Colligative Reviewer Chemistry (Universidad de Manila) PDF

lOMoARcPSD\|47827816 [Colligative Reviewer](https://www.studocu.com/ph/document/universidad-de-manila/chemistry/colligative-reviewer/73722759?utm_campaign=shared-document&utm_source=studocu-document&utm_medium=social_sharing&utm_content=colligative-reviewer) [Chemistry (Universidad de Manila)](htt...

lOMoARcPSD\|47827816 [Colligative Reviewer](https://www.studocu.com/ph/document/universidad-de-manila/chemistry/colligative-reviewer/73722759?utm_campaign=shared-document&utm_source=studocu-document&utm_medium=social_sharing&utm_content=colligative-reviewer) [Chemistry (Universidad de Manila)](https://www.studocu.com/ph/course/universidad-de-manila/chemistry/6489003?utm_campaign=shared-document&utm_source=studocu-document&utm_medium=social_sharing&utm_content=colligative-reviewer) Scan to open on Studocu Studocu is not sponsored or endorsed by any college or university **Colligative Property -** This is defined as the properties that depend only on the number of solute particles in solution and not on the nature of the solute particles. - **Electrolyte Solution** - contains solutes that dissociate into ions when dissolved and are able to conduct electricity. - **Non-electrolyte Solution** - contains solutes that do not dissociate into ions when dissolved and therefore do not conduct electricity. The **larger the number of molecules** of dissolved particles contained in a solution, the **greater its impact on the colligative properties.** **Vapor Pressure Reduction** - Adding a nonvolatile solute to a solvent lowers the solvent\'s vapor pressure. - fewer solvent particles escape into the gas phase, and so the vapor pressure is lowered. The higher the concentration of solute particles, the less solvent is at the interface and the lower the vapor pressure. **Volatile** -A volatile substance is one that readily evaporates or sublimates at room temperature or below. **Non-volatile** - A non-volatile substance refers to a substance that does not readily evaporate into gas under existing conditions. - A solute that is nonvolatile (does not have a measurable vapor pressure), the vapor pressure of its solution is always less than that of the pure solvent. **Raoult's law** - states that the vapor pressure of a solvent above a solution is equal to the vapor pressure of the pure solvent at the same temperature scaled by the mole fraction of the solvent present.  **Boiling Point Elevation** - When a non-volatile solute lowers the vapor pressure of a solvent, the boiling point is also affected. - Boiling point elevation refers to the increase in the boiling point of a solvent upon the addition of a solute. When a non-volatile solute is added to a solvent, the resulting solution has a higher boiling point than that of the pure solvent. The temperature difference between a **solution\'s boiling point** and **a pure solvents boiling point** is called the **boiling point elevation.** The boiling point of elevation of a solution is **directly proportional** to the number of solute particles. **Formula:** **Freezing Point Depression** - a lower vapor pressure of a solution compared to that of a pure solvent affects the freezing point of a solution. - The freezing point depression is one of the colligative properties that is the difference in the freezing points of the solution from the pure solvent. As solute is added to a solvent, the freezing point of the solution will be lowered than the freezing point of the pure solvent (without the solute). The amount of change in the freezing point is related to the number of particles of solute in a solution and is not related to the chemical composition of the solute. The freezing point of a solution is **directly proportional** to the molal concentration of the solution. Formula:  **Osmotic Pressure** - Osmosis is the diffusion of a solvent through a semipermeable membrane. - The pressure difference at equilibrium is called the **osmotic pressure**. - The amount of additional pressure caused by water molecules that moved into the concentrated solution. The osmotic pressure of a solution is **proportional** to the number of solute particles in a given volume of solution or molarity. The **hypertonic solution** is the opposite of a hypotonic solution, where there is more solute outside the cell than inside it. In this type of solution, more solvent will exit the cell than enter it in order to lower the concentration of solute outside the cell thus the cell shrinks due to the loss of water (water moves from a higher concentration inside the cell to a lower concentration outside). On the other hand, the **isotonic solution** has the same concentration of solutes both inside and outside of the cell. Under these conditions, there is no net movement of solvent; in this case, the amount of water entering and exiting the cell's membrane is equal. While the **hypotonic solution** there is a higher concentration of solutes inside the cell than outside the cell. When this occurs, more solvent will enter the cell than leave it to balance out the concentration of solute.