if .700 g of thyroxine is dissolved in 9.5g benzene, the freezing point of the s
ID: 874448 • Letter: I
Question
if .700 g of thyroxine is dissolved in 9.5g benzene, the freezing point of the solution is 5.184*C. Pure benzene freezes at 5.444*C and has a Kf 5.12*C/mol. What is the molar mass of thyroxine? Please work out the problem step by step I would really like to understand. Thank you!!if .700 g of thyroxine is dissolved in 9.5g benzene, the freezing point of the solution is 5.184*C. Pure benzene freezes at 5.444*C and has a Kf 5.12*C/mol. What is the molar mass of thyroxine? Please work out the problem step by step I would really like to understand. Thank you!!
Explanation / Answer
The freezing point depression dTf is directly proportional to the molality m of the solute.
dTf=Tf(solvent)?Tf(solution)= m
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