2+

Answer 1

Given that you know K for the reaction The equilibrium expression equals K at equilibrium. Note that the total volume after mixing has been held constant, so we can use molarities after dilution as the starting concentrations of the two reactants.

K = [FeSCN²⁺]/([Fe³⁺][SCN^-])

If x ibe the molarity of the Fe³⁺ reacted, then , for the first case:

K = x/((1.25 x 10^-4M (.5 ml/5 ml) -x)(1.0 M(2.5 ml/5 ml)-x)) which leads to a quadratic in x.

You can do this for each row. Note that if you want moles, you'll multiply x by .005 liters.