<p>This is called supercooling. I’ll use (pure) water as an example.</p>
<p>Crystals of ice take some time to form, so if water is cooled fast enough, the water can remain a liquid past its normal freezing point before ice crystals begin to form. During this time, the temperature continues to drop as energy continues to be released. Then when ice crystals finally begin forming, the temperature rises slightly and then plateaus since the phase change from liquid to solid requires energy to complete.</p>
<p>Usually a curve like that shows up with negative phase changes (gas -> liquid, liquid -> solid). This lowest dip area is the temperature (boiling pt. or freezing pt.) for the particular substance. The reason it goes up is that these downward phase changes are exothermic processes (hence why steam burns are worse than water scalds).</p>
<p>The reason both states coexist on that plateau as well is that, since the temperature is not dropping, apparently there are still molecules condensing or freezing (to negate the effects of the temperature drops, sort of like an equilibrium). Then, after all the molecules have changed states, the downward trend continues once more.</p>