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The formation constant of [M(CN)6]4– is 2.50 × 1017, where M is a generic metal. A 0.170-mole quantity of M(NO3)2 is added to a liter of 1.51 M NaCN solution. What is the concentration of M2 ions at equilibrium?

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The best way to work these is in a two step process. The first step is to assume the complex forms completely (and with a huge formation constant that is a good assumption) with the aid of an ICE chart. The second step is to start with those materials and see how much they will dissociate using a second ICE chart. As follows:
.......M^+2 + 6CN^- ==> M(CN)6^4-
I....0.170...1.51........0
C...-0.170..-6*0.170.....0.170
E....0.......0.49........0.170
=================================
......0......0.49........0.170....I
......x.....+6x...........-x......C
......x....0.49+6x.......0.170-x..E

Kf = 2.50E17 = [M(CN)6^4-]/(M^2+)(CN^-)^6
Substitute the last E line into Kf expression and solve for x.

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