Question

1) We have assumed that the unknown does not dissociate into more than one particle when

dissolved. If this was an incorrect assumption and the solid did dissociate slightly. Then how

would the calculated molar mass of solute from our experiment differ from the actual molar mass?

The calculated would be (too high, too low or unaffected) compared to the actual? Explain briefly.

2)If you measured the experimental freezing point of 30g cyclohexane with 0.012mols of Toluene

(MWT= 92.15) and compared it to a measurement of 30g cyclohexane with 0.012mols

benzophenone (MWT = 182.22). What would you expected to observe about the two separate

freezing points? Explain Briefly

3) Why is cyclohexane used as a solvent in this experiment instead of water? Water is much safer

and much cheaper.

Answer 1