The osmolality of urine, plasma and other solutions is often determined by cryoscopy, which determines the decrease in freezing temperature of water. The cryoscopic constant of water is 1.853 K-Kg/mol (for concentrations of solutes expressed in molality). A normal urine sample has a freezing point of -1.11'C. A urine sample from a patient has a freezing point of -2.05°C. Using that information, what would you conclude regarding the state of hydration of the patient? What is the approximate osmolality in normal urine and in the urine of the patient? What is the mole fraction of osmolytes in the urine samples?

Q: A solution is made by dissolving 6.60 grams of MgCl2 in 380.0 mL of water. What is the freezing…

A: Given, Mass of MgCl2 = 6.60 g  Volume of water = 380.0 mL  Density of water = 1.00 g/mL  Kf of water…

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A: The homogenous mixture of two or more substant is known as a solution.

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Solutions

Solutions can be considered as homogeneous mixtures which contain two or more than two chemical substances. The chemical substance which is the greater part is defined as solvent. And the chemical substance that is dissolved in a solvent is referred to as solute. Solution chemistry plays an important role in chemistry since it supports many commercial applications of solutions.