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how many of these solutions could be used to precipitate Pb2+ ion from .2 M solution of lead nitrate
 one year ago
 one year ago
how many of these solutions could be used to precipitate Pb2+ ion from .2 M solution of lead nitrate
 one year ago
 one year ago

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JusaquikieBest ResponseYou've already chosen the best response.0
i think they would break down as follows Lead Nitrate Pb2+ 2(NO3) KCl = K+ Cl KOH = K+ (OH) NaCH3COO = guessing Na+ CH3 COO CaBr2 = Ca^2+ Br
 one year ago

JusaquikieBest ResponseYou've already chosen the best response.0
The answer is 3 but i don't know how to figure this out. I would have guessed 1 because CaBr2 is the only 2Br to strip away the2 (NO3)
 one year ago

aaronqBest ResponseYou've already chosen the best response.1
NaCH3COO would dissociate in to Na+ and CH3COO (which is the conjugate base of acetic acid) you're finding out which solution would precipitate Pb^2+ out so look at solubility tables, i'm pretty sure Pb(OH)2 is insoluble maybe PbBr2
 one year ago

JusaquikieBest ResponseYou've already chosen the best response.0
ok on the soulubility chart provided exceptions are Br Cl I and (SO4)2
 one year ago

JusaquikieBest ResponseYou've already chosen the best response.0
does that mean PbBr would be insouluble so that would be a precpitate?
 one year ago

aaronqBest ResponseYou've already chosen the best response.1
PbBr2 ..since Pb is 2+ and Cl is 1 .. balance out charges the chart i have says PbBr2, PbCl2 and Pb(OH)2 are insoluble
 one year ago

aaronqBest ResponseYou've already chosen the best response.1
so yeah, only the third one would not cause a precipitate
 one year ago

JusaquikieBest ResponseYou've already chosen the best response.0
and (OH) is insoulible with no exceptions for Pb so that would make 3 this makes sense now, i was trying to have Pb2+ left over after froming something witht the rest of the ions.
 one year ago

JusaquikieBest ResponseYou've already chosen the best response.0
so all but the NaCH3COO
 one year ago

aaronqBest ResponseYou've already chosen the best response.1
yeah, thats all you can do to show they will precipitate. if you were given more information (like the concentration of the other solutions) you could've shown they precipitate using their Ksp's
 one year ago

JusaquikieBest ResponseYou've already chosen the best response.0
Thank you again for your time i will be giving out medals all night lol i have my chem final in the morning =p Thank you
 one year ago

aaronqBest ResponseYou've already chosen the best response.1
no problem man, i have those next week also. good luck with your final !
 one year ago
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