Calculate the molality of a sodium chloride brine solution that exhibits a density of 1.13 g / mL and a mass percent of 17.7% at room temperature. b. Calculate the freezing point of this sodium chloride brine solution mentioned in Part "a" above. c. Calculate the molarity of the same sodium chloride brine solution. (Part a). d. Calculate the mole fraction for water in a totally different sodium chloride solution (not Part a), if 20.0 g of this table salt (NaCl) was added to 93. mL of water to create a 100. mL of brine solution. The density of the pure water at this room temperature was accurately pre-determined to be 0.9986 g per mL. e. Calculate the vapor pressure of water above the brine solution mentioned in Part "d" above. f. Calculate a final molarity (M) for a solution if 10. mL of Part "d" is diluted to 0.20 L with pure water. 11 g. Discuss the miscibility of ethylene glycol in water using London dispersion, dipole-dipole, hydrogen bond interactions. In your discussion illustrate, with a drawing, each concept and the specific intermolecular interactions based on polarity, dipoles, and dipole moments. h. Draw the phase diagram for pure water. Be sure to define and briefly discuss the salient points, including, boiling point, melting point, sublimation point, critical point, etc. 12