Solubility is defined as the maximum amount of solute that can dissolve in a given amount of solvent at a specified temperature. There are two components of solubility - soluble substances that dissolve in solvents and insoluble substances that do not dissolve. Liquids can be miscible, meaning they mix to form a solution, or immiscible, meaning they do not mix. Solubility depends on overcoming attractions between particles so that solute particles can disperse uniformly among solvent particles. Solubility generally decreases with increasing temperature for solutions of gases in liquids.

1. SOLUBILITY

2. WHAT IS SOLUBILITY?
SOLUBILITY is defined
as the maximum
amount of solute that
dissolves in a given
amount of solvent at
specified
temperature.

3. TWO COMPONENTS OF SOLUBILITY
 SOLUBLE
 INSOLUBLE

4. TWO OTHERS TERMS DESCRIBE THE
SOLUBILITY OF A LIQUID TO ANOTHER
LIQUID
•MISCIBLE – Liquids
capable of mixing and
forming a solution.
•IMMISCIBLE- Those
that do not mix to form a
solution or are generally
insoluble in each other.

6.  When a solution forms, solute
particles ( molecules or ions) disperse
uniformly among solvent particles. For
uniform dispersal to take place,
attractions between solute-solute
particles and between solvent- solvent
particles must first be overcome.
 A rough rule of thumb is ‘’like
dissolves like’’ ‘’ Like’’ means similar in
polarity.

7.  POLARITY – is the
tendency to form
distinctive, opposing
charges based on
the orientation of
chemical bonds and
spatial structure of
the molecule

8. •For solutions of gas in liquid ,
the solubility decreases with
temperature.
• As the temperature increases,
the Solubility of the oxygen in
gas in the liquid water
decreases and therefore the
gas released.

9.  Small changes in pressure have little
effect on the solubility of solids in liquids
or of liquids in liquids, but a marked effect
on the solubility of gases in liquid.
 This was first shown by WILLIAM HENRY
( 1774-1836) AN English chemist and
physician. In 1830, he proved that the
solubility of a gas in liquid was directly
proportional to the partial pressure of the
gas above the liquid. This is known Henry’s
Laws.