1. Neutralization Reactions Reaction that occurs between an acid and a base. Example: HCl + NaOH  NaCl + H 2 O & Water Products always include: A “Salt”

2. Neutralization Reactions Example: HCl + Mg(OH) 2  H2OH2O+ MgCl 2 2 2 Always H 2 O Then Mg +2 and Cl -1 (Ionic charges!)

3. Neutralization Reactions Example: If it takes 30.0 mL of 0.100 M NaOH to neutralize 25.0 mL of HCl, what was the pH of the HCl? HCl + NaOH  H 2 O + NaCl 1:1 mole ratio for HCl & NaOH

4. = 0.00300 mol NaOH 0.100 mol NaOH 0.0300 L 1.00 L 1:1 Ratio of NaOH & HCl… Then there is 0.00300 mol HCl too.

5. Since this is a strong acid which turns completely into [H 3 O + ]… pH = -log[0.120] moles Molarity = Liters = 0.00300 mol HCl 0.0250 L M = 0.120 mol/L = 0.921

6. Titrations Lab reaction where a known acid or base is added to an unknown acid or base to find the concentration (pH!) [http://upload.wikimedia.org/wikipedia/commons/6/69/Titration.gif]

7. Titrations Commonly, a known base is added to the burette. An unknown acid is added to flask with an indicator.

8. Titrations The base is added until the equivalence point is reached. Moles H 3 O + = Moles OH - [http://cwx.prenhall.com/petrucci/medialib/media_portfolio/text_images/FG18_09.JPG]