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    I need help getting the ionic equation for this:

    Lead Nitrate(V) + Sodium Chromate(VI) ---> Sodium Nitrate(V) + Lead Chromate(VI)

    Which is

    Pb(NO3)2 + Na2CrO4 ----> 2NaNO3 + PbCrO4

    :confused:
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    :bawling:
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    Bung some state symbols into there, split the ionic substances up into their constituent ions (whilst leaving anything else well alone), and see what happens.
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    Pb2+ (NO3-)2 + Na+2Cr04,2- ---> 2Na+NO3- + Pb2+CrO4,2-


    i think
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    Chromates (CrO42-) are usually insoluble. Exceptions include Na2CrO4, K2CrO4, (NH4)2CrO4, and MgCrO4.
    The Na+, K+, and NH4+ ions form soluble salts.
    The nitrate (NO3-) ion forms soluble salts

    Pb(NO3)2 [aq] + Na2CrO4 [aq] ----> 2NaNO3 [aq] + PbCrO4 [strike]
    Pb2+ [aq] + 2NO3- [aq] + 2Na+[aq] + CrO4 2-[aq] -----> 2Na+ [aq] + 2NO3-[aq] + PbCrO4[strike]

    Left with
    Pb2+ [aq] + CrO4 2-[aq] -----> PbCrO4[strike]


    You see I'm not sure if lead chromate is soluble. According to http://chemed.chem.purdue.edu/genche...18/soluble.php it isn't. If it was soluble, then everything would be (aq) and so all ions would cancel each other out and you would have no net ionic equation.
 
 
 
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