1. DE Chemistry – King William High School

2.  …are homogeneous mixtures  Solute (Kool-Aid) + solute (water)  “like dissolves like”…(polar dissolves polar & nonpolar dissolves nonpolar)  Why does oil not mix with water?

3.  Ionic solids break up into their ions in water through a process called hydration (water molecules surround them)  EX: NaCl  EX: CaCl 2

4.  Electrolytes dissociate in water and can produce an electric current  IONIC  Strong electrolytes completely dissociate  EX: MgSO 4  Weak electrolytes partially dissociate  EX: NH 4 OH

5.  Do NOT separate into ions in water and therefore do NOT conduct an electric current  COVALENT  EX: sugar (sucrose)

6.  Saturated solution - contains the maximum amount of solute that can dissolve in the solvent  Unsaturated solution – is dilute…can hold more solute

8.  The hotter a solution is…the more solute you can dissolve  Supersaturated solutions – contains more solute than its solubility allows

9.  The solubility of a gas in a liquid (CO 2 in your soda) is directly proportional to the pressure of the gas above the liquid  Why does your soda go “flat” after it has been opened?

10.  Page 294; Table 9.8  EX: K 2 S  EX: Ca(NO 3 ) 2  EX: PbCl 2  EX: AlPO 4

11.  Mass percent =  EX: What is the mass percent of NaOH in a solution prepared by dissolving 30.0 g NaOH in 120.0 g of water?

12.  M = mol/L  EX: What is the molarity of 60.0 g of NaOH in 250 mL of solution?

13.  MV = MV  What volume of 18.0 M HCl do you need to prepare 500 mL of 2.0 M HCl?

14.  Colloids – are homogenous mixtures where the particles are bigger than solute particles…and they do not “settle” out of solution  Colloid examples on page 305 – table 9.12  Suspensions – heterogeneous mixtures (their particles tend to “settle” out over time