A 1.0 L solution contains 3.00×10-4 M Cu(NO3)2 and 1.63×10-3 M ethylenediamine (en). The Kf for Cu(en)22+ is 1.00×1020. What is the concentration of Cu2+(aq ) in the solution?
Cu+2 + 2EN --> Cu(EN)2+2
Kf = [Cu(EN)2+2] / [Cu+2][EN]^2
Kd= 1/Kf = 1/(10^20) = 10^-20
Kd = [Cu+2][EN]^2 / [Cu(EN)2+2]
initially
[Cu+2] = 0
[EN] = 0
[Cu(EN)2] = assume 100% 3*10^-4 --> 3*10^-4
in equilibrium
[Cu+2] = 0 + x
[EN] = 0 +2x
[Cu(EN)2] = 3*10^-4 - x
substitute
Kd = [Cu+2][EN]^2 / [Cu(EN)2+2]
10^-20 = (x)(2X)^2 /(3*10^-4 - x)
since x <<< 3*10^-3, thn 3*10^-4 - x = 3*10^-4
10^-20 = (x)(2X)^2 /(3*10^-4)
(10^-20) * (3*10^-4) = 4*x^3
(((10^-20) * (3*10^-4)) /4 )^(1/3) = x
9.0856*10^-9 = x
then
[Cu+2] = x = 9.0856*10^-9M
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