1. A homogeneous mixture containing a solute dissolved in a solvent.
Solutions
A homogeneous mixture containing a solute dissolved in a solvent.

2. Homogeneous mixtures Any two samples have the same composition
particles are SO SMALL
atoms, molecules, ions
THEY CAN’T BE SEEN & will pass through a filter
So how do you separate the components?

3. Two or more substances with different boiling points can be separated using fractional distillation (ex. Crude oil)

4. How do substances dissolve in each other?

5. When a non-polar, organic molecule dissolves it breaks apart into individual molecules. Called solvation, & forms a non-electrolytic solution.

6. Click
the
pic.

7. NaCl separates into ions (called ionization)
NaCl separates into ions (called ionization). When the water molecules surround the ions its called hydration & it forms an electrolytic solution.

8. How will these salts dissociate/ionize?
NaCl(s) 
Na+(aq) + Cl-(aq)
Na2SO4 (s) 
2Na+(aq) + SO42-(aq)
Pb(NO3)2 (s)
Pb2+(aq) + 2NO3-(aq)

9. Why are some ionization reactions endothermic and some exothermic????

10. Separate the solute into ions, atoms or molecules. +∆H
Forming a solution
Occurs in 3 steps
“Expand” the solvent
Overcome the IMF to make room for the solute. +∆H
“Expand” the solute
Separate the solute into ions, atoms or molecules. +∆H
Allow solvent and solute to COMBINE and form sol’n. -∆H
∆Hsol’n = ∆H1 + ∆H2 + ∆H3

11. Example: NaCl(s)  Na+(aq) + Cl-(aq)
∆H1 = +21kJ/mol REQUIRED to overcome Hydrogen bonding in H2O (IMF)
∆H2 = +786kJ/mol REQUIRED to separate the salt into ions
∆H3 = -783 kJ/mol IS RELEASED when ions and polar water molecules attract
∆Hsol’n = +24kJ/mol
This is an endothermic change….. Generally unfavorable in the universe. So….why does NaCl dissolve so readily?

12. Entropy

13. Types of Solutions Solid solutions a.k.a alloy Gas solutions
2 or more gases or vapors dissolved
ex. AIR
Solid solutions a.k.a alloy
copper + zinc = brass
copper + tin = bronze
Amalgam
An alloy made with mercury

14. Liquid solutions liquid, solid or gas dissolved in liquid
2 liquids that mix = miscible
2 liquids that don’t mix = immiscible
(aq) water is the solvent
tincture
alcohol is the solvent

15. water is
the universal solvent
because it dissolves
almost everything

16. Solubility Rules Like dissolves like polar dissolves polar
non-polar dissolves non-polar
Similar IMF will dissolve in each other

17. Oil and Water

18. The End