Name_______________________________________ date__________________ period______
SOLUTIONS
1. Mixtures=2 or more substances together that retain their properties
Heterogeneous=not uniform throughout, not evenly mixed (suspensions)
Homogeneous=uniform, same composition throughout
(colloids, solutions)
2. Solutions=homogeneous mixture whose particles are molecules, ions, or atoms
3. Properties: Solutions=
1. Homogeneous
2. Will not separate
3. clear and transparent
4. Will not filter
5. Single phase
4. Parts:
solute= substance being dissolved/dissolved substance
solvent= substance in which solute dissolves
solubility= maximum amount of solute that will dissolve in a specific amount of solvent
at a specific temperature
soluble/insoluble= ability or inability of a solute to dissolve under specific conditions
miscible= 2 liquids that will dissolve in one another
5. Types
tinctures= solvent= alcohol
aqueous= solvent= water
hydration= solute particles surrounded by water molecules
dissociation= (+) and( –) ions separated in water by hydration
CaCl2 –> Ca+2 + 2Cl-
Na2SO4 –> 2Na+ + SO4-2
solid= rare as solvent, solutes usually solids or gases
alloys= one or more solids evenly mixed with a metal
amalgams= solvent= Hg
liquid= most common solvent, solutes=any phase
gas= solutes=other gases or vapors
6. Factors affecting solubility:
1. Nature of solvent and solutes(“like dissolves like”)
a) ionic and polar solutes dissolve in polar solvents
b) non-polar solutes dissolve in non-polar solvents
2. temperature - solid and liquid solutes= solubility increases with heat
- gas solutes = solubility decreases with heat
3. Pressure (gases only) -Henry’s Law= greater pressure increases solubility of gases
4. amount of substances already dissolved
7. Factors affecting rate of dissolving:
1. Size of solute particles
2. Stirring
3. Temperature of solvent
4. Amount already dissolved
8. Energy changes during dissolution: solid into liquid: (usually) requires energy(endothermic)
gases into liquid: releases energy(exothermic)
9. Characteristics describing solutions:
saturated=maximum amount dissolved solute@specific temp.
unsaturated=less than maximum
supersaturated= more than max. under normal conditions
dilute= relatively low amount solute
concentrated=relatively high amount solute
molarity(M)=moles solute per liter solution = moles solute =M, M=#moles , or
Liters solution
L
L=#moles , or , #moles=M X L
M
(Also) :Finding a new Volume or Molarity for a new solution made
from a solution of already known Molarity: M1 X V1=M2 X V2
molality(m)= moles solute
Kilogram solvent
10. Colligative properties= properties of a solvent affected only by amount of solute
1. Freezing point depression: solvent freezes @ lower temp. with more solute
-Tf = m X Kf
than normal freezing point
2. Boiling point elevation: solvent boils @ higher temp. with more solute
Tb = m X Kb
than normal boiling point