Why does a solution have an elevated boiling point and a depressed freezing poitn compared with the pure?
Because when you have a chemical entity added to pure water–or pure solvent–you are changing the internal chemistry. The molecules of water behave differently in the presence of a solute than they would in just pure water. Think sea ice, freezing at a different temperature than pure water, because there’s salt in the seawater. Industrial chemists can calculate (with the help of computers and statistics) an approximate way in which various amounts of solute will change the chemistry reactions going on inside a particular solution. Another factor that an industrial chemist will consider is the order of mixing. Pure water to which salt is added, allowed to come to equilibrium, and then to which sugar is added will behave differently and have different properties than pure water to which sugar is added, allowed to come to equilibrium, and then to which salt is added. That’s true, even though the amounts of water, salt, and sugar are the same; so are the room temperature, material (glass,
