1. CP Chemistry
Chapter 14
Solutions Notes

2. Do you remember what a homogeneous mixture is?
Solutions
definition: homogeneous mixtures containing two or more substances
two components found in solutions:
solute = substance that gets dissolved; smallest part of solution
solvent = substance that does the dissolving; largest part of solution
So a solution is composed of two parts: solute + solvent

3. Examples of Solutions Not always made of 2 liquids
Solid in solid
Solid in liquid
Gas in liquid
Other examples?
Examples of Solutions
Not always made of 2 liquids
Can be any combination of solids, liquids, and gases
Examples: air, steel, metal alloys, ice tea, Crystal light, acids, soda

4. Can be any phase of matter
Soluble vs. Insoluble
Soluble = substance that can be dissolved in a solvent, ex. sugar and water
Insoluble = substance that can NOT be dissolved in solvent, ex. oil and water

5. Miscible vs. Immiscible
Two LIQUIDS!!
Miscible vs. Immiscible
miscible = two liquids that are soluble in each other, ex. alcohol and water
immiscible = two liquids that are NOT soluble in each other, ex. oil and water
Soluble = can be dissolved or mixed

6. Covalent don’t form charges
Solvation
process of solvent particles breaking apart solute ions/molecules by surrounding them
ionic substances – water molecules break crystal apart and separate compound into its cations and anions
covalent substances – water molecules interact with polar molecules and surround them
Cations = +
Anions = -
Covalent don’t form charges

7. Picture of Solvation animation of solvation

8. Electrolytes
Solutions that can conduct electricity due to ions in the solution
Ionic compounds become electrolytes, ex. NaCl
Covalent compounds can NOT become electrolytes, ex. sugar

9. Factors Affecting Solvation
To increase solvation – must increase the number of times the solute and solvent touch:
Shake (agitate) the mixture
Break to increase surface area
Bake – increase temperature

10. Solubility
definition: maximum amount of solute that will dissolve in a given amount of solvent at a specific temperature and pressure
three classifications:
unsaturated = contains less than maximum amount of dissolved solute
saturated = contains maximum amount of dissolved solute
supersaturated = contains more than maximum amount of dissolved solute

11. What happens if you add more solute to:
Unsaturated solution:
solute will dissolve
Saturated solution:
solute will not dissolve, will sink to bottom of container
Supersaturated solution:
solute will crystallize, will cause the extra solute to come out of solution

12. Solubility Curves
Graph showing how much of a substance will dissolve in 100 grams of water at various temperatures
Can use to determine if solutions will be unsaturated, saturated, or supersaturated

13. Saturation on a Solubility Curve
Unsaturated – point below solubility curve
Saturated – point on solubility curve
Supersaturated – point above solubility curve

14. Temperature and Solubility
Solid solutes
as temperature increases, solubility of the solid will increase
ex. best time to sweeten tea is when it is still hot from brewing, when cold sugar just goes to bottom of container
Gas solutes
as temperature decreases, solubility of a gas will decrease
ex. warm sodas produce more foam than cold sodas and go flat faster