Testing the Accuracy of Solution Titration

Abstract\nThe purpose of this key is to find out parsimony of the saltlike effect by titrating measured volume with a strong base of cognise concentration. The experiment was carried out it a science lab and from the results we run aground that the unexplored concentration was 0.2688172043 gram moleecule/dm3. My results showed that the concentration was higher than it should shake off been; the correct concentration was 0.2 mol/dm3. We also found anomalies in our results; this could be due that the detail that we were unfamiliar with testing the trueness of a standard solution.\n\n installation\nThe goal of this experiment is to check off how to mighty standardize an alkaline solution of which we do non know the exact concentration. A secondary goal is to properly give away how to titrate a solution.\nI hypothesize that by titrating the unknown solution with a standardized titrant, one deal therefore use the entropy gathered by this to learn exactly how much titrant was needful to reach equilibrium, and many moles of the titrant were compulsory to completely react with the solution of unknown concentration. By victorious the stoichiometric ratios of these compounds into account, we can then calculate the concentration of the unknown solution by using the formula:\nMaterials and Methods\nThe materials used in the titration are as followed:\n buret\nWhite tile (used to observe a colour win over in the solution)\nPipette\npH indicator (methyl orange)\nConical flask\nTitrant (sodium carbonate)\nAnalyte (the solution of unknown concentration)\n\nTitration result\nFirstly I rinsed the burette, the pipette and the conic flask with distilled water.\n because I fit(p) an accurately measured volume of the analyte into the conical flask using the pipette, on with a few drops of methyl orange. Then I placed the standardized solution into the burette, and destine its initial volume in a lab notebook. At this stage, ...