Equal numbers of moles of two soluble, substances, substance $\mathrm{A}$ and substance $\mathrm{B}$, are placed into separate $1.0-\mathrm{L}$ samples of water.
a. The water samples are cooled. Sample A freezes at $-0.50^{\circ} \mathrm{C}$, and Sample $\mathrm{B}$ freezes at $-1.00^{\circ} \mathrm{C}$. Explain how the solutions can have different freezing points.
b. You pour $500 \mathrm{~mL}$ of the solution containing substance $\mathrm{B}$ into a different beaker. How would the freezing point of this $500-\mathrm{mL}$ portion of solution $\mathrm{B}$ compare to the freezing point of the $1.0-\mathrm{L}$ sample of solution $\mathrm{A}$ ?
c. Calculate the molality of the solutions of $\mathrm{A}$ and $\mathrm{B}$. Assume that $i=1$ for substance $\mathrm{A}$.
d. If you were to add an additional $1.0 \mathrm{~kg}$ of water to solution B, what would be the new freezing point of the solution? Try to write an answer to this question without using a mathematical formula.
e. What concentration (molality) of substances $\mathrm{A}$ and $\mathrm{B}$ would result in both solutions having a freezing point of $-0.25^{\circ} \mathrm{C}$ ?
f. Compare the boiling points, vapor pressure, and osmotic pressure of the original solutions of $\mathrm{A}$ and $\mathrm{B}$. Don't perform the calculations; just state which is the greater in each case.