1. Titration

2. Definition Process used to determine the strength of an unknown acid or base Can determine the unknown acid by adding to it a base of known strength until it is neutralized Will know when it is neutral by using an indicator

3. Indicators pH sensitive dye

4. Transition Interval Range over which an indicator changes color Some change at pH’s of around 7 - great for showing neutralization Some change at pH’s lower than 7 - show strong acids Some change at pH’s higher than 7 - show strong bases

7. Equivalence Point Point at which the solutions are present in equal amounts See the equivalence point with indicators If the acid and base are both strong, the equivalence pt is at a pH of 7 If the acid is strong and the base is weak, the equivalence pt is lower than 7 pH If the acid is weak and the base is strong, the equivalence pt is higher than 7 pH

9. Problem If you have.05L of HCl at an unknown concentration and you add to it.025L of a.10M NaOH base, an indicator shows that it has reached neutralization. What is the molarity of the acid? Step 1: Find the moles of the known Step 2: Write the balanced equation Step 3: Use mole ratio to find moles of the unknown Step 4: Determine M of unknown

10. Practice 1) In a titration, 27.4ml of 0.0154M Ba(OH) 2 is added to a 20.0ml sample of HCl solution of unknown concentration. What is the molarity of the acid solution? 2) By titration, 17.6mL of H 2 SO 4 neutralized 27.4mL of LiOH solution. What is the molarity of the acid?