Online Exporter big recharged hot water bag for Brasilia Manufacturer

Online Exporter
 big recharged hot water bag for Brasilia Manufacturer

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Online Exporter
 big recharged hot water bag for Brasilia Manufacturer detail pictures

Online Exporter
 big recharged hot water bag for Brasilia Manufacturer detail pictures

Online Exporter
 big recharged hot water bag for Brasilia Manufacturer detail pictures

Online Exporter
 big recharged hot water bag for Brasilia Manufacturer detail pictures

Online Exporter
 big recharged hot water bag for Brasilia Manufacturer detail pictures

Online Exporter
 big recharged hot water bag for Brasilia Manufacturer detail pictures

Online Exporter
 big recharged hot water bag for Brasilia Manufacturer detail pictures

Online Exporter
 big recharged hot water bag for Brasilia Manufacturer detail pictures

Online Exporter
 big recharged hot water bag for Brasilia Manufacturer detail pictures

Online Exporter
 big recharged hot water bag for Brasilia Manufacturer detail pictures


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  • How to Make an Instant Cold Pack from Sodium Acetate.

    We’ve proven that crystallizing sodium acetate “hot ice” actually gets warmer: http://www.youtube.com/watch?v=CAwxhAP9mnc

    So the opposite should be true; if we dissolve it, it should get colder. We prove this in this video and show it cools down to about 9 Celsius in our experiments. This gives an “instant cold pack” effect very similar to the ones you find in store-bought instant cold packs. This is not as good as the store-bought packs, but it’s reusable.

    To make it, simply make the hot ice like our other videos here: http://www.youtube.com/watch?v=21IcpkxgBVY

    Crystallize the hot-ice and let the solid sodium acetate trihydrate cool down to room temperature. Then store it in an air-tight container.

    To initiate cooling, just add an equal amount of water.

    Special notes:

    You have to make the hot ice before you can make the cold pack. Using raw sodium acetate bought online won’t work because it’s dried out. Creating hot-ice introduces the right amount of water needed for this experiment.

    You also can’t let your freshly made hot ice dry out. Nor can you let it evaporate to make sodium acetate powder, it has to be hot ice for this to work.

    Why:
    Two competing effects occur during solvation. The exothermic effect of the water molecules interacting with the ions of sodium and acetate. And the endothermic effect of breaking up the interactions of ions. By using sodium acetate trihydrate at room temperature, you’ve already gotten rid of some of the exothermic interactions. But the endothermic ones remain. If you used anhydrous sodium acetate, the exothermic interactions roughly cancel out the endothermic ones.

    Thanks for watching

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