2.  Homogeneous mixtures  Can be solid, liquid or gas  Aqueous solution Water that contains dissolved substances

3. SOLVENTSOLUTE  The dissolving medium Water Gasoline Non-polar molecules will dissolve in other non-polar molecules!  Dissolved particles Salt, sugar Oil, grease Remember: only the surface area of a solute can be dissolved!

4.  Water is in constant motion (kinetic energy) water molecules collide with solute molecules  Water is polar It is slightly + & - Attracted to ions SOLVATION – water surrounds each charged ion

5.  Stirring (agitation) ↑ time b/c fresh solvent is brought in contact with the solute Only affects rate, not amt of solute that will dissolve  Temperature ↑ temp ↑ time b/c it increases the kinetic energy of the solvent, which causes more collisions with the solute.  Surface Area ↑ surface area ↑ time b/c more solute is exposed to the solvent

6.  The amt of solute that dissolves in a given amt of solvent at a specific temp & pressure to make a saturated solution (g solute/100g solvent) contains the max amt of solute! If more solute is added it will NOT dissolve Unsaturated – doesn’t have all the solute that it can dissolve

7. TEMPERATUREPRESSURE  Affects solids, liquids & gas  Usually solubility ↑ as the temp ↑  Affects gases the most!  Solubility ↑ as pressure ↑  HENRY’S LAW Solubility (S) is directly proportional to the pressure (P) S 1 = P 1 S 2 P 2

8.  Number of moles of a solute dissolved in 1 liter of solution  Dilute – small amt of solute  Concentrated – large amt of solute

9.  IV saline solutions contain 0.90g NaCl in 100mL of solution. What is the molarity?

10.  Reduces the number of moles of solute per unit volume  The total # of moles doesn’t change!  M 1 V 1 = M 2 V 2

11.  How many milliliters of aqueous 2.0M MgSO 4 solution must be diluted with water to prepare 100mL of aqueous 0.40M MgSO 4 ?