1. Solution Preparation and Dilutions

2. Solution Preparation How do we create chemical solutions in a laboratory setting with a certain concentration/molarity? Obtain the mass of the chemical compound serving as solute Dissolve the solute in a small amount of the solvent Add enough solvent to reach the desired volume.

3. Example 1: Prepare a 6L solution of 4M NaCl

4. Example 2: Prepare a 250 ml solution of 0.05M HCl

5. Example 3: Prepare a 400 ml solution of 5M CuSO 4

6. Dilutions

7. What is a dilution? Taking a CONCENTRATED solution and making it LESS concentrated Adding more solvent to decrease the amount of solute in the solution M 1 V 1 = M 2 V 2 Used when 2 solutions are involved Units do not matter but keep the same units throughout the problem !!! Ex. Tea and sweetner

8. Example 1: Prepare 2.50L of a 0.360M H 2 SO 4 solution from a stock H 2 SO 4 solution of 18.0 M.

9. Example 2: A stock solution of KF has a concentration of 1.20M. To what final volume must 100ml of this solution be diluted to produce a 0.45 solution of KF?

10. Example 3: What volume of 17.4 M acetic acid is needed to prepare 1.00 L of 3.00 M acetic acid?

11. Serial Dilutions A type of dilution The dilution is made through a series of smaller dilutions from a stock or original solution Dilution factor Amount transferred/(amount transferred + amount of water) 1 ml of chemical solution into 9 ml of water is a 1/10 dilution factor. **How dilute is the resulting solution, multiply the dilution factors for each series.

13. Homework Read over lab procedure Complete solution preparation/dilution worksheet