A solution of Na2CO3 is added dropwise to a solution that contains 1.00×10-2 M Fe2+ and 1.49×10-2 M Cd2+. What concentration of CO32- is need to initiate precipitation? Neglect any volume changes during the addition.
Ksp value: FeCO3: 2.10*10-11
Ksp value: CdCO3: 1.80*10-14
Which cation precipitates first?
What is the concentration of CO32- when the second cation begins to precipitate?
CdCO3(s) <=> Cd2+(aq) + CO32-(aq)
Ksp = [Cd2+][CO32-] = 1.80 x 10-14
[Cd2+] = 1.49 × 10-2 M
1.49 × 10-2 x [CO32-] = 1.80 x 10-14
[CO32-] = 1.21 x 10-12 M
FeCO3(s) <=> Fe2+(aq) + CO32-(aq)
Ksp = [Fe2+][CO32-] = 2.10 x 10-11
[Fe2+] = 1.00 × 10-2 M
1.00 × 10-2 x [CO32-] = 2.10 x 10-11
[CO32-] = 2.10 x 10-9 M
Precipitation occurs when ionic product Qsp >= Ksp
Thus [CO32-] = 1.21 x 10-12 M is needed to initiate precipitation and Cd2+ precipitates out first.
When second cation Fe2+ starts to precipitate, [CO32-] = 2.10 x 10-9 M.
A solution of Na2CO3 is added dropwise to a solution that contains 1.00×10-2 M Fe2+ and...
A solution of Na2CO3 is added dropwise to a solution that contains 1.21×10−2M Fe2+ and 1.48×10−2M Cd2+ . What concentration of CO32− is need to initiate precipitation? Neglect any volume changes during the addition. Express your answer with the appropriate units. The solubility-product constants, Ksp , at 25 ∘C for two compounds [iron(II) carbonate, FeCO3 , and cadmium(II) carbonate, CdCO3 ] are given by the table Substance Ksp FeCO3 2.10×10−11 CdCO3 1.80× 10−14
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