Answer:
The solubility of CuX is 1.425x10⁻⁷M
Explanation:
Given:
initial concentration of NaCN=0.2M
Ksp=1.27x10⁻³⁶
The reaction are:
CuX → Cu²⁺ + X²⁺, Ksp=1.27x10⁻³⁶
Cu²⁺ + 4CN⁻ → (Cu(CN)₄)²⁻, Kf=1x10²⁵
The overall reaction is:
CuX + 4CN⁻ → (Cu(CN)₄)²⁻ + X²⁺
The equilibrium constant is:
K=Ksp*Kf=1.27x10⁻³⁶*1x10²⁵=1.27x10⁻¹¹
CuX + 4CN⁻ → (Cu(CN)₄)²⁻ + X²⁺
I - 0.2 0 0
C - -4 +x +x
E - 0.2-4 x x
The equation for equilibrium is:
![K=\frac{[Cu(CN)4]^{2} [X]}{[CN]^{4} } \\1.27x10^{-11} =\frac{x^{2} }{(0.2-x)^{4} }](https://tex.z-dn.net/?f=K%3D%5Cfrac%7B%5BCu%28CN%294%5D%5E%7B2%7D%20%5BX%5D%7D%7B%5BCN%5D%5E%7B4%7D%20%7D%20%5C%5C1.27x10%5E%7B-11%7D%20%3D%5Cfrac%7Bx%5E%7B2%7D%20%7D%7B%280.2-x%29%5E%7B4%7D%20%7D)
Here, solving for x:
x=1.425x10⁻⁷M=CuX