1. Making Dilutions

2. Diluting a solution reduces the number of moles of solute per unit volume, but the total number of moles does not change. Higher molarity = more concentrated

3. Put in order from most dilute to most concentrated 6.0 M 0.05 M 1.05 1.5 M 5 x10 -3 M 3.5 M

4. http://phet.colorado.edu/en/simul ation/molarity

5. How can we change concentration? If we want to make 3.0 M hydrochloric acid, but we only have 6.0 M hydrochloric acid, what can we do?

6. Dilution Equation M 1 V 1 = M 2 V 2 Volumes can be in mL or L, but they must be the same on both sides. V is total volume of the solution, not the volume of water added!

7. Practice I have 20.0 mL of 2.00 M solution. I need to make 0.400 M solution. To what volume should I add? M 1 V 1 = M 2 V 2 (2.00 M)(20.0) = (0.400 M)V 2 V 2 = 100. mL

8. I have 0.25 L of 3.0 M HBr. How much water should be added to produce a 2.0 M solution? M 1 V 1 = M 2 V 2 (3.0 M)(0.25 L) = (2.0 M)V 2 V 2 = 0.375 L V is total volume. I already have 0.25 L of HBr, 0.375 - 0.25 = 0.125 So I should add 0.13 L of water