Colligative Properties

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Colligative Properties Noun

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[kuh-lig-uh-tiv prop-er-teez]

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Colligative Properties

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Properties of a solution determined by the number of solute particles present, rather than their specific chemical identity.

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Example: This image shows a solution, which consists of solute particles dissolved in a solvent. Colligative properties are determined by the concentration of these solute particles.

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Solute Noun

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[sol-yoot]

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Solute

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A substance that is dissolved in another substance, known as the solvent, to form a complete solution.

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Example: This diagram shows that a solute (pink particles) is the substance that dissolves in a solvent (blue particles) to create a solution.

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Solvent Noun

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[sol-vent]

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Solvent

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A substance that dissolves a solute, resulting in a solution, and is typically the component present in the greatest amount.

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Example: This diagram identifies water as the solvent, the liquid component that dissolves the solute (sugar) to create a solution.

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Vapor Pressure Lowering Noun

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[vay-per presh-er loh-er-ing]

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Vapor Pressure Lowering

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The colligative property defined as the reduction in the vapor pressure of a pure solvent when a non-volatile solute is added.

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Example: Adding a solute (like salt) to a solvent (like water) reduces the number of solvent particles escaping into vapor, which lowers the vapor pressure.

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Boiling Point Elevation Noun

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[boil-ing point el-uh-vay-shun]

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Boiling Point Elevation

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The phenomenon where the boiling point of a liquid solvent increases upon the addition of a non-volatile solute.

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Example: Adding a solute, like salt, to a solvent, like water, increases the temperature at which the solution boils compared to the pure solvent.

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Freezing Point Depression Noun

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[freez-ing point dih-presh-un]

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Freezing Point Depression

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The phenomenon where the freezing point of a liquid solvent decreases upon the addition of a solute.

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Example: Adding salt to icy roads lowers the freezing point of water, causing the ice to melt even when the temperature is below 0°C (32°F).

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van't Hoff Factor (i) Noun

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[vant hoff fak-ter]

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van't Hoff Factor (i)

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A measure representing the number of discrete particles that a solute formula unit forms when dissolved in a solvent.

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Example: This diagram shows an ionic solid dissolving in water. One unit breaks into multiple separate particles (ions), increasing the total number of particles in the solution.

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Electrolyte Noun

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[ih-lek-truh-lite]

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Electrolyte

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A substance that produces an electrically conductive solution by dissociating into ions when dissolved in a polar solvent.

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Example: This diagram shows that when salt (an electrolyte) dissolves in water, it breaks into charged ions that conduct electricity, unlike sugar (a non-electrolyte).

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Non-electrolyte Noun

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[non-ih-lek-truh-lite]

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Non-electrolyte

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A substance that does not produce ions when dissolved, resulting in a solution that does not conduct electricity.

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Example: A sugar solution is a non-electrolyte because it does not form ions in water, so it cannot conduct electricity to light the bulb.

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Dissociation Noun

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[dih-soh-see-ay-shun]

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Dissociation

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The process in which a compound or molecule breaks apart into smaller particles, such as atoms, ions, or radicals.

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Example: When an ionic compound like salt (NaCl) is put in water, the water molecules pull the positive (Na+) and negative (Cl-) ions apart, causing it to dissociate.