1. Solution Concentration  Concentration is a measure of how much solute is dissolved in a specific amount of solvent or solution  Molarity (M) = mol solute L solution

2. Molarity example #1 1. You have 0.8 L of a 0.5 M HCl solution. How many moles of HCl does this solution contain?

3. Molarity Example #1 2. How many moles of NaOH are contains in 65.0 mL of a 2.20 M solution of NaOH in water?

4. Heterogeneous Mixtures  Suspensions – a mixture containing particles that settle out if left undisturbed - Can separate them with filtration - The suspended particles are fairly large (compared to solute particles in a solution) ‏ (greater than 1000 nm) Ex. Sand in water 2) Colloids – a mixture with particles of intermediate size (between those of solution and suspension) ‏ (Between 1-1000 nm)

5. - Cannot separate by filtration - Tend to look cloudy - The particles are large enough to scatter light – called the Tyndall Effect Ex. Headlights in a fog, milk, gelatin - Suspensions can also show the Tyndall Effect, but solutions do not because the particles are not large enough to reflect light

6.  3) Solutions-  a. In a solution, the dissolved solute particles are so small that they cannot be seen. (Less than 1 nm in size)  b. They remain dissolved in the solution and will not settle out.  c. Even if you pour the solution through filter paper, both the solute and the solution will pass through the paper.  Ex. Salt Water