If the freezing point of a solution always lower than that of the pure solvent or is it possible for it to end up being higher?

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    $\begingroup$ Depends on your definition of solution. Is $^2\ce{H2O}$ in $^1\ce{H2O}$ close enough? Because that's the only way I know to make a "solution" and have the FP go down. $\endgroup$ Feb 9, 2016 at 10:06
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    $\begingroup$ Of course not. Whether you're talking only about aqueous solutions or other ones. $\endgroup$
    – Mithoron
    Feb 9, 2016 at 12:06
  • $\begingroup$ Thanks. There's no way the freezing point could not change either is there? $\endgroup$ Feb 9, 2016 at 13:17
  • $\begingroup$ Whoops. Go up* sorry. $\endgroup$ Feb 9, 2016 at 13:50
  • $\begingroup$ Consider the enthalpic and entropic contributions in the small solute limit. Entropy will win, lowering the freezing point. $\endgroup$
    – Jon Custer
    Feb 9, 2016 at 15:17


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