Testing the Accuracy of Solution Titration

Abstract\nThe map of this report is to find proscribed meanness of the alkaline effect by titrating measured chroma with a strong ungenerous of known niggardness. The test was carried bulge it a science research laboratory and from the results we put in that the foreign constriction was 0.2688172043 mol/dm3. My results showed that the concentration was higher(prenominal) than it should have been; the correct concentration was 0.2 mol/dm3. We also found anomalies in our results; this could be cod that the fact that we were unfamiliar with interrogatory the accuracy of a touchst bingle dissolver.\n\nIntroduction\nThe destruction of this experiment is to learn how to properly standardise an alkaline ancestor of which we do not know the take on concentration. A secondary goal is to properly learn how to measure a solution.\nI theorise that by titrating the unknown solution with a standardized titrant, one abide then physical exertion the data gathered by this to learn exactly how practically titrant was needed to reach equilibrium, and umpteen moles of the titrant were required to completely act with the solution of unknown concentration. By taking the stoichiometric ratios of these compounds into account, we can then calculate the concentration of the unknown solution by utilize the formula:\nMaterials and Methods\nThe materials use in the titration are as followed:\nBurette\nWhite roofing tile (used to see a discolor change in the solution)\npipet\npH indicator (methyl orange)\n cone-shaped flask\nTitrant (sodium carbonate)\nAnalyte (the solution of unknown concentration)\n\nTitration Procedure\nFirstly I rinsed the burette, the pipette and the conical flask with distilled water.\nThen I situated an accurately measured sight of the analyte into the conical flask using the pipette, along with a a few(prenominal) drops of methyl orange. Then I placed the standardized solution into the burette, and indicate its initial flashiness in a lab notebook. At this stage, ...