1. Solution and Acid/Base Review

2. pH Review 1.What does the pH of a solution measure? 2.What is the common pH scale based on? 3.Why is a pH of 7 considered neutral? 4.What is the pH of a 0.001 M HCl solution? 5.What is the hydrogen ion concentration of a solution that has a pH of 9? 6.What is the hydroxide ion concentration of a solution with a pH of 10? 7.What is the pH of a 0.001 M NaOH solution?

3. pH measures the acidity of a solution. H 2 O   H + + OH - K w = [H + ][OH - ] = 10 -14 pH = -log[H + ] pOH = -log[OH - ] pH + pOH =14

4. Titration Review 1.What is an acid/base titration used for? 2.What type of chemical reaction is involved? 3.Give a general equation for this type of reaction. 4.What is the name of equipment is used for a titration? 5.How will you determine the endpoint? 6.Write a balanced equation for the reaction of phosphoric acid (H 3 PO 4 ) with sodium hydroxide. 7.What is the concentration of a vinegar solution (acetic acid) if it takes 35.87 mL of a 0.23 M NaOH solution to neutralize 15.00 mL of the acid?

5. Acid Base Titrations A standard solution, of known concentration is added to a known volume of the solution of unknown concentration. A neutral endpoint is reached when an indicator changes color. The volume of the standard solution is then recorded. MaVa= MbVb

7. Solution and Molarity Review 1. What are the 2 parts of a solution? 2. What are some properties of a solution? 3.What do chemist use to measure solution concentration? 4.Define molarity. 5.What is the molarity of a solution made by dissolving 13.0 g NH3 in 100.0 mL of water? 6.How many grams of sodium chloride lwould be needed to make 150.0 mL of a 6.0 M solution? 7.What is the molarity of a solution made by dilution 13.0 mL of a 2.00 M HCl to a final volume of 300.0 mL?

8. Solutions A solution is a homogeneous mixture. That means it is made of two or more substances that are uniformly mixed. The solute is dissolved in the solvent. 1.Solutions are uniform, but the concentration can vary. 2.The solute is broken down into molecular size pieces. It can not be seen, and does not filter or settle out of the solution. 3.Solutions are a single phase. The solute will change to the phase of the solvent as it dissolves. Molarity M = Moles solute Liters of solution For dilution problems: M 1 V 1 = M 2 V 2