Colligative Properties of Solutions

Front

Colligative Properties Noun

---

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

Back

Colligative Properties

---

Physical properties of solutions that are affected by the number of solute particles, not by their chemical identity.

---

Example: Adding a solute (like salt) to a solvent (like water) makes it harder for the solvent to evaporate, a change known as a colligative property.

Front

Solute Noun

---

[sol-yoot]

Back

Solute

---

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

---

Example: This diagram shows a solution, pointing to the solute (the white particles) that is dissolved in the solvent (the blue liquid) to form the mixture.

Front

Solvent Noun

---

[sol-vent]

Back

Solvent

---

The substance in which a solute is dissolved to form a solution, typically present in the largest amount.

---

Example: This diagram shows that in a solution, the solvent is the substance present in the largest amount that dissolves the other substance, the solute.

Front

Electrolyte Noun

---

[ih-lek-truh-lite]

Back

Electrolyte

---

A substance that dissociates or ionizes in a solvent to produce a solution that can conduct electric current.

---

Example: This image shows an ionic solid dissolving in water. The solid breaks apart into positive cations and negative anions, which become surrounded by water molecules.

Front

Nonelectrolyte Noun

---

[non-ih-lek-truh-lite]

Back

Nonelectrolyte

---

A substance that dissolves in a solvent but does not ionize, resulting in a solution that cannot conduct electricity.

---

Example: This diagram shows that a sugar solution does not conduct electricity, as the light bulb remains unlit, identifying sugar as a nonelectrolyte.

Front

Dissociate Verb

---

[dih-soh-shee-eyt]

Back

Dissociate

---

The process where an ionic compound separates into its constituent ions when dissolved in a suitable solvent.

---

Example: When an ionic solid is placed in water, the polar water molecules attract and pull apart the positive and negative ions, causing the solid to dissociate.

Front

Ionize Verb

---

[ahy-uh-nahyz]

Back

Ionize

---

The process where a molecular compound reacts with a solvent, such as water, to form ions in solution.

---

Example: This diagram shows hydrogen chloride (HCl) molecules breaking apart in water to form positively charged hydronium ions (H3O+) and negatively charged chloride ions (Cl-).

Front

Strong Electrolyte Noun

---

[strong ih-lek-truh-lite]

Back

Strong Electrolyte

---

An electrolyte that completely or almost completely dissociates or ionizes in a solution, producing many conductive ions.

---

Example: A strong electrolyte, like KCl, fully breaks apart into charged ions in a solution, allowing electricity to flow easily and light a bulb brightly.

Front

Weak Electrolyte Noun

---

[week ih-lek-truh-lite]

Back

Weak Electrolyte

---

An electrolyte that only partially dissociates or ionizes in a solution, producing only a few conductive ions.

---

Example: The image shows that in an acetic acid solution, only some molecules dissociate into ions, allowing a small electric current to flow and making the light bulb glow dimly.

Front

Molality Noun

---

[moh-lal-i-tee]

Back

Molality

---

A measure of solution concentration defined as the number of moles of solute per kilogram of the solvent.

---

Example: This image shows the mathematical formula for molality, which is calculated by dividing the moles of a solute by the kilograms of the solvent.