Abstract The purpose of this report is to find out concentration of the alkaline solution by titrating measured volume with a strong base of known concentration. The experiment was carried out it a science lab and from the results we found that the unknown concentration was 0.2688172043 mol/dm3. My results showed that the concentration was higher than it should have been; the correct concentration was 0.2 mol/dm3. We also found anomalies in our results; this could be due that the fact that we were unfamiliar with testing the accuracy of a standard solution. Introduction The goal of this experiment is to learn how to properly standardize an alkaline solution of which we do not know the exact concentration. A secondary goal is to properly learn how to titrate a solution. I hypothesize that by titrating the unknown solution with a standardized titrant, one can then use the data gathered by this to learn exactly how much titrant was needed to reach equilibrium, and many moles of the titrant were required to completely react 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 using the formula: Materials and Methods The materials used in the titration are as followed: Burette White tile (used to see a colour change in the solution) Pipette pH indicator (methyl orange) Conical flask Titrant (sodium carbonate) Analyte (the solution of unknown concentration) Titration Procedure Firstly I rinsed the burette, the pipette and the conical flask with distilled water. Then I placed 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 indicate its initial volume in a lab notebook. At this stage,