Chemical Forums
Chemistry Forums for Students => Analytical Chemistry Forum => Topic started by: AllHallows20 on February 20, 2012, 03:52:54 PM
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This is the question I'm trying to answer:
If a 0.100 M solution of NaOH is added to a solution containing 0.200 M Ni2+, 0.200 M Ce3+, and 0.200 M Cu2+, which metal hydroxide will precipitate first? Ksp for Ni(OH)2 = 6.0 X 10-16, Ksp for Ce(OH)3 = 6.0 X 10 -22, and Ksp for Cu(OH)2 = 4.8 x 10-20.
I know to first calculate when each of the metals will precipitate but I can't seem to get that to work out correctly
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Calculate - for each metal separately - concentration of OH- needed for precipitation.
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I'm attempting that but I'm pretty sure I'm doing it wrong, I used the formula ksp=[2.00M][1.00x]^2 for Ni and cu and to the 3rd power for ce
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You are doing strange things.
Write Ksp formula for Ni(OH)2.
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6.0X10^-16=[Ni][OH]^2
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OK, what is Ni2+ concentration?
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.200 M
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So, what is OH- concentration needed for precipitation?
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.200 M?
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no wait would it be .4M
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Why do you guess instead of calculating? Plug Ni2+ concentration into the formula and solve for the only unknown - [OH-]. Basic algebra.
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oh jeeze, thanks I have no idea how I made things so much more complicated than they had to be.