Sodium Carbonate Concentration By The Process Of Titration

carbonate was weighed accurately and dissolved in distilled water in a 250 mL volumetric flask. The solution was then made up to the mark with distilled water and mixed thoroughly. Titration Procedure A burette was filled with the standard sodium carbonate solution. Using a pipette, a measured volume of hydrochloric acid was transferred into a conical flask. A few drops of methyl orange indicator were added to the hydrochloric acid solution. The burette was then slowly titrated with the sodium carbonate solution until the endpoint was reached, which was indicated by a colour change from pink to yellow. The volume of sodium carbonate solution used was recorded. This process was repeated three times to obtain an average volume of sodium carbonate solution used. RESULTS The average volume of sodium carbonate solution used was 24.5 mL. CALCULATIONS The concentration of hydrochloric acid was calculated using the formula: Concentration of HCl = Concentration of Na2CO3 x Volume of Na2CO3 / Volume of HCl The concentration of sodium carbonate was 0.1 M. The volume of sodium carbonate used was 24.5 mL. The volume of hydrochloric acid used was 25 mL. Therefore, the concentration of hydrochloric acid was 0.098 M. CONCLUSION The concentration of hydrochloric acid was determined to be 0.098 M using the process

This produces a 0.1 M difference from the expected value of 1.0 M. The discrepancy between the expected and actual values could potentially be caused by a few errors or misconducts. In this case, the use of solid sodium carbonate could contribute to an error because of its hygroscopic nature, which means it absorbs moisture from its surroundings, increasing its weight and affecting the calculations. Additionally, the volume of hydrochloric acid used to neutralize the sodium carbonate could be incorrect due to the possibility of overshooting, where a drop of hydrochloric acid accidentally drips into the sodium hydroxide after the endpoint has already been achieved. The result could also be changed due to contamination of the beaker or flask because of a failure to thoroughly rinse them. Therefore, older excess solutions could potentially mix with the hydrochloric acid or sodium carbonate, changing the volume, concentration, or product.