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## Homework Statement

The reaction 2Fe

^{3+}+ Ni(s) = 2Fe

^{2+}+ Ni

^{2+}has equilibrium constant K = 1.5E34. What is the concentration of Fe

^{3+}at equilibrium if a lot of Ni(s) is added to a 0.1 M solution of Fe

^{3+}that initially contains no Fe

^{2+}?

## The Attempt at a Solution

K = 4x

^{3}/(0.1-2x)

^{2}

My plan is to find x. [Fe

^{3+}] is then 0.1-x, but how do I solve this problem involving a cube root?