This document defines key concepts related to solutions, including: - A solution is a homogeneous mixture of a solvent and one or more solutes. Common solvents are water. - The process of dissolving a solute involves the solute and solvent particles separating and the solvent surrounding and solvating the solute particles. This process can be endothermic or exothermic. - Solubility depends on properties of the solute and solvent as well as temperature and pressure. Solubility curves show how solubility changes with temperature. Saturation occurs when a solution contains the maximum amount of solute possible.

1. Solutions

2. What Is A Solution?
Recall that a solution is a homogeneous
mixture. (the same throughout)
Solvent – major component of a solution.
 Dissolves the solute(s). (Usually Water)
Solute(s) – minor component(s) of a solution.
 Active ingredients of a solution. (The salt in salt
water)
Solution = solvent + solute(s)

3. Some Common Solutions

4. The Solution Process
3 things happen when a solute dissolves:
1. Solute particles separate.
 This requires energy to overcome the
intermolecular forces holding them together.
2. Solvent molecules separate.
 This also requires energy.
3. Solvent particles surround solute particles.
 Known as “solvation”.
 Releases energy.

5. The Solution Process
1. Particles separate from
solute.
2. Solvent molecules move apart
to accommodate solute.
3. Solvation

6. Ions in Solution
Solvated
cation
Solvated
anion

7. The Solution Process

8. Energy Changes in Solutions
 The formation of a solution always involves a
temperature change.
 Can be a large or small temperature change.
 Can get warmer or cooler as solute dissolves.
 ∆H = enthalpy (heat) of solution
 Energy absorbed or released as a solute dissolves in
a solvent.
 +∆H = endothermic sol’n process.
 More heat absorbed than released.
 Temperature decreases as sol’n is formed.
 -∆H = exothermic sol’n process.
 More heat released than absorbed.
 Temperature increases as sol’n is formed.

9. Energy Changes in Solutions

10. Solubility
 Not all substances dissolve in water.
 Remember, “like dissolves like”.
 Polar solutes tend to dissolve more in polar solvents.
 Non-polar solutes tend to dissolve more in non-polar
solvents.
 Some (but not all) ionic compounds will dissolve
in water.
 Of those that do, temperature affects how much
they dissolve.
 Solids usually dissolve more in warm water.
 Gases usually dissolve more in cool water.

11. Solubility
 Insoluble – less than 0.1 grams of solute will dissolve in
100 grams of solvent.
 BaSO4 is insoluble in water.
 Only 0.0002448 grams of BaSO4 will dissolve in 100 grams of
water.
 Slightly soluble – 0.1 to 1 gram of solute will dissolve in
100 grams of solvent.
 Ag2SO4 is slightly soluble in water.
 About 0.8 grams of Ag2SO4 will dissolve in 100 grams of water
at 20ºC.
 Soluble – more than 1 gram of solute will dissolve in
100 grams of solvent.
 NaCl is soluble in water.
 35.9 grams of NaCl will dissolve in 100 grams of water at
20ºC.

12. Solubility Rules
Use your list of solubility rules to
determine whether each of the following
salts is soluble or insoluble in water.
NaCl
K2SO4
CaCO3
NH4NO3
Cu3(PO4)2
AgBr
NaCl is soluble.
K2SO4 is soluble.
CaCO3 is insoluble.
NH4NO3 is soluble.
Cu3(PO4)2 is insoluble.
AgBr is insoluble.

13. Saturation
 Saturated solution
 A sol’n containing the max. amt. of solute for a given amt. of
solvent at constant temp. and pressure.
 If additional solute is added it will not dissolve.
 Unsaturated solution
 A sol’n that does not contain the max. amt. of solute for a
given amt. of solvent.
 Additional solute can dissolve in an unsaturated solution.
 Supersaturated solution
 A sol’n that contains more solute than it can theoretically hold
at a given temperature.
 Addition of more solute causes the excess solute to precipitate.

14. Solubility Curves
Solubility curve chart – compares the
solubilities of several compounds in
water as a function of temperature.
Usually expresses solubility in terms of
grams of solute per 100 grams of water.

15. Solubility
Curves
 How many grams
of KNO3 can
dissolve in 100
grams of water at
30ºC?
 Answer: About
48 grams.

16. Solubility
Curves
 How many grams
of KClO3 can
dissolve in 100
grams of water at
55ºC?
 Answer: About
25 grams.

17. Solubility
Curves
 How many
grams of NH4Cl
can be
dissolved in
200 grams of
water at 40ºC?
 Answer: About
96 grams.

18. Solubility
Curves
 A saturated
solution of NaNO3
is prepared at
70ºC in 100
grams of water. If
the temperature is
lowered to 40ºC,
how many grams
of NaNO3 will
precipitate?
 Answer: About
30 grams will
precipitate out.

19. Solubility
Curves
 If 35 grams of
NH4Cl are
dissolved in 100
grams of water at
30ºC, is the
solution
unsaturated,
saturated, or
supersaturated?
 Answer: The
solution is
unsaturated.

20. Solubilities of Gases
 Henry’s Law – The solubility
of a gas in a liquid increases
as the pressure above the
liquid increases.
 Explains decompression
sickness (the “bends”).
 Nitrogen is forced to
dissolve in scuba divers’
blood by high pressure.
 If the diver ascends too
quickly, the nitrogen
bubbles come out of
solution and form painful
and possibly fatal gas
embolisms.