Chapter 13: Properties of Solutions Vocabulary

Vocabulary flashcards covering key terms, definitions, formulas, and concepts from Chapter 13: Properties of Solutions.

Solution

A homogeneous mixture of two or more pure substances in which the solute is dispersed uniformly throughout the solvent.

Entropy

A thermodynamic quantity that measures randomness or disorder, the increase of which favors the spontaneous formation of solutions.

Solvation

The interaction between solute and solvent molecules that allows a solid to dissolve; called hydration when water ($H_2O$) is the solvent.

Saturated Solution

A solution that is in dynamic equilibrium with undissolved solute, containing the maximum amount of solute that can dissolve at a given temperature.

Unsaturated Solution

A solution containing less solute than the maximum capacity that can dissolve in the solvent at a given temperature.

Supersaturated Solution

An unstable solution that holds more dissolved solute than is normally possible at a given temperature.

Solubility

The maximum amount of solute that can dissolve in a given amount of solvent at a specific temperature.

Miscible

A term describing liquids that are able to dissolve and mix completely with one another in all proportions.

Immiscible

A term describing liquids that do not dissolve or mix in one another, such as nonpolar hexane and polar water ($H_2O$).

Henry's Law

A gas law stating that the solubility of a gas in a liquid is directly proportional to the partial pressure of that gas above the solution.

Mass Percentage

A unit of concentration calculated as $\text{Mass \% of component} = \frac{\text{mass of component in soln}}{\text{total mass of soln}} \times 100$.

Parts per Million (ppm)

A unit of concentration used for trace amounts, calculated as $\text{ppm of component} = \frac{\text{mass of component in soln}}{\text{total mass of soln}} \times 10^6$.

Mole Fraction ($\chi$)

A concentration unit defined as $\text{Mole fraction of component} = \frac{\text{moles of component}}{\text{total moles of all components}}$.

Molarity ($M$)

A concentration unit defined as $\text{Molarity} = \frac{\text{moles of solute}}{\text{liters of soln}}$, which varies with temperature due to volume expansion or contraction.

Molality ($m$)

A concentration unit defined as $\text{Molality} = \frac{\text{moles of solute}}{\text{kilograms of solvent}}$, which remains constant regardless of temperature changes.

Colligative Properties

Physical properties of solutions that depend solely on the quantity or concentration of solute particles, not on their chemical identity.

Raoult's Law

A principle stating that the vapor pressure of a volatile solvent over a solution is equal to the mole fraction of the solvent multiplied by the vapor pressure of the pure solvent.

van 't Hoff Factor ($i$)

The number of discrete particles into which a formula unit of a solute dissociates when dissolved in a solvent.

Osmosis

The net movement of solvent molecules across a semipermeable membrane from a solution of lower solute concentration to one of higher solute concentration.

Osmotic Pressure ($\Pi$)

The external pressure required to prevent the net movement of solvent across a semipermeable membrane, given by $\Pi = iMRT$.

Isotonic Solution

A solution having the same osmotic pressure as another solution, resulting in equal rates of solvent movement across a semipermeable membrane in both directions.

Hypotonic Solution

A solution with a lower osmotic pressure than another solution, causing solvent to leave it at a higher rate than it enters.

Hypertonic Solution

A solution with a higher osmotic pressure than another solution, causing solvent to enter it at a higher rate than it leaves.

Crenation

The shrinking of a red blood cell caused by the net loss of water when placed in a hypertonic environment.

Hemolysis

The swelling and eventual bursting of a red blood cell caused by the net influx of water when placed in a hypotonic environment.

Colloid

A mixture containing dispersed particles that are larger than individual ions or molecules, but small enough that gravity does not cause them to settle out.

Emulsifier

A substance that enables nonpolar substances to disperse and dissolve in a polar solvent by stabilizing a colloidal suspension.