Chapter 4: Reactions in Solution— Aqueous Chemistry in Nature

Solution:

homogeneous mixtures of two or more substances

_{^{- can be a solid, liquid, or gas}}

Solute:

substance being dissolved; smaller amounts

_{^{- mixes with solvent so the solute and solvent have the same physical state}}

Solvent:

substance doing the dissolving; larger amounts

_{^{- Aqueous solutions: WATER is the solvent}}

Solubility

is the maximum amount of solute that dissolves in a specific amount of solvent

_{^{temperature dependent}}

Solubility formula

= g of solute/100 g water

Unsaturated solutions

contain less than the maximum amount of solute that can dissolve at that temperature. If more solute is added, it will dissolve in the solution.

Saturated solutions

contain less than the maximum amount of solute that can dissolve at that temperature. If more solute is added, it will dissolve in the solution.

Supersaturated solutions

contain more than the maximum quantity of solute predicted to be soluble in a given volume of solution at a given temperature.

The concentration of a solution is expressed as:

amount of solute/amount of solvent OR amount of solute/amount of solution

Parts per million (ppm):

1 mg solute/1 kg solution

Parts per billion (ppb):

1 mg solute/1 kg solution

Molarity

is a concentration unit used in chemistry

Molarity formula:

moles (n) of solute/volume (v) of solution in liters

M formula

= moles/L

moles formula

= L x M

L formula

moles/M