1. Chapter 11 Notes Solutions
Mixtures that are Homogenous. Same throughout. Will always be the same at top as bottom.
Suspensions are solutions that have large solutes that settle out over time. Ex. Dirt and water.
Colloids are solutions with large solutes but smaller than suspensions. They make the solution look cloudy and never settle out. Ex Fog
Solute gets dissolved (salt)
Solvent does dissolving (water)

2. Chapter 11 Solubility –How easily something dissolves.
Soluble – Easily dissolved
Insoluble – won't dissolve
Solubility is based on how much solvent you have, what that solvent is, temperature, etc.
Gases tend to decrease solubility with temp while solids tend to increase.

3. Chapter 11 Saturated, unsaturated, supersaturated
Saturated – holding as much solute as possible
Unsaturated – solvent can still hold more solute
Supersaturated – Solvent forced to hold more solute than it normally should (done with heat)

4. Chapter 11 Molarity = Moles Solute/Liters solvent
Higher Molarity the stronger/more concentrated the solution
Polarity – when a molecule doesn’t evenly share its electrons and you get a positive and negative end.
Like dissolves like – polar things dissolve other polar things and nonpolar dissolves nonpolar.

5. Chapter 11
Emulsifying agent – Substance that can be used to help like dissolve unlike (polar dissolve nonpolar). Ex Soap
Soap also acts as a surfactant which lowers surface tension.

6. Chapter 11 Ways to increase solubility:
a. Increase Temperature: solids and liquids will dissolve due to the collision theory faster at higher temperatures, gases however dissolve best at low temperatures.
b. Stirring: More collisions = faster dissolving
c. Increase Surface area: More contact between solute and solvent increases dissolving.

7. Chapter 11
Solubility Graph

8. Chapter 11
Solubility chart:

9. Chapter 11
Molarity Equation: Molarity (M) = moles of solute Liters of solvent *Remember if you have grams you must convert to moles first by dividing by Formula Mass