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The boiling point of a substance is the temperature at which the liquid phase of a compound changes into a vapor. This occurs when the vapor pressure of the liquid is equal to the atmospheric pressure around it.
Water reaches the normal boiling point at 100 degrees centigrade, a temperature that is equivalent to standard atmospheric pressure on Earth. Different substances have different boiling points.
Boiling points of pure compounds are dependent on the vapor pressure and volatility of the liquid. If the liquid contains dissolved impurities (solutes) or other miscible compounds, the solutes lower the vapor pressure of the liquid, and the normal boiling point is raised in proportion to the concentration of the solutes.
The boiling point of a substance can also be changed by changing the surrounding environment’s pressure. This is especially true for liquids at higher elevations where the atmospheric pressure is lower than at sea level.
Chemical structure has a big influence on boiling points, since molecules that are tightly bound together have stronger intramolecular forces than molecules with a looser bonding. For example, ethanol has a higher normal boiling point than acetone due to the OH structure in ethanol that makes it harder for molecules to leave the liquid state.
However, molecular weight has a relatively minor effect on the normal boiling point of a substance. For example, ethanol has a lower molecular weight than butane, but it has a higher normal boiling point than a mixture of butane and propane because the molecules are closer together in the ethanol.