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The boiling point is the temperature at which a liquid’s vapour pressure exceeds its atmospheric pressure. This is a property of all pure liquids.

Different substances have different vapor pressures, and therefore different boiling points. This is due to the intermolecular forces that are created between molecules as they evaporate, and by the difference in atom weights between individual molecules.

A boiling point is also affected by the presence of dissolved solutes. For example, salt water boils at a higher temperature than pure water at the same barometric pressure.

The same effect can occur when a mixture of liquids is mixed together. If the mixture has a liquid with a lower boiling point than the other liquid, the mixture will eventually separate into two (or more) layers.

Boiling points can be determined by either simple distillation or by using graphs based on the pressure and temperature of the liquid. These graphs, like the nomograph or Clausius-Clapeyron equation, use known values to create a curve.

Some substances, such as wood and calcium carbonate, do not have a boiling point at normal conditions but will sublime to gases when heated instead of changing into a liquid. Others, such as solid carbon dioxide, do not form a liquid when heated under standard conditions but will convert to gas when pressure is increased.