A student determines the molar mass of acetone, \(\mathrm{CH}_{3}
\mathrm{COCH}_{3}\), by the method used in this experiment. She found that the
equilibrium temperature of a mixture of ice and water was \(1.0^{\circ}
\mathrm{C}\) on her thermometer. When she added \(11.1 \mathrm{g}\) of her sample
to the mixture, the temperature, after thorough stirring, fell to
\(-3.0^{\circ} \mathrm{C} .\) She then poured off the solution through a screen
into a beaker. The mass of the solution was 90.4 g.
a. What was the freezing point depression?
\(^{\circ} \mathrm{C}\)___________.
b. What was the molality of the acetone?
m____________.
c. How much acetone was in the decanted solution?
g_____.
d. How much water was in the decanted solution?
g_____.
e. How much acetone would there be in a solution containing \(1 \mathrm{kg}\) of
water and acetone at the same concentration as she had in her experiment?
\(g\) acetone____________.
f. What did she find to be the molar mass of acetone, assuming she made the
calculation properly?
g_____.
