Testing the Accuracy of Solution Titration

Abstract\nThe purpose of this composing is to find out do exploitation of the alkalic antecedent 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 instal that the unappreciated concentration was 0.2688172043 breakwater/dm3. My results showed that the concentration was higher than it should stomach been; the correct concentration was 0.2 jetty/dm3. We also found anomalies in our results; this could be due that the concomitant that we were unfamiliar with testing the accuracy of a standard solution.\n\n accession\nThe goal of this experiment is to curb how to flop standardize an alkaline solution of which we do not know the exact concentration. A secondary goal is to properly swindle how to titrate a solution.\nI hypothesize that by titrating the unknown solution with a standardized titrant, one bathroom hence use the info gathered by this to learn exactly how much titrant was needful to reach equilibrium, and many moles of the titrant were inevitable to completely react with the solution of unknown concentration. By pickings 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:\nburette\nWhite tile (used to unwrap a colour smorgasbord in the solution)\nPipette\npH indicator (methyl orange)\nConical flaskful\nTitrant (sodium carbonate)\nAnalyte (the solution of unknown concentration)\n\nTitration force\nFirstly I rinsed the burette, the pipet and the conelike flask with distilled water.\n wherefore I set(p) an accurately measured volume of the analyte into the conical flask using the pipette, along with a few drops of methyl orange. Then I placed the standardized solution into the burette, and read its initial volume in a lab notebook. At this stage, ...