So, I did a lab a few days ago and I was able to calculate the molar mass of antifreeze using the freezing point depression. It was a longish process and the very last question asked me to derive an equation that would find the molar mass of anything dissolved in water if given the freezing point depression and the mass of the solute. This is what I came up with and I think it is good, but I'm not sure if I could simplify it further:
Mass/ (.001∆Tmass)
___________
1.86
Anybody know if that is simplified to its fullest extent?
Ok...remember how on facebook chat a few months ago I told you that melting point depression (meltinp point = freezing point) was not dependent on the material itself, just the molar amount of the material? Well, this is what you will be showing.
dT = K*m*i where:
dT is the depression observed
K is the cryoscopic constant for the solvent
m is the molality of the material
i is the mizzl (van't Hoff factor really), which is an integer which represents the number of molecules per mole
so, using your original data, you can solve for K, which will remain constant as long as you stay in water.
You can now rearrange to:
dT/(K*i) = m
I have to go to the airport and then take someone to dinner. If you need further help, check your PMs.