The freezing point of an aqueous solution that contains a nonelectrolyte is –9.0°C. a. What is the freezing-point depression of the solution?
b. What is the molal concentration of the solution?

Explanation:

The first thing to do here is use the freezing point of the solution to calculate the freezing-point depression, ΔTf.

As you know, the freezing-point depression is a measure of how low the freezing point of a solution is compared with the freezing point of the pure solvent.

You're dealing with an aqueous solution, so right from the start you know that the solvent is water. Pure water freezes at 0∘C under

aquifers are bounded above and below by impermeable rock. the driving force of groundwater movement in confined aquifers is pressure, rather than gravity.

fe 55.85 g/mol and h2o 18.02 g/mol.