Wanting to form nickel(II) cyanide, Ni(CN)2, a chemist adds hydrocyanic acid, HC

Question

Wanting to form nickel(II) cyanide, Ni(CN)2, a chemist adds hydrocyanic acid, HCN, to a solution containing Ni2+ ions hoping to precipitate Ni(CN)2. The important equlibria for this process are given below:
HCN(aq) <--> H+(aq) + CN-(aq) Ka=4.0x10^(-10)
Ni(CN)2(s) <--> Ni2+(aq) +2CN-(aq) Ksp= 3.0x1-^(-23)

a) what is the equilibrium constant, Knet, for the following reaction which describes the precipitation reaction the chemist wants to perform?
Ni2+(aq) + 2HCN(aq) <--> 2H+(aq) + Ni(CN)2(s)
Knet=?????

b) can the chemist readily form Nickel (II) Cyanide in this manner?
c) The chemist runs the reaction and allows the solution to come to equilibrium before diluting the solution by a factor of 10. Calculate Q upon dilution.

Explanation / Answer

cube root(Ksp x ka^2) =1.68x10-14 No.It cannot be Q = [ni cn 2][H]^2 /([ni][HCN]^2) turns to be 356.78x10-5

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