1. CONCENTRATION OF SOLUTIONS
A measure of the amount of solute in a given amount of solvent or solution
DILUTE
There is relatively small amount of solute in the solvent
CONCENTRATED
There is relatively large amount of solute in the solvent

2. MOLARITY The number of moles of solute in one liter of solution
mol / L
ALWAYS CONVERT volume of solution to LITERS
1.4 M means 1.4 moles of solute in 1.0 L of solution
Symbol = M
Example: M solution of X
Read as: a 0.34 molar solution of X

3. 1 M NaCl vs. 6 M NaCl

4. MOLARITY 1.4 M means 1.4 moles of solute in 1.0 L of solution
Molarity – M (mol/L)
Mass solute – g
Molar Mass solute (MM) – g/mol
Volume of solution – L

5. MOLARITY
What is the molarity of a solution composed of 5.85 moles of potassium iodide, KI, dissolved in enough water to make L of solution?
How many moles of H2SO4 are present in L of a M H2SO4 solution?
What volume of 3.00 M NaCl is needed for a reaction that requires 1.46 moles g of NaCl?

6. MOLARITY (Diluting a Solution)
Molarity – M
Volume of solution – L
Suppose you wished to make L of M silver nitrate by diluting a stock solution of M silver nitrate. How many millimeters of the stock solution would you need to use?
If mL of a 2.45 M stock solution of sodium hydroxide is diluted with water to make 168 mL of sodium hydroxide solution, what is the molarity of the final solution?

7. MOLARITY (Diluting a Solution)
3. How many liters of 3.0 M KOH can be obtained by diluting L of 8.0M of KOH?