EVALED® evaporators for wastewater treatment were first manufactured thirty-five years ago and were designed with a far-sighted intuition which proved that the acceleration of this phenomenon, through the use of package-modular standard units, would have represented a “clean system” to separate water from any pollutant component with a higher boiling temperature than water’s.
Evaporators for wastewater treatment exploit a natural phenomenon: evaporation.

Evaporation is the passage from the liquid to the gaseous state that only impacts the surface of the liquid. On the other end, if boiling temperature (different for each specific liquid and pressure connected) is exceeded, the constancy of the temperature and pressure parameters let the boiling process happen. Both processes fall under the name of vaporization.

To make the change of state, called evaporation latent heat, first heat (energy) needs to be provided. Quantity depends on the type of liquid and on its mass and temperature. For instance, the latent heat for one kilo of water at 373 K (100°C) is of about 2300kJ (550 kcal, 640 Wh) at atmospheric pressure (about 100 kPa).

The same heat quantity is released by water during the vapor phase, when condensation phenomenon occurs.

It is the temperature point where vapor pressure reaches the external pressure value (fixed), vaporization therefore occurs in a tumultuous way (boiling) that not only impacts the surface of the liquid, but its entire mass.

Boiling temperature point depends on the liquid type and varies according to pressure. Water boiling point occurs at 373 K (100°C) with an atmospheric pressure of about 100 kPa. But at high altitudes, on top of the mountains for instance, where pressure value is lower than the sea level, water boils with a lower temperature. When pressure is definitely low (vacuum) and equal to about 4 kPa (40 mbar), boiling temperature is reached at 302 K (29°C).

Different liquids have different boiling points: ethyl alcohol, for instance, has a boiling point equal to 351.4 K (78.4 °C) at 75kPa (760 mbar).

In case of saline solutions, boiling temperature, operating at a constant pressure, changes according to the presence of salts and their concentration. Ebullioscopic elevation is therefore the boiling temperature difference between water and a solution with a fixed concentration of salts. For instance boiling temperature of a solution of NaCl at 35% w/w in water at the atmospheric pressure level will show a 10 K (at 37 ° C) increase in boiling temperature.