1. Solution Concentrations
Different ways of representing how much stuff is contained in a solution

2. Solution Components
Solution: a homogeneous mixture of two or more substances in a single phase
Atoms, molecules, or ions are thoroughly mixed so that the substance has a consistent composition and properties
Solute: The substance being dissolved
USUALLY the smaller amount
The particles of solute are so small that they can not be seen
Solvent: The substance doing the dissolving

3. Some Commonly Used Ways of Representing Concentration
Molality
Moles of solute per kilogram of solvent
Percent by Volume
Percent by Mass
Parts per Million
Parts per Billion
Parts per Trillion

4. Molarity
Number of moles of solute per liter of solution

5. Perform the following calculations…
What is the molarity of a solution prepared by dissolving g of potassium hydroxide to produce a mL solution?
What is the molarity of a mL solution that contains g of citric acid (C3H5O(COOH)3)?
How much sodium hydroxide would be needed to produce mL of a 6.00 M solution?
How many grams of K2Cr2O7 are needed to make mL of a 0.125M solution?

6. Preparing Solutions by Dilution
In many cases, solutions are sold in high concentrations and diluted with distilled water (or other solvents) to produce a solution with a desired concentration
Any ideas why?
When this is the case, the number of moles is the quantity that will determine the volumes needed…

7. Perform the following calculation
Calculate the amount of a 12.0 M hydrochloric acid solution (HCl) that is needed to produce mL of a 2.00 M HCl solution.
Determine the moles of solute required for the desired solution
Use the SAME NUMBER OF MOLES to calculate the volume of the concentrated solution that would provide this amount
Make up the volume difference with distilled water (or other specified solvent, if you are actually making the solution)

8. Perform the following calculations…
What volume of a 6.77 M nitric acid (HNO3) solution to produce a mL of a 1.50 M solution?
What is the molarity of a solution that is made by diluting ml of a 4.74 M HCl solution to mL?
How much final solution would be made by adding water to 1.19 mL of a 8.00 M acetic acid solution (CH3COOH) to produce a final molarity of 1.50 M?

9. Perform the following calculations…
What is the final molarity of an ammonium chloride solution produced by diluting mL of a 3.79 M solution to 2.00 L?
A 3.8 M solution of iron (II) sulfate is diluted to eight times its original volume. What is the new molarity of the solution?