1. Molar Concentration

2. Measuring Concentration Molarity (M): the number of moles of solute in 1 liter solution. Example: 0.5 moles of NaCl dissolved in 1 liter solution of water = = 0.5 M 0.5 moles 1 liter

3. If you have 3 L of water, how many moles of HCO 3 do you need to make a 0.6 M solution of HCO 3 ? Problem on your own:

4. Concentrated or Dilute? Concentrated means there are many solute particles in a solution. Dilute means there are relatively few solute particles in a solution.

5. Neutralization: The combining of an acid and a base in amounts that result in the elimination of all excess acid or base. M 1 V 1 = M 2 V 2 M 1 = solution 1 molarity V 1 = volume of solution 1 M 2 = solution 2 molarity V 2 = volume of solution 2

6. Neutralization: Problem: If you have 50 mL of 0.5 M acid. How much 0.25 M of a base do you need to add for neutralization to take place?

7. The math involved: M 1 V 1 = M 2 V 2 (0.5)(50mL) = (0.25)(V 2 ) 25 = (0.25)(V 2 ) = V 2 25 0.25 V 2 = 100mL

8. If you have 100 mL of 1.0 M acid, how much of 0.5 M of a base do you need to add for neutralization to take place? Problem on your own: