Chemistry: Mixtures and Solutions Flashcards

This set of vocabulary flashcards covers mixtures, types of solutions, concentration units like molality, solubility laws, colligative properties, and equilibrium concepts based on the provided chemistry notes.

Effect of Non-volatile Solutes

When a non-volatile substance is added to a pure liquid, the boiling point rises and the freezing point falls.

Osmosis

The diffusion of a solvent from a lower concentration solution to a higher concentration solution through a semipermeable membrane.

Boiling Point Elevation

The difference between the boiling point of a solution and the boiling point of the pure solvent.

Boiling

The process that occurs when the vapor pressure of a liquid equals the surrounding atmospheric pressure.

Boiling Point at High Altitudes

The boiling point of water decreases at high altitudes because the atmospheric pressure is lower.

Salting Roads in Winter

Adding salt to ice on roads lowers the freezing point of the ice, causing it to melt.

Gas-Liquid Solution Example

Adding ammonia gas ($NH_3$) to water is considered a gas-liquid solution.

Steel

A homogeneous mixture categorized as a solid-solid solution or alloy.

Molality ($m$)

The ratio of moles of solute to one kilogram of solvent ($mol/1000\,g$ or $mol/kg$).

Solvation

The process of surrounding solute particles with solvent particles.

Factors Increasing Dissolution Speed

Agitating (stirring) the solution, increasing the surface area of the solute, and raising the temperature of the solvent.

Henry's Law

States that at a constant temperature, the solubility of a gas in a liquid is directly proportional to the pressure of the gas above the liquid.

Gas Solubility Factors

The solubility of a gas in a liquid increases with an increase in pressure and a decrease in temperature.

Colligative Properties

Properties that depend on the number of solute particles in a solution, including vapor pressure lowering, boiling point elevation, freezing point depression, and osmotic pressure.

Common Ion Effect

The reduction in the solubility of a substance due to the presence of a common ion.

Ion Product ($Q_{sp}$) and Solubility Product ($K_{sp}$)

A precipitate forms when $Q_{sp} > K_{sp}$; no precipitate forms and the solution is unsaturated if $Q_{sp} < K_{sp}$.

Homogeneous Mixture

A mixture whose components are mixed uniformly and cannot be distinguished, such as sugar dissolved in water.

Suspension

A heterogeneous mixture containing particles that settle out over time, such as a mixture of water and sand or water and chalk.

Tyndall Effect

A phenomenon used to distinguish between homogeneous mixtures and heterogeneous mixtures (like colloids) by scattering light.