What is the freezing point of solution that has 185.25 grams of Ca(OH)2 (formula mass = 74.1) dissolved in 2,500 grams of water at standard pressure?

The freezing point depression ∆T = KF·m where KF is the molal freezing point depression constant and m is the molality of the solute. Rearrangement gives: mol solute = (m) x (kg solvent) where kg of solvent is the mass of the solvent (lauric acid) in the mixture. This gives the moles of the solute.

Explanation:

Does this help at all??

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