In: Chemistry
What is the molar solubility of nickel(II) sulfide in 0.053 M KCN? For NiS, Ksp = 3.0
Ksp of NiS = 3.0 x 10^-19
Kf of Ni(CN)42- = 1.0 x 10^31
NiS (s) --------------> Ni2+ (aq) + S2- (aq)
Ni2+ (aq) + 4 CN- (aq) ------------> [Ni(CN)42-] (aq)
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NiS (s) + 4 CN- (aq) ------------> [Ni(CN)42-] (aq) + S2- (aq)
Keq = Kf x Ksp
= 1.0 x 10^31 x 3.0 x 10^-19
= 3.0 x 10^12
NiS (s) + 4 CN- (aq) ------------> [Ni(CN)42-] (aq) + S2- (aq)
0.053 M 0 0
0.053-4x x x
Keq = x^2 / (0.053 - 4x)^4
3.0 x 10^12 = x^2 / (0.053 - 4x)^4
1.732 x 10^6 = x / (0.053 - 4x)^2
1.732 x 10^6 = x / 16 x^2 + 0.002809 - 0.424 x
2.77x 10^7 x^2 + 4865.2 - 734368 x = x
x = 0.01297
molar solubility = 1.3 x 10^-2 M