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Topic: How would I do this net ionic?  (Read 3679 times)

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Offline a_huynh00

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How would I do this net ionic?
« on: April 29, 2009, 10:06:05 PM »
A solution of potassium dichromate is added to lead (II) nitrate in an acidic solution.


I know it's a redox problem and I got

14H^+ + Cr2o7^2- + 3Pb^2+ ==> 3Pb^3+ + 2Cr^3+ + 7H2O

or is it

14H^+ + Cr2o7^2- + 6Pb^2+ ==> 6Pb^3+ + 2Cr^3+ + 7H2O
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Offline UG

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Re: How would I do this net ionic?
« Reply #1 on: April 30, 2009, 12:06:37 AM »
The latter one because the charges are balanced.
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Offline Borek

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Re: How would I do this net ionic?
« Reply #2 on: April 30, 2009, 04:57:57 AM »
I have never heard about Pb3+, as far as I can tell lead is stable as either Pb2+ or Pb4+. So neither of these reactions can be correct.

Also you don't take into account low solubility of PbCrO4. Could be in low pH lead gets oxidized to Pb4+ and there is no precipitate, but it won't hurt to consult equilibrium constants to be sure.
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