Chemical Forums
Chemistry Forums for Students => Undergraduate General Chemistry Forum => Topic started by: Rutherford on March 27, 2014, 09:48:29 AM
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The melting point of cryolite (molar mass 210 g) is 1282.7K. However, by adding sodium fluoride cryolite is made to melt at 1233K. Calculate the percentage (on w/wbasis) of sodium fluoride needed to be added to reduce the melting point to 1233K assuming that it dissociates completely. The heat of fusion of cryolite in this temperature range is 114kJmol-1.
What equation should be used here?
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Sigh, I know the equation, but I have no idea what it is called nor how it is derived.
You need to calculate cryoscopic constant from Kf=RT2/L, where L is the heat of fusion (beware of units!). This is probably related to Van 't Hoof equation.
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Oh, you reminded me now. It should be:
ΔT=RTm2χs/ΔHf (Tm is the melting point of pure solvent, χs is the molar share of the solute).
I got that χ=41.4% while their answer is 4.14%. Can someone check this?
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I agree with χ = 41.4 mol%. By the way, that should be Tm2 in your equation.
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Corrected. Thanks.
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Good, but you still need to answer the question!
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I got that χ=41.4% while their answer is 4.14%.
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χ is the mole fraction of solute; they ask for the weight % of NaF.
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Why is their answer 4.14% then? The w/w share won't have this value.