Free Essays on Colligative Properties Lab - Brainia.com.
The final colligative property is osmotic pressure. Osmosis is the process by which water flows from an area of high concentration to an area of low concentration. This property is a critical component of body fluids because it will determine how much water flows into or out of cells.
Experiment on Colligative properties Colligative properties are the properties of solutions that depend on the TOTAL concentration of solute particles in solution. The list of colligative properties includes: a) lowering vapor pressure above a solution; b) freezing temperature depression; c) boiling temperature elevation; d) osmotic pressure.
Experiment 1: Colligative Properties Determination of the Molar Mass of a Compound by Freezing Point Depression. Objective: The objective of this experiment is to determine the molar mass of an unknown solute by measuring the freezing point depression of a solution of this solute in a solvent as compared to the freezing point of the pure solvent.
This third category, known as colligative properties, can only be applied to solutions. By definition, one of the properties of a solution is a colligative property if it depends only on the ratio of the number of particles of solute and solvent in the solution, not the identity of the solute.
Start Virtual ChemLab, select Colligative Properties, and select Freezing Point Depression from the list of assignments. The lab will open in the Calorimetry laboratory with a beaker containing 45.00 g of ice and a coffee cup calorimeter on the lab bench.
Colligative properties depend on the number of particles present, not on the type of particles or their mass. Osmotic Pressure The osmotic pressure of a solution is the difference in pressure between the solution and the pure liquid solvent when the two are in equilibrium across a semi-permeable membrane, which allows the passage of solvent molecules but not of solute particles.
Overall, the colligative properties can be very useful in our everyday lives. The neat thing about them is that it doesn't matter what the solute is, just how much is there. For example, if you added the same number of moles of sugar and salt, the salt would have a greater effect than the sugar because it is ionic.