Boiling point
The boiling point of a substance is the temperature at which the substance boils, or enters a state of rapid evaporation. For pure water this is 100° Celsius or 212° Fahrenheit, at standard pressure. Standard pressure is 1.0 Atmosphere (unit)
Boiling points can be changed in several ways. The addition of solutes or other substances usually changes the boiling point. Additionally, changing the pressure on a liquid changes its boiling point.
The boiling point of a liquid depends on the pressure of the surrounding air. An increase in air pressure raises the boiling point; a decrease in air pressure lowers the boiling point. In the low pressure environment at the top of Mt Everest for example, water boils at only 69 °C. (156.2 °F). Aquanauts find that water in their habitat only boils at high pressure.
Boiling point can also be defined in terms of vapour pressure as the temperature at which vapour pressure of liquid becomes equal to atmospheric pressure
Sugar, salt or other non-volatile solutes in water will usually make the boiling point higher. Alcohol, in contrast, is a volatile chemical that lowers the boiling point of water. Even a large amount dissolved in the water will usually make only small changes in the boiling point.
Boiling Point Media
Water boiling at 99.3 °C (210.8 °F) at 215 m (705 ft) elevation
Demonstration of the lower boiling point of water at lower pressure, achieved by using a vacuum pump.
A log-lin vapor pressure chart for various liquids
Boiling points of alkanes, alkenes, ethers, halogenoalkanes, aldehydes, ketones, alcohols and carboxylic acids as a function of molar mass
Ball and stick model of the butane molecule.
Ball and stick model of the isobutane molecule.
Ball and stick model of the pentane molecule.
- IsopentaneDballs
- NeopentaneDballs
Binary boiling point diagram of two hypothetical only weakly interacting components without an azeotrope
