Chemical Forums
Chemistry Forums for Students => Undergraduate General Chemistry Forum => Topic started by: meghan on February 27, 2010, 08:45:27 AM
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I'm not sure what the final step would be in the problem below. I have solved for :delta:T for freezing and boiling points already.
Q: Calculate the melting point of a 1.7 m solution of sodium chloride assuming 100% dissociation. For water kbp=0.512 degree C/m and kfp = 1.86 degree C/m.
I don't know how to get melting point. Is the difference between the change in freezing point and melting point? Here's what I did so far.
:delta:Tbp =kbpmsol particles
:delta:Tbp = .512 C/m x 1.70 m
:delta:Tbp = .870 C
:delta:Tfp =kfpmsol particles
:delta:Tfp = .1.86 C/m x 1.70 m
:delta:Tfp = 3.16 C
Thanks for your help.
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Q: Calculate the melting point of a 1.7 m solution of sodium chloride assuming 100% dissociation. For water kbp=0.512 degree C/m and kfp = 1.86 degree C/m.
I don't know how to get melting point. Is the difference between the change in freezing point and melting point? Here's what I did so far.
:delta: Tbp =kbpmsol particles
:delta: Tbp = .512 C/m x 1.70 m
:delta: Tbp = .870 C
:delta: Tfp =kfpmsol particles
:delta: Tfp = .1.86 C/m x 1.70 m
:delta: Tfp = 3.16 C
Thanks for your help.
You haven't considered dissociation of NaCl anywhere.
About the melting point thingy...
Hint : What is the solvent?
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Thank you for the guidance. I understand this now. ;D