<P> A saturated liquid contains as much thermal energy as it can without boiling (or conversely a saturated vapor contains as little thermal energy as it can without condensing). </P> <P> Saturation temperature means boiling point . The saturation temperature is the temperature for a corresponding saturation pressure at which a liquid boils into its vapor phase . The liquid can be said to be saturated with thermal energy . Any addition of thermal energy results in a phase transition . </P> <P> If the pressure in a system remains constant (isobaric), a vapor at saturation temperature will begin to condense into its liquid phase as thermal energy (heat) is removed . Similarly, a liquid at saturation temperature and pressure will boil into its vapor phase as additional thermal energy is applied . </P> <P> The boiling point corresponds to the temperature at which the vapor pressure of the liquid equals the surrounding environmental pressure . Thus, the boiling point is dependent on the pressure . Boiling points may be published with respect to the NIST, USA standard pressure of 101.325 kPa (or 1 atm), or the IUPAC standard pressure of 100.000 kPa . At higher elevations, where the atmospheric pressure is much lower, the boiling point is also lower . The boiling point increases with increased pressure up to the critical point, where the gas and liquid properties become identical . The boiling point cannot be increased beyond the critical point . Likewise, the boiling point decreases with decreasing pressure until the triple point is reached . The boiling point cannot be reduced below the triple point . </P>

The boiling points for two compounds are given below