Saturated and Supersaturated Solutions
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Take a saturated solution, for example, let's use salt water. At room temperature, you totally saturate the solution. Then, you slowly heat the solution, and suddenly you can add more.
Does this make it a super saturated solution?
Also, once you take the solution back down to room temperature, will salt crystals reappear in the solution that was previously saturated at room temperature? To rephrase: will you see salt crystals at the bottom of the beaker?
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Solution Summary
The solution clearly explains the theory behind saturation in order to answer the questions of what makes a solution supersaturated and the effects of heat on solubility as well as the problem of predicting whether or not precipitate will reform.
Solution Preview
Suppose you have a saturated solution - a solution with a small amount of precipitate that has been heated just until all the precipitate is dissolved. That is now saturated.
Now as temperature drops, the solubility ...
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