Question
A pan full of hot salt water, NaCl(aq), is cooled and NaCl(s) precipitates. Explain why this happens.
Chloride ions are more strongly attracted to the metal in the pan than the sodium ions at low temperatures.
As the vapor pressure of the solution decreases the solubility of the salt goes down.
As the temperature decreases the solubility of the salt goes down and the salt in excess settles out as a precipitate.
As the temperature decreases the solubility of the salt goes up and the salt in excess dissolves.
Chloride ions are more strongly attracted to the metal in the pan than the sodium ions at low temperatures.
As the vapor pressure of the solution decreases the solubility of the salt goes down.
As the temperature decreases the solubility of the salt goes down and the salt in excess settles out as a precipitate.
As the temperature decreases the solubility of the salt goes up and the salt in excess dissolves.
Answers
is the answer Chloride ions are more strongly attracted to the metal in the pan than the sodium ions at low temperatures?
I think that's hogwash.
then is this the correct answer
As the temperature decreases the solubility of the salt goes down and the salt in excess settles out as a precipitate.
As the temperature decreases the solubility of the salt goes down and the salt in excess settles out as a precipitate.
That's much better, although the solubility of NaCl is not much higher at 100 C than it is at 0 C.
http://www.kentchemistry.com/links/Kinetics/SolubilityCurves.htm
http://www.kentchemistry.com/links/Kinetics/SolubilityCurves.htm