1. Solution Chemistry

2. Solutions are special kinds of mixtures
Let’s review!!
Element – pure substance
homogeneous throughout
only one kind of matter present
Compound – pure substance
homogenous throughout
made from 2 or more elements
chemical in nature
Mixture – can be homogeneous or heterogeneous
made from 2 or more elements, compounds, or both
physical in nature

3. Because solutions are mixtures they have two parts:
solutes thing being dissolved
most often a solid, but can be any state
think: SODA
solvents thing doing the dissolving
most often a liquid – water for instance – but can be any state
think: our atmosphere – NITROGEN
Dissolving does not mean a change in state. Solutes do not melt! They remain a solid (if they are a solid to begin with)

4. The charge of the nucleus Is felt making it feel positive
Polarity – the uneven distribution of charges on a molecule
uneven distribution is a result of:
a. Sharing of electrons between atoms with different energy
1. Asymmetric molecules are polar
Electrons are very
Present on this side
Of the molecule
That makes this side
Or pole of the molecule
Feel negative
This side or pole of the
Molecule has no
Electrons present.
The charge of the nucleus
Is felt making it feel
positive
Hydrogen has one electron on the K shell
Fluorine has 9 electrons on the K and L shells. Fluorine is a larger atom with
More energy. F controls all of the electrons.

5. In the water molecule, hydrogen is a smaller atom with less energy
than oxygen.
When the electrons are share between these two atoms,
oxygen controls the electrons because it is an atom with more energy.
Because of this the molecule has two poles – one that feels positive
(hydrogen’s end) and the other that feels negative (oxygen’s end).

6. Molecules can also be nonpolar – an even distribution of charge on the molecule.
a. Sharing of electrons between atoms of equal energy
1. Diatoms
Here this diatom, electrons are on the same energy level. Electrons are on the same
energy shells and therefore are controlled equally by each atom. Electrons spin
equally around each nucleus.

7. 2. Symmetric molecules

8. Well how does all this connect with solutions
Well how does all this connect with solutions? The reason why solutes stay in solution
is because of polarity. Polar solutes dissolve most easily in polar solvents – water is polar
and so it can dissolve all polar molecules. Nonpolar solvents dissolve nonpolar solutes.
NaCl
Cl -
Cl -
Na +
Na +
Cl -
Cl -
Cl -
Na +
Na +
Na +
Cl -
Na +
Na +
Cl -
NaCl is an ionic compound
that is made up of + Na
ions and - Cl ions.
NaCl
When an ionic compound
dissolves in water it is
called DISSOCIATION.
Cl -
Cl -
Na +
Cl -
Na +
Na +
Na +
Na +
Cl -
Cl -
Cl -
Na +
Cl -
Cl -
Cl -
Cl -
Cl -
Na +
Cl -
Na +
Na +
Cl -
Na +

9. If a non polar molecule is put into water, it will NOT dissolve because of the like
Charges that will meet in the water and the solute.
CH4 is a symmetric
molecule that is
non polar. It will not
dissolve in water
because it will be repelled
by the positive pole of
the water molecule.

10. Solubility – the ability of a solvent to dissolve a solute.
Solubility will be affected by:
pressure
temperature
particle size – the smaller the particles of solute
the easier it will fit into the
spaces of the solvent.
stirring – moving the solute around pushes
particles into solution.
Affects molecular distance of solvent.
The larger the MD, the more solute that
can be dissolved, and vice versa.

11. Temperature:

13. Pressure:

14. There exists two types of solutions ( well there really are more
but that’s all we’re going to talk about)
Saturated Remember, solubility and therefore saturation is
b. Unsaturated dependent on temperature of solvent!!
**On solubility chart, saturation is marked anywhere on the graph
Line. Unsaturation is the area under the graph line.**

15. Concentration: the amount of solute dissolved in a GIVEN
amount of solvent.
Dilute – a little bit of solute in a specific amount of solvent.
Concentrated – a lot of solute in the SAME amount of
solvent.

16. Special solutions Suspensions Colloids Made of solute/solvent
Heterogeneous
Solute is suspended in the solvent for a period of time
Solute will eventually settle out of solution
Oil and vinegar
Chocolate milk
Sand and water
A special kind of suspension where the solute is held in the solvent for an extended time period.
Homogeneous
The use of an emulsifier is needed to keep the solute in suspension.
Mayonnaise
Whipped cream

17. Acid base comparison base acid
Any aqueous solution that releases Hydrogen ions in solution.
Generally, any compound that contains Hydrogen
Will react with metals to release Hydrogen gas.
Has a pH between 1 and 6.9
Tastes sour
Turns blue litmus red
Will react with a base to produce a salt + water
Any aqueous solution that releases hydroxyl ions (OH) in solution.
Generally, any compound that contains the OH ion.
Has a pH between 7 and 14
Tastes bitter
Feels slippery
Turns pink litmus blue.
Will react with an acid to product a salt + water.

18. Acid: hydrochloric acid – HCl stomach acid
sulfuric acid H2SO4 car battery acid
nitric acid HNO fertilizers
carbonic acid H2CO3 acid found in sodas
Bases: sodium hydroxide – NaOH Drano
human blood
potassium hydroxide – KOH soaps
calcium hydroxide – Ca(OH)2 hair relaxer, remover,
Ca supplement in baby food.
Neutralization reaction:
Acid + base = salt + water
HCl NaOH NaCl HOH
pH pH pH pH 7