3.7 Solutions and Mixtures

Solutions come in the form of:

Solids, liquids, and gases

Do macroscopic properties of solutions vary?

No

Why do macroscopic properties of solutions not vary?

Solution composition is uniform throughout

For liquid solutions, the solute may be:

A gas, a liquid, or a solid

Are there different methods for describing solution concentration?

Yes

Most common concentration measure used in the laboratory:

Molarity

Equation for molarity:

M=n/L (M=molarity, n=moles of solute, L=liters of total solution)

Properties of liquid solutions:

The components cannot be separated by using filtering, there are no components large enough to scatter visible light, the components can be separated using processes that are a result of the intermolecular interactions between and among the components

The fact that in liquid solutions, there are no components large enough to scatter visible light is based on:

Tyndall Effect

Examples of processes used to separate components of liquid solutions:

Distillation, chromatography

What happens when ionic compounds form solutions?

Dissociate into ions

The concentration of the ions found in a solution of a given concentration may be / may not be the same as the original solution.

May not be

Why may the concentration of the ions found in a solution of a given concentration not be the same as the original solution?

Ionic compounds dissociate into ions when they form solutions

Example of how the concentration of ions found in a solution of a given concentration may not be the same as the original solution:

While 1 mole of sodium chloride, NaCl will dissolve in water to form 1 mole of sodium ions, Na+ and 1 mole of chloride ions, Cl1-, one mole of calcium chloride will dissolve in water to form one mole of calcium ions, Ca2+ and two moles of chloride ion, Cl1-. Because of this a 1 molar solution of calcium chloride will contain 1 mole of calcium ions but two moles of chloride ions, therefore the chloride ions will have twice the molarity of the solution.