ACID_BASE_TITRATION In Chemistry and calculation .ppt
- 2. Titration • a method of analysis that will allow you to determine the precise endpoint of a reaction and therefore the precise quantity of reactant in the titration flask. • A buret is used to deliver the second reactant to the flask. • An indicator or pH Meter is used to detect the endpoint of the reaction.
- 3. Doing a Titration • Begin by preparing your buret by 1. washing with soap and water 2. rinsing with tap and then distilled water 3. and rinsing with the titrant solution • You should check for air bubbles and leaks, before proceeding with the titration. • Be sure the tip of the buret is filled. • Never dispense so that liquid is below the last calibration that you can read.
- 4. • Take an initial volume reading and record it. • Before beginning a titration, you should always calculate the expected endpoint volume.
- 5. • Prepare the solution to be analyzed by placing it in a clean Erlenmeyer flask or beaker. • If your sample is a solid, make sure it is completely dissolved. • Add indicator.
- 6. • Use the buret to deliver a stream of titrant to within a couple of mL of your expected endpoint. • You will see the indicator change color when the titrant hits the solution in the flask, but the color change disappears upon stirring.
- 7. • Approach the endpoint more slowly and watch the color of your flask carefully. • Use a wash bottle to rinse the sides of the flask and the tip of the buret, to be sure all titrant is mixed in the flask. • Make sure you know what the endpoint should look like. • For phenolphthalein, the endpoint is the first permanent pale pink. • The pale pink fades in 10 to 20 minutes.
- 8. • • If you think you might have reached the endpoint, you can record the volume reading and add another partial drop. • Sometimes it is easier to tell when you have gone past the endpoint. • If the flask looks like this, you have gone too far!
- 9. Acid-Base Indicators • An acid-base indicator is a weak acid or a weak base. • The undissociated form of the indicator is a different color than the original form of the indicator. • An Indicator does not change color from pure acid to pure alkaline at specific hydrogen ion concentration, but rather, color change occurs over a range of hydrogen ion concentrations. • This range is termed the color change interval. It is expressed as a pH range.
- 10. Litmus • Litmus is a weak acid. It has a seriously complicated molecule which we will simplify to HLit. The "H" is the proton which can be given away to something else. The "Lit" is the rest of the weak acid molecule. • There will be an equilibrium established when this acid dissolves in water. Taking the simplified version of this equilibrium: • The un-ionized litmus is red, whereas the ion is blue.
- 11. End Point of an Indicator • should not be confused with the equivalence point of a titration • indicator changes color at its endpoint • equivalence point is the stoichiometric point where neutralization takes place • ideally, the end point of the indicator and the stoichiometric equivalence point should coincide
- 13. Titration curves for strong acid vs. strong base Running acid into the base Running base into the acid
- 14. Titration curves for strong acid vs. weak base Running acid into the base Running base into the acid
- 15. Titration curves for weak acid vs. strong base Running acid into the base Running base into the acid
- 16. Acidic, Basic, and Neutral Salts • A salt is formed between the reaction of an acid and a base. • Usually, a neutral salt is formed when a strong acid and a strong base is neutralized in the reaction: H+ + OH- => H2O • When weak acids and bases react, the relative strength of the conjugated acid-base pair in the salt determines the pH of its solutions. • The salt, or its solution, so formed can be acidic, neutral or basic.
- 17. • A salt formed between a strong acid and a weak base is an acid salt, for example NH4Cl. • A salt formed between a weak acid and a strong base is a basic salt, for example CH3COONa. • These salts are acidic or basic due to their acidic or basic ions as shown in the tables here.
- 18. Ions of Neutral Salts: pH = 7 Cations Anions Na+ Mg2+ Cl- ClO4 - K+ Ca2+ Br- BrO4 - Rb+ Sr2+ I- ClO3 - Cs+ Ba2+ NO3 -
- 19. Acidic salts: pH < 7 Acidic Ions Transition metal ions NH4 + Fe2+ Al3+ Cu2+ HSO4 - Pb2+ H2PO4 - Sn2+