Given that the freezing point depression constant for water is 1.86 C kg/mol, how do you calculate the change in freezing point for a 0.833m sugar solution?

1 Answer
anor277
Jul 16, 2018

Is not freezing point depression simply the product....

Explanation:

#"Freezing point depression"=k_fxx"molality of solution"#

...where #k_f=underbrace(1.86*K*kg*mol^-1)_"molal freezing point depression constant"#

And so the observed molal freezing point depression is...

#1.86*K*kg*mol^-1xx0.833*mol*kg^-1=+1.55*K#..

But this is a freezing point depression, and so the fusion point of the solution should be #-1.55# #""^@C#...

How would the freezing point evolve if we had a solute that underwent speciation in aqueous solution, i.e. say sodium acetate or sodium chloride?

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