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Iron(II) nitrate and hydrocyanic acid react to form the hexacyanoferrate(II) ion, [Fe(CN)6] -4 (aq), with a...

Iron(II) nitrate and hydrocyanic acid react to form the hexacyanoferrate(II) ion, [Fe(CN)6] -4 (aq), with a formation constant of 1.438x1035 . This complex ion has an intense blue color in solution

. a. If you add 182.734g of iron(II) nitrate solid to 750.0mL of 0.8324M CN-1 (aq) solution, what is the concentration of CN-1 (aq) still in solution when the reaction reaches equilibrium?

b. Copper(II) also forms a complex ion with cyanide ions, tetracyanocuprate(II) ion, [Cu(CN)4] -2 (aq), with a formation constant of 1.028x1025 . This complex ion has an intense green color in solution. If 10.0mL of 0.500M Cu+2(aq) and 10.0mL of 0.500M Fe+2(aq) are both added to 500.0mL of 20.0mL of CN-1 (aq), explain what you would expect to see.

PLEASE WRITE SO I CAN READ IT. It does me no good if I cant read what you write. thanks!

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