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chemnoob
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I'm wondering what happens in a single displacement reaction if the displacing metal (the one that's going into the solution) reaches it's solubility limit before the other metal in the solution is fully displaced.
Say for example you had a strong silver nitrate solution, and you placed enough solid lead in it to potentially displace all of the silver.
Pb + 2AgNO3 -> 2Ag + Pb(NO3)2
Since AgNO3 has approx four times more solubility than Pb(NO3)2, it is possible that the Pb(NO3)2 would reach it's solubility limit before all of the Ag is displaced. So when this happens does the displacement just stop (or drastically slow), or does the reaction continue, with the excess Pb(NO3)2 precipitating out?
Say for example you had a strong silver nitrate solution, and you placed enough solid lead in it to potentially displace all of the silver.
Pb + 2AgNO3 -> 2Ag + Pb(NO3)2
Since AgNO3 has approx four times more solubility than Pb(NO3)2, it is possible that the Pb(NO3)2 would reach it's solubility limit before all of the Ag is displaced. So when this happens does the displacement just stop (or drastically slow), or does the reaction continue, with the excess Pb(NO3)2 precipitating out?
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