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

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Jusaquikie
 4 years ago
Best ResponseYou've already chosen the best response.0i 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

Jusaquikie
 4 years ago
Best ResponseYou've already chosen the best response.0The 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)

aaronq
 4 years ago
Best ResponseYou've already chosen the best response.1NaCH3COO 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

Jusaquikie
 4 years ago
Best ResponseYou've already chosen the best response.0ok on the soulubility chart provided exceptions are Br Cl I and (SO4)2

Jusaquikie
 4 years ago
Best ResponseYou've already chosen the best response.0does that mean PbBr would be insouluble so that would be a precpitate?

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

aaronq
 4 years ago
Best ResponseYou've already chosen the best response.1so yeah, only the third one would not cause a precipitate

Jusaquikie
 4 years ago
Best ResponseYou've already chosen the best response.0and (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.

Jusaquikie
 4 years ago
Best ResponseYou've already chosen the best response.0so all but the NaCH3COO

aaronq
 4 years ago
Best ResponseYou've already chosen the best response.1yeah, 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

Jusaquikie
 4 years ago
Best ResponseYou've already chosen the best response.0Thank 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

aaronq
 4 years ago
Best ResponseYou've already chosen the best response.1no problem man, i have those next week also. good luck with your final !
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