Supersaturated Solutions (Sodium Acetate) - Data Error?

Question

The situation is that right now, at least in my mind, there is a major logical fallacy in my results for a lab experiment, dealing with the supersaturation and crystallization of Sodium Acetate.
For the first step, I poured a certain amount of Sodium Acetate (we used "crystals" as units) into 5 mL of tap water. The result was an increase of temperature (not recorded) and an unsaturated solution.

For the second step, we added a spoonful of Sodium Acetate, resulting in a cooler, saturated solution.

Now, my main question is, why was there an increase in temperature in the first step, yet there was a decrease in temperature in the second step? Does it have something to do with the saturation of the solution?

A response ASAP will be GREATLY appreciated. Thanks.

Answer 1

The salt was hydrated and released energy, putting in more served to increase its concentration and thus it re associated.