Compare the solvents listed in Table $1.$ If each were mixed with a solute so that a solution was prepared that had $1m(1$ molality$),$ which solvent would experience the smallest change in freezing point?

The solvent with the smallest $KF$ will experience the smalle $f$ change in freezing point.

A$.$ How many grams of sucrose $)=(342\mathrm{.}3\frac{g}{m}ol$ are needed to prepare a $1\mathrm{.}5$ molality aqueous solution with $500.g$ of water?

B$.$ Calculate the theoretical boiling point of this solution.

In a freezing point experiment using lauric acid as a solvent the following values were obtained: $T_f($lauric acid$)=43\mathrm{.}2C$

$T_f($with $0\mathrm{.}75g$ of solute in $4\mathrm{.}00g$ of lauric acid$)=40\mathrm{.}6C$

Use this data to calculate the molecular mass of the solute. $($Lauric acid: $K_f=3\mathrm{.}9C*k\frac{g}{m}ol).$ Note that this solute is a nonelectrolyte.

$4.$ A$.$ Calculate the expected vapor pressure for a solution prepared from $82\mathrm{.}0g$ of tartaric acid $)=(150\mathrm{.}7\frac{g}{m}ol$ and $125g$ of water at $20\mathrm{.}0C.$ VP pure water at $20\mathrm{.}0C$ is $17\mathrm{.}5$ torr. $(*$ this compound is a weak electrolyte. In this calculation, please treat it as a nonelectrolyte$)$

B$.$ Because tartaric acid is a weak electrolyte, how would the true vapor pressure of the solution described above deviate from the vapor pressure of the solution when we assumed $i=1?($circle your answer$)$

Actual VP: higher same lower than calculated VP$.$

$7$