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
1392g NaCl

4. Example 2:
Prepare a 250 ml solution of 0.05M HCl
0.45g HCl

5. Example 3:
Prepare a 400 ml solution of 5M CuSO4
320g CuSO4

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
M1V1 = M2V2
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 H2SO4 solution from a stock H2SO4 solution of 18.0 M.
50 ml of 18.0 M sulfuric acid

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?
0.267L, 267 ml

10. Example 3:
What volume of 17.4 M acetic acid is needed to prepare 1.00 L of 3.00 M acetic acid?
How much water would I need to add to 500ml of a 2.4M KCl solution to make a 1.0M solution?
0.172 L or 172 ml

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.