[CHM 112] Pre-Lab: Freezing Point Depression

[Andrew J. Pounds]

Here is some help for those of you that have not yet successfully 
complete the freezing point depression prelab...

Remember,

$\Delta T = k_f m$  where m is the molality (moles of solute divided by 
the kilograms of solvent).

$\frac{(\Delta T )(\mathrm{kg\  \ of\ \  solvent})}{k_f} = 
\mathrm{moles\ of\ solute}$

Once you calculate the moles of solute use that value and the mass of 
solute to determine the molar mass of the solute.


On 06/28/13 13:22, wrote:
> Okay, thank you so much!
>
>
>
>
>
> On Jun 28, 2013, at 1:22 PM, "Andrew J. Pounds" <pounds_aj at mercer.edu 
> <mailto:pounds_aj at mercer.edu>> wrote:
>
>> Let me get to computer where I can log into BlackBoard and I'll see 
>> what you have already done.
>>
>>
>> On 06/28/13 13:18,  wrote:
>>> Dr. Pounds,
>>>    I have tried multiple times on this pre-lab and on the question 
>>> that's asking for the molar mass of the solute, I can't seem to get 
>>> right. I'm using the formal you gave us at the end of class and I'm 
>>> doing something wrong. Could you explain the steps so I can see 
>>> where I'm getting it wrong in my calculations?
>>>
>>> Thank You,
>>>
>>
>>
>> -- 
>> Andrew J. Pounds, Ph.D.  (pounds_aj at mercer.edu 
>> <mailto:pounds_aj at mercer.edu>)
>> Professor of Chemistry and Computer Science
>> Mercer University,  Macon, GA 31207   (478) 301-5627
>> http://faculty.mercer.edu/pounds_aj
>>
>>


-- 
Andrew J. Pounds, Ph.D.  (pounds_aj at mercer.edu)
Professor of Chemistry and Computer Science
Mercer University,  Macon, GA 31207   (478) 301-5627
http://faculty.mercer.edu/pounds_aj

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