The molality of a solution can be determined using Equation $1$ if the boiling point elevation is measured and the boiling point constant $(K_b)$ of the solvent is known. The value of $K_b$ for water is $0\mathrm{.}512kg*\frac{K}{m}ol.$

$T=m0\mathrm{.}512kg*\frac{K}{m}ol$

molality $=\frac{T}{0\mathrm{.}512(kg)*\frac{K}{m}ol}$

$T=$ Boiling point of solution $-$ Boiling point of pure water

A solution was prepared by dissolving $12\mathrm{.}00g$ glucose in $100\mathrm{.}0g$ water. The resulting solution was found to have a boiling point of $100\mathrm{.}34C.$ Calculate the molar mass of glucose. Note: Glucose is a molecular solid that exists as discrete molecules in solution.

$2.$ Solution A contains $20g$ of sodium chloride, NaCl, dissolved in $200mL$ of water. Solution $B$ has $40g$ of sodium chloride dissolved in $200mL$ of water.

a$.$ Which solution will have the highest boiling point?

b$.50mL$ of Solution $A$ is placed in a section of semipermeable dialysis tubing and then sealed. The tube is placed in a beaker containing the $200mL$ of Solution B$.$ After a period of time, the boiling points of the solutions inside and outside the dialysis tube are determined.

How will the boiling point of each solution have changed from its original boiling point? Explain.

$3.$ The freezing point depression of a solution is dependent on the number of particles in solution, not the type of particles. If $0\mathrm{.}1$ moles of each of the following soluble ionic compounds, sodium phosphate, $N{a}_{3}P{O}_4,$ and sodium chloride, NaCl, are added to separate beakers containing $1L$ of distilled water, which would have the lower freezing point? Explain.