Try NaCl or glucose . If it can be solubilized it is likely it will depress the melting point of PEA.
A melting point is a characteristic physical property of a substance. So melting point analysis is one of the simplest and most useful techniques for identification of a chemical substance.
Melting Point Depression
Melting point analysis can also provide information about the purity of a sample. A substance (solid) containing soluble impurities usually melts at a lower temperature than the pure compound. It can also melt over a wide range of temperatures. This is called the “melting point depression”.
In general, the smaller the range of melting temperatures, the higher the purity of the sample.
Note that insoluble impurities will have no effect on a compound’s melting point.
Role of Intermolecular Forces
Most of the solids we encounter in the laboratory (organic or inorganic) are crystalline solids. These have molecules (for solids like caffeine) or repeating clusters of ions (for solids like CuSO4) arranged in a regular, tightly packed repeating crystal lattice.
The lattice is held together by various intermolecular forces, which come about because of the chemical nature of the solid.
These forces must be disrupted when a substance melts, which requires an input of energy. This in turn translates to an elevated temperature. So, the stronger the forces that hold together a solid, the higher its melting point.
How Impurities Affect Melting Point
It’s not difficult to understand how impurities affect the melting point. Foreign substances in a crystalline solid disrupt the repeating pattern of forces that holds the solid together. So a smaller amount of energy is required to melt the part of the solid surrounding the impurity.
This explains the melting point depression (lowering) observed from impure solids.
The more impure the solid is, the more the structure is disrupted and the greater the variation in intermolecular forces in different areas of the solid.
The Effect
The melting temperature is lowered compared to the pure solid, and the solid melts over a wider range of temperatures.
Pure 2-hydroxyethyl amides of the sort with which you are working can be partially dehydrated (azeotropic removal of water or heating under vacuum) creating a mixture of the starting amide and the 2-alkyl oxazolidine. As per earlier answer, this mixture should have a lower melting point. The oxazolidine can revert to the amide in the presence of water.
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