Solutions and Mixtures

Solution (Homogeneous Mixture)

A mixture whose macroscopic properties do not vary throughout the sample (uniform composition).

Heterogeneous Mixture

A mixture whose macroscopic properties depend on location in the mixture (non-uniform composition).

Molarity (M)

The most common concentration measure used in the laboratory, defined as moles of solute per liter of total solution.

Molarity Equation

M = nsolute/ Lsolution (n = moles solute; L = liters total solution).

Solubility and IMFs

Intermolecular forces influence the solubility and separation of mixtures (like dissolves like principle).

Properties of Liquid Solutions (Components)

Components cannot be separated by filtering; there are no components large enough to scatter visible light (Tyndall Effect).

Properties of Liquid Solutions (Separation)

Components are separated using processes that are a result of intermolecular interactions (distillation, chromatography, etc.).

Ion Concentration in Solutions

Ionic compounds dissociate into ions; the molarity of an individual ion in the solution may be a multiple of the solution's molarity based on the compound's formula (e.g., 1 M CaCl2 yields 1 M Ca2+ and 2 M C