1. Ch 12 Solutions 12.1 Types of Mixtures
Solutions are homogeneous mixtures
2 or + substances uniform throughout
Soluble: Capable of being dissolved
Solute: Being dissolved
Solvent: Doing the dissolving
Types of solutions
Can be solids (metal alloys), liquids (salt water), or gases (air)

2. Colloids Intermediate size between solution and suspension
1nm-100nm in diameter
Dispersion phase (particles) & dispersion medium (liquid)
Appears cloudy
Ex: emulsion (liquid in liquid), milk, fog, liquid aerosols

3. Tyndall Effect Light is scattered by particles of colloid
Figure 1.6
Tyndall Effect
Light is scattered by particles of colloid
Ex headlight scatter particles in fog
Brownian motion: motion due to collisions of rapidly moving particles in colloids

4. Separating Solutions, Colloids, and Suspensions
Shine light colloid vs solution
Settles out suspension

5. Electrolytes Nonelectrolytes Dissolves in water to make a solution
Conducts an electric current readily
Nonelectrolytes
Does not conduct an electric current

6. 12.2 The Solution Process Factors affecting dissolving
Increase the surface area: more surface area of solute in contact with solvent it dissolves faster
Agitating the solution: mixing/stirring puts more of surface of solute in contact with solvent
Heating the solvent: as temp increases the solvent molecules speed up/greater KE and more collisions

7. Supersaturated Solution
Solution Equilibrium
Physical state dissolution = crystallization rate
Saturated Solution
Max amount of dissolved solute
Unsaturated Solution
Less then max amount of dissolved solute
Supersaturated Solution
More dissolved solute then usual for given conditions

8. Solubility: “likes dissolve likes” Ionic compounds
Water is the solvent: hydration
Ionic substances form crystals with water: hydrate
CuSO4 . 5H2O

9. Nonpolar solutions Liquids
Ionic compounds not soluble in nonpolar solvent
Nonpolar solvent molecules not attract/cannot break bonds of ions holding crystal together
Liquids
Immiscible: liquids not soluble in each other
Miscible: liquids that dissolve freely in one another

10. Affects of Pressure Henry’s Law Pressure has little effect
Gas + solvent ↔ solution
Henry’s Law
Solubility of gas in liquid is directly proportional to partial pressure of the gas on the surface of liquid
Have constant temp
Effervescence: escape of gas from liquid, ex soda

11. Effects of Temperature
Increase temp decreases gas solubility
Increase temp increase liquid/solid solubility usually
Energy influence
Solvated: solute surrounded by solvent
Enthalpy of solution: E absorbed by heat of soln when solute dissolves in solvent

12. 12.3 Concentration of Solutions
Concentration: amount of solute in solvent
Molarity (M)
Number of moles in 1 L of solution

13. Molality (m)
number of moles in 1 kg of solution