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GSp xƒџџџџџџџџџџџџџџџџџџџџџџџџ3Science F:Microsoft Office:Microsoft Word 6:NormalLAB: TITLE OF LABsciencescience'@ћќзН@LПвезН@hˆДчН@мЅhOР e!I=6ъ6о6оо6о6о6о6о64L7L7L7L7L7d7 n7L7h<V~7~7~7~7~7Д7Д7Д76: B<B<B<B<B<B<&О<X=3h<о6Д7~76Д7Д7Д7h<Д7о6о6~7~7Д7Д7Д7Д7о6~7о6~76:7 7,о6о6о6о6Д76:Д7‚Д7Lab: ACID/BASE TITRATIONS  Introduction A titration is a process used to determine the volume of a solution needed to react with a given amount of another substance. In this experiment, you will titrate hydrochloric acid solution, HCl,of unknown concentration, with a basic sodium hydroxide solution, NaOH, which you will have to prepare and standardize. You will monitor the titration using an electronic pH probe/computer setup. When HCl solution is the analyte, the pH of the solution is initially low. As base is added, the change in pH is quite gradual until you are close to the equivalence point, where the pH increases very rapidly. The change in pH then becomes more gradual again before leveling off with the addition of excess base. The region of rapid pH change, the equivalence point, is the most critical part of the titration. The volume of NaOH titrant used at the equivalence point will be used to determine the molarity of the HCl. The titration will be repeated, but with an unknown weak monoprotic acid as the analyte. You will want to compare the weak acid titration curve with the strong acid curve. From the titration curve for a weak acid you will be able to determine the molecular mass of the acid and the Ka. MATERIALS: potassium acid phthalate, KHC8H4O4 (KHP) solid sodium hydroxide hydrochloric acid, unknown concentration unknown weak acid standard buffer solutions 4 and 7 Vernier pH probe/MacIntosh computer set-up buret, ring stand, appropriate clamps beakers, erlenmeyer flasks, volumetric flasks Procedure 1. Prepare 500 mL of 0.1 M NaOH solution using solid NaOH, distilled water, and a volumetric flask. 2. Dry 2 - 3 g of KHP in the oven for 15 minutes. Cool covered if possible. 3. Weigh to the nearest 0.1 mg, 3 samples of KHP between 0.5 and 0.6 g and place the samples in erlenmeyer flasks. 4. Dilute each sample of KHP with 50 to 75 mL of distilled water and add 1 drop of phenolphalein. Swirl to mix and make sure the KHP is completely dissolved before proceeding. 5. Fill a buret with your NaOH solution and titrate each of the KHP samples. 6. Calculate the molarity of the NaOH solution. The results of the three calculations should be identical. You now have a standardized NaOH solution Store it in a brown bottle and label it. 7. Using a pipet and pipet pump, pipet 10 mL of the HCl into a 250 mL beaker..Place the beaker on a magnetic stirrer. Add 50 - 75 mL of distilled water to augment the volume. 8. Calibrate the pH probe according to the directions. Be sure to use the 4 buffer first. 9. Place the pH probe into the beaker. Be sure the magnetic stirrer does not hit the probe. Click the start button. Click the keep button . Enter the first volume reading into the computer as 0.00 mL. 10. Now begin your titration. Fill your buret to the 0.00 mL mark. Add an increment of NaOH titrant. When the pH stabilizes,again click the keep botton and enter the volume reading on the buret. Add smaller amounts of NaOH as you approach the inflection/equivalence point (0.1 -0.2 mL). Continue to add NaOH until the pH remains constant. 11. Recalibrate the axes if necessary. Print the graph and the data table. Clean up this portion of the lab. Rinse the probe in distilled water and store it in its keeping solution until you are ready to use it again. Determine the molarity of the HCl. 12. Prepare the unknown weak acid for titration. Measure out between 0.25 and 0.30 g of unknown weak acid. Add 50 to 75 mL of distilled water. Slight heating may be needed to effect solution. Cool the sample before proceeding with the titration. 13. Follow the same titration procedure used in the strong acid titration. 14. Determine the Ka and the molecular weight of the unknown weak acid. Data 1. Record all data for the standardization of NaOH. This includes the mass of NaOH used, the volume of the volumetric and the initial and final volumes of the three titrations. 2. The titration data for the strong and weak acids is recorded on the data tables printed from the computer. Calculations 1. Calculate the molarity of the standardized sodium hydroxide solution. 2. Calculate the molarity of the HCl. 3. Calculate the Ka and the molecular weight of the unknown weak acid. 4. Compare the two titrations. 5. Compare the accepted value for the Ka of this acid with the experimental value. 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