Background: I was recently playing around with some reusable heat packs, the kind that operate by phase change of sodium acetate trihydrate and noticed that they didn't reach the temperature that I had expected (58 °C) rather, they stayed at 52 °C.

There were two such packs, roughly 50 mm × 100 mm × 15 mm and placed together with the broad sides in contact. Between them and at the center, there was a calibrated PT-100 RTD (which I certainly trust to be better than 1 °C accurate). The entire mass was then insulated with a few layers of thick wool fabric. The temperature reading became constant at 52 °C within a few minutes of crystallization being initiated in both packs and remained very stable for more than 10 minutes thereafter.

It's worth noting that although the manufacturer labeled the contents as being 'Sodium acetate (food grade)' and water, no proportions are given. Also, the contents of the pack are bright red, indicating the presences of unlisted dyes.

Question: What would be the most likely causes for the discrepancy? Contaminants, incorrect, proportions something else?

I'm ultimately interested in using this reaction to maintain ~58 °C in an experiment. I'd like to avoid the same result if I mix up a batch of this stuff from pure ingredients.

  • $\begingroup$ Its previous environment might be to blame. But, was this a case of contamination? Perhaps not! What conditions could lead to this backward data? Results generate more questions-some which can only be answered by the seller-and, perhaps a few things were used as "replacements", and in combining, the results attached you to this mystery. Keep us updated! $\endgroup$
    – user20735
    Commented Sep 8, 2015 at 21:17
  • $\begingroup$ I'd guess that there was something besides sodium acetate in the packs. If there was just sodium acetate then the pack would become a rock when in the solid state. So there is probably extra water with NaCl so that the pack still stays somewhat squishy when the solid acetate forms. $\endgroup$
    – MaxW
    Commented Nov 7, 2015 at 23:01

1 Answer 1


My assumption is that the addition of water (other than water of hydration) lowers the temperature - consider that the heat of crystallization is shared among the sodium acetate, the added water and even the packaging. Perhaps the manufacturer adds water to lessen the chance of burns.

You'd need to experiment with lab-grade chemicals to be sure, such as this ~99% pure sodium acetate trihydrate.


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