Effects of Concentration on Colligative Properties PDF

Effects of Concentration on the Colligative Properties of Colligative properties of solutions are properties that depend upon the concentration of solute molecules or ions, but not upon the identity Colligative properties include vapor pressure lowering, boiling point elevation, fr...

Effects of Concentration on the Colligative Properties of Colligative properties of solutions are properties that depend upon the concentration of solute molecules or ions, but not upon the identity Colligative properties include vapor pressure lowering, boiling point elevation, freezing point depression, and osmotic pressure. Lowering the Vapor Pressure Vapor pressure is the pressure of a vapor in thermodynamic equilibrium with its condensed phase in a closed container. When a non-volatile solute is dissolved in a solvent, the vapor pressure of the solvent is Boiling Point Elevation The boiling point of a liquid is defined as the temperature at which the vapor pressure of that liquid equals the Freezing Point Depression Normal freezing or melting point is the temperature at which solid and liquid are in equilibrium under 1 atm. The addition of solute will decrease the vapor pressure and so will decrease the freezing point. Osmotic Pressure This is the external pressure that must be applied to the solution in order to prevent it from being diluted by the entry of solvent via osmosis. Osmosis is the movement of solvent particles across a semipermeable membrane from a Osmotic pressure is directly proportional to the concentration of the solution. Therefore, doubling the concentration will also  Difference Between the Colligative Properties of Electrolyte and Electrolytes are substances that can form solutions that are able to conduct electricity through this solution. Such solutions are known as electrolytic solutions. Nonelectrolytes are An electrolyte solution is a solution that generally contains ions, atoms or molecules that have lost or gained electrons, and is electrically conductive. For this reason they are often called ionic solutions, Nonelectrolyte solutions do not conduct electricity. Examples include solutions of nonpolar gases (H2, noble gases, CH4, gaseous hydrocarbons, SF6, air), nonpolar organic compounds (liquid and solid When an electrolyte is dissolved in a solvent such as water, the electrolyte separates into ions (or any other conductive species). Therefore, dissolving one When a nonvolatile (does not turn to vapor easily) solute is added to a liquid to form a solution, the vapor pressure above  Boiling Point Elevation and Freezing Point Depression The boiling point of a liquid is defined as the temperature at which the vapor pressure of the liquid is equal to the prevailing atmospheric pressure. Boiling points measured under 1 atm Since a non-volatile solute decreases the vapor pressure of a liquid, a solution will not boil at normal boiling point of the solvent at 1 atm pressure. It is necessary to increase the temperature above this point in order to attain a vapor pressure Freezing Point Depression The freezing point is the temperature at which the liquid changes to a solid. At a given temperature, if a substance is added to a solvent (such as water), the solute-solvent interactions prevent the solvent from going into the solid phase. The solute-solvent interactions require the temperature to decrease further in A common example is found when salt is put on icy roadways. The salt is put on the roads so that the water on the roads will not freeze at the normal 0°C but at a lower temperature The freezing point depression is the difference in the freezing points of the solution from the pure solvent. This is true for any solute added to a solvent; the freezing point of the solution will be lower than