Calculate the aqueous molar solubility of copper (II) hydroxide (Ksp=4.8X10^-20)

Question

Calculate the aqueous molar solubility of copper (II) hydroxide (Ksp=4.8X10^-20) ADJUSTED to (not mixed with) .010M sodium cyanide, given that cyanide complexes Cu2+ to form Cu(CN)4^2+ with a formation constant of 1.0x10^25. Calculate the aqueous molar solubility of copper (II) hydroxide (Ksp=4.8X10^-20) ADJUSTED to (not mixed with) .010M sodium cyanide, given that cyanide complexes Cu2+ to form Cu(CN)4^2+ with a formation constant of 1.0x10^25. Calculate the aqueous molar solubility of copper (II) hydroxide (Ksp=4.8X10^-20) ADJUSTED to (not mixed with) .010M sodium cyanide, given that cyanide complexes Cu2+ to form Cu(CN)4^2+ with a formation constant of 1.0x10^25.

Explanation / Answer

Cu(OH)2 --> Cu2+ + 2 OH-

Cu(OH) --> (S - x) + 2 S

Cu2+ + 4 CN- --> Cu(CN)42-

S - x + (0.01 - 4 x) --> x

Formation constant = [Cu(CN)42- ] / ([CN-]4 * [Cu2+]) = x / {(S - x) (0.01 - 4 x)4} = 1025 >>1

Ksp = (S - x) * 4 S2= 4.8 x 10-20

Solving for S and x simultaneously we get,

S = 0.00235 M

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