<p>What is the reason that a solute decrease the freezing point of a solution? Please explain in terms of intermolecular forces please.</p>
<p>Something to do with the greater energy require to be break bonds of solution than solvent?</p>
<p>You can find your answer here: [Freezing-point</a> depression - Wikipedia, the free encyclopedia](<a href=“http://en.wikipedia.org/wiki/Freezing-point_depression]Freezing-point”>Freezing-point depression - Wikipedia)</p>
<p>Excerpt:</p>
<p>“The freezing point depression is a colligative property, which means that it is dependent on the presence of dissolved particles and their number, but not their identity. It is an effect of the dilution of the solvent in the presence of a solute. It is a phenomenon that happens for all solutes in all solutions, even in ideal solutions, and does not depend on any specific solute-solvent interactions. The freezing point depression happens both when the solute is an electrolyte, such as various salts, and a nonelectrolyte. In thermodynamic terms, the origin of the freezing point depression is entropic and is most easily explained in terms of the chemical potential of the solvent.”</p>
<p>Yeah I read that before. Does that mean because there’s less conecetration that it’s more difficult for them to form a crystal structure?</p>
<p>Ok, if you read the second paragraph under explanation that should help.</p>
<p>Basically, at the freezing point, both the solid and liquid (the pure liquid) have the same amount of energy. Since most solutes only dissolve in the liquid, the liquid’s energy (but not the solid’s) energy will change. This causes a change in the freezing point, which you can see on the graph to the right.</p>
<p>Sorry if that didn’t make any sense, my class just started on intermolecular forces : )</p>
<p>But try re-reading that second paragraph, and I think it’ll start making sense for you.</p>
<p>Thanks so much!</p>