1. mixture that is the same throughout....
Solutions

2. Solution composed of....
solvent-does the dissolving (usually water, the universal solvent on earth)-larger amount
solute-gets dissolved (salt, CO2)-smaller amount
Polar substances (ionic) will dissolve in water because water is polar.
Ocean is a solution
Soda is a solution

3. Solubility: How well the solute dissolves in the solvent
Can get more sugar to dissolve in tea by:
stirring
heating (hot tea dissolves more)
Increase surface area of solute
(sugar cube vs sugar granules)

4. Gases dissolved in water…
These are the opposite of trying to add sugar…
to get more CO2 dissolved you need to get the water
Colder
Don’t stir

5. Types of solutions:
Unsaturated: can dissolve MORE solute (can add more sugar and it will all dissolve).
Saturated: holding MAXIMUM amount of solute. If you add any more, the solute will settle at the bottom.
Supersaturated: heat a overly-saturated solution so all solute dissolves, then cool so it stays dissolved….Sweet tea, rock candy

6. Electrolyte: conducts electricity
Ionic Compounds are electrolytes because they dissociate (break apart) into + and – entities when aqueous.
Ex: NaCl in water becomes Na+ and Cl-
Remember: Nonpolar substances have an even spread of electrons and have no + and – ends.
How does this relate to sports and thunderstorms?

7. Hydrates: a compound that contains water
ex. CuSO4*5H2O
Efflorescent Hydrates--will lose waters to the atmosphere, high vapor pressure
e.g. Na2CO3*10H2O → Na2CO H2O
Hygroscopic Hydrates--will take waters from the atmosphere, low vapor pressure
e.g. CaCl2*H2O + H2O → CaCl2*2H2O

8. Deliquescent Compounds--like stronger hygroscopic hydrates, will take waters from the atmosphere, very low vapor pressure
Used to keep sensitive equipment dry
Do not touch with your hands
e.g. NaOH
or packets found in
shoe boxes and jerky packages

9. Notes Homework is 15.2 #8-15 (p457) And 16.1 #3-6 (p477)
sample problem 15.1 on page 456 will help with problem 15